英文版化学实验报告

合集下载

化学震荡实验报告（完整版）

化学震荡实验报告（完整版）报告编号：YT-FS-5574-86化学震荡实验报告(完整版)After Completing The T ask According To The Original Plan, A Report Will Be Formed T o Reflect The Basic Situation Encountered, Reveal The Existing Problems And Put Forward Future Ideas.互惠互利共同繁荣Mutual Benefit And Common Prosperity化学震荡实验报告(完整版)备注：该报告书⽂本主要按照原定计划完成任务后形成报告，并反映遇到的基本情况、实际取得的成功和过程中取得的经验教训、揭露存在的问题以及提出今后设想。

⽂档可根据实际情况进⾏修改和使⽤。

化学振荡操作说明1. 根据需处理⼯件选⽤合适的磨料，投⼊研磨机，视⼯件的实际情况⼤⼩配好药剂PM600，并对⼯件进⾏清洗直⾄排⽔⼝流出清⽔为⽌。

2. 当排出之清⽔量⾄⼀根尾指粗细时，即关闭排⽔阀投⼊⽔及PM600⽐例 1:1，调⾼研磨频率进⾏研磨。

3. 当⼯件变灰⽩⾊时，对⼯件进⾏检测。

如⼯件表⾯情况不甚理想(纹路过深)对⼯件进⾏清洗，投⼊第⼆次PM600研磨⼯件⾄端⾯柱⾯光泽⼀⾄，⽆⽩雾雾及⿇点⿊斑的感觉。

4.研磨⼯件⾄理想效果后，对⼯件进⾏彻底清洗。

投⼊抛光剂及防锈剂进⾏抛光处理30min，抛光速度视⼯件⼤⼩及机台⼤⼩⽽定。

备注：1.选⽤磨料之原则：不堵塞⼯件及不扩孔为原则。

2.⼯件端⾯⼑痕过深时，退⾄车床组做端⾯研磨处理。

3.加⼊PM600切削⼀段时间后，若发现⽯头翻转过慢时或是⽯头过黏时，对研磨机内加⼊适量的⽔润滑。

4.⼤锅处理量为200~250kg，⼩锅处理量为50~80kg。

⼯件越长处理料越少。

5.每48hr打黄油⼀次，设备间隔使⽤每72hr打黄油⼀次。

化学实验报告全英

Experiment Title: Synthesis of Silver Nitrate from Silver and Nitric AcidDate: March 10, 2022Objective: The objective of this experiment was to synthesize silver nitrate (AgNO3) by reacting silver (Ag) with nitric acid (HNO3) and to observe the formation of the product.Materials:1. Silver (Ag) - 0.5 g2. Nitric acid (HNO3) - 10 mL3. Beaker4. Test tube5. Funnel6. Pipette7. Distilled water8. Sodium chloride (NaCl) - 0.5 g9. Ethanol (C2H5OH) - 10 mL10. Sodium chloride (NaCl) - 0.5 g11. Ethanol (C2H5OH) - 10 mL12. SpectrophotometerProcedure:1. Weigh 0.5 g of silver (Ag) using a balance and transfer it into a test tube.2. Add 10 mL of nitric acid (HNO3) to the test tube containing the silver (Ag).3. Swirl the test tube gently to ensure that the silver (Ag) reacts completely with the nitric acid (HNO3).4. Observe the reaction and note any changes in color or appearance.5. Once the reaction is complete, allow the mixture to cool to room temperature.6. Filter the mixture using a funnel and filter paper to separate the silver nitrate (AgNO3) from the remaining solution.7. Collect the silver nitrate (AgNO3) on a filter paper and dry it in an oven at 100°C for 1 hour.8. Dissolve 0.5 g of sodium chloride (NaCl) in 10 mL of ethanol (C2H5OH) and transfer it to a test tube.9. Add 10 mL of distilled water to the test tube containing the sodium chloride (NaCl) solution.10. Add a few drops of the silver nitrate (AgNO3) solution to the sodium chloride (NaCl) solution.11. Observe the formation of a white precipitate and note its color and appearance.12. Measure the absorbance of the silver nitrate (AgNO3) solution usinga spectrophotometer at a wavelength of 590 nm.Results:1. The reaction between silver (Ag) and nitric acid (HNO3) resulted in the formation of a colorless solution, indicating the successful synthesis of silver nitrate (AgNO3).2. The silver nitrate (AgNO3) was successfully separated from the remaining solution using filtration.3. The precipitate formed when silver nitrate (AgNO3) was added to the sodium chloride (NaCl) solution was white, confirming the presence of silver nitrate (AgNO3) in the reaction mixture.4. The absorbance of the silver nitrate (AgNO3) solution was measured using a spectrophotometer at a wavelength of 590 nm, and the value obtained was 0.6.Discussion:The synthesis of silver nitrate (AgNO3) from silver (Ag) and nitric acid (HNO3) was successful in this experiment. The reaction between silver (Ag) and nitric acid (HNO3) resulted in the formation of a colorless solution, which was consistent with the expected color of silver nitrate (AgNO3) solution. The precipitate formed when silver nitrate (AgNO3) was added to the sodium chloride (NaCl) solution was white, indicating the presence of silver nitrate (AgNO3) in the reaction mixture. The absorbance value obtained using a spectrophotometer confirmed the presence of silver nitrate (AgNO3) in the solution.Conclusion:In conclusion, the synthesis of silver nitrate (AgNO3) from silver (Ag) and nitric acid (HNO3) was successfully achieved in this experiment. The reaction resulted in the formation of a colorless solution, and the presence of silver nitrate (AgNO3) was confirmed through the formation of a white precipitate and the absorbance measurement using a spectrophotometer.。

化学实验报告英文版

化学实验报告英文版Chemical Experiment ReportAbstract:This report presents the findings and analysis of a chemical experiment conducted to investigate the effects of temperature on the rate of reaction between hydrochloric acid (HCl) and sodium thiosulfate (Na2S2O3). The experiment involved varying the temperature of the reactants and measuring the time taken for the reaction to occur. The results indicate a clear correlation between temperature and reaction rate, with higher temperatures leading to faster reactions.Introduction:Chemical reactions are influenced by various factors, including temperature, concentration, and catalysts. The purpose of this experiment was to examine the impact of temperature on the rate of a chemical reaction. The reaction between hydrochloric acid and sodium thiosulfate was chosen due to its well-documented reaction kinetics.Methodology:The experiment was conducted using a simple setup consisting of a conical flask, a stopwatch, and a thermometer. Initially, 50 mL of 1 M hydrochloric acid was poured into the flask, followed by the addition of 10 mL of 0.1 M sodium thiosulfate. The stopwatch was started as soon as the sodium thiosulfate was added, and the time was recorded when the solution turned opaque due to theformation of a yellow precipitate. The experiment was repeated at different temperatures by immersing the flask in water baths maintained at specific temperatures.Results and Discussion:The experiment was carried out at four different temperatures: 20°C, 30°C, 40°C, and 50°C. The average reaction times at each temperature were recorded and are presented in Table 1 below:Temperature (°C) Reaction Time (s)20 12030 9040 7050 50Table 1: Average reaction times at different temperaturesFrom the results, it is evident that as the temperature increased, the reaction time decreased. This indicates that higher temperatures accelerate the rate of the reaction between hydrochloric acid and sodium thiosulfate. The relationship between temperature and reaction rate can be explained by the collision theory. According to this theory, particles must collide with sufficient energy to overcome the activation energy barrier for a reaction to occur. As temperature increases, the average kinetic energy of the particles also increases, leading to more frequent and energetic collisions.Furthermore, the reaction between hydrochloric acid and sodium thiosulfate isexothermic, meaning it releases heat. As the reaction progresses, the released heat raises the temperature of the solution, further increasing the reaction rate. This positive feedback mechanism contributes to the observed trend of faster reactions at higher temperatures.Conclusion:In conclusion, this experiment demonstrates the significant influence of temperature on the rate of the reaction between hydrochloric acid and sodium thiosulfate. As temperature increases, the reaction time decreases due to more energetic collisions and the exothermic nature of the reaction. These findings have practical implications in various fields, such as industrial chemistry and environmental science, where controlling reaction rates is crucial.Further research could explore the effect of temperature on other chemical reactions and investigate the specific activation energy values for different reactants. Additionally, studying the impact of other factors, such as concentration and catalysts, on reaction rates would provide a comprehensive understanding of chemical kinetics.。

化学实验报告英语

化学实验报告英语Chemical Experiment ReportIntroductionChemical experiments play a crucial role in the field of science and technology. They provide valuable insights into the properties and behavior of various substances. In this report, we will discuss a series of chemical experiments that were conducted in a laboratory setting. The experiments aimed to explore the effects of different variables on the reaction rate and product formation. Experiment 1: Reaction Rate and ConcentrationIn this experiment, we investigated the relationship between reaction rate and concentration. We prepared a solution of hydrochloric acid and sodium thiosulfate. By varying the concentration of sodium thiosulfate and keeping the concentration of hydrochloric acid constant, we observed the time taken for the solution to turn cloudy. As expected, we found that a higher concentration of sodium thiosulfate resulted in a faster reaction rate. This experiment demonstrated the importance of concentration in determining the rate of a chemical reaction.Experiment 2: Temperature and Reaction RateTemperature is another crucial factor that influences reaction rates. To study this, we heated a solution of potassium permanganate and oxalic acid to different temperatures. We then measured the time taken for the solution to change color. The results showed that an increase in temperature led to a significantincrease in the reaction rate. This can be attributed to the fact that higher temperatures provide more energy to the reacting particles, increasing their collision frequency and the likelihood of successful collisions.Experiment 3: Catalysts and Reaction RateCatalysts are substances that can speed up a chemical reaction without being consumed in the process. In this experiment, we examined the effect of a catalyst on the decomposition of hydrogen peroxide. We added a small amount of manganese dioxide to a solution of hydrogen peroxide and observed the release of oxygen gas. The presence of the catalyst facilitated the decomposition of hydrogen peroxide, leading to a faster reaction rate. This experiment highlighted the role of catalysts in enhancing reaction rates and their importance in various industrial processes.Experiment 4: pH and Product FormationThe pH of a solution can significantly influence the formation of products in a chemical reaction. To investigate this, we conducted an experiment involving the reaction between acetic acid and sodium bicarbonate. We varied the pH of the acetic acid solution by adding different amounts of sodium hydroxide. We then measured the volume of carbon dioxide gas produced. The results indicated that a higher pH resulted in a greater volume of carbon dioxide gas. This experiment emphasized the impact of pH on the formation of products in chemical reactions.ConclusionChemical experiments provide valuable insights into the behavior and properties of substances. Through the experiments discussed in this report, we explored the effects of concentration, temperature, catalysts, and pH on reaction rates and product formation. These experiments demonstrate the importance of understanding the factors that influence chemical reactions and their applications in various fields, including pharmaceuticals, materials science, and environmental studies. By furthering our knowledge in this area, we can continue to make advancements in the field of chemistry and contribute to the development of new technologies.。

英文版化学实验报告

三、The Main reagentsandInstrument
Themain reagents：Cyclohexanol、Sodium chloride、Concentrated sulfuric acid、Anhydrous magnesium sulfate、Ethyl ether、Sodium dichromate
The last, the productas a colorlessoil,0.8 gofproduct wasobtained,andin the experiment,we can knowthe boiling pointof the product is154.1°C
There aretheoretical yield2.36 gproductexperimentwas0.8grams, sothere isa yieldof 34.8%
二、The experimental principle
The main reaction:
3 RCH2OH (环己醇）+ Cr2O72-+ 2 H+→ 3 RC=O +2Cr3++7H2O
The deputy reaction:
3 RCH2OH (环己醇）+H2Cr2O7+H2SO4→ 3 RCHO + Cr2(SO4)3+8H2O
Fractions of stratification, the upper is a colorless liquid, the lower is a colorless oily
3 gof theliquid wasevaporatedtoa saturatedsalt,aftertransferred to a separatoryfunnel andthe organiclayer wasseparated andallowed to standlayered,dried over anhydrous magnesiumsulfate.The liquidwas distilledafter drying, theproductweighed

化学实验报告常见英文

Experiment Title: Synthesis of Ethanol from EthanolamineDate: [Date]Objective:The objective of this experiment was to synthesize ethanol from ethanolamine using the dehydration reaction. Ethanolamine is a compound with the molecular formula NH2CH2CH2OH, and it can be dehydrated to produce ethanol (CH3CH2OH) and ammonia (NH3).Materials:- Ethanolamine (NH2CH2CH2OH)- Sulfuric acid (H2SO4)- Concentrated sulfuric acid- Ethanol- Sodium chloride (NaCl)- Distilled water- Sodium hydroxide (NaOH)- Sodium sulfate (Na2SO4)- Potassium permanganate (KMnO4)- Barium chloride (BaCl2)- Distillation apparatus- Reaction vessel- Round-bottom flask- Condenser- Thermometer- Test tubes- Pipettes- Weighing scale- Stirring rod- Safety goggles- Gloves- Lab coatProcedure:1. Measure 5 g of ethanolamine using a weighing scale and transfer it toa round-bottom flask.2. Add 5 mL of concentrated sulfuric acid to the flask and stir the mixture thoroughly.3. Place the flask in a water bath and heat it to 60°C for 2 hours. This will facilitate the dehydration reaction.4. After 2 hours, remove the flask from the water bath and allow it to cool to room temperature.5. Transfer the reaction mixture to a distillation apparatus. The distillation apparatus consists of a round-bottom flask, a condenser, and a receiving flask.6. Heat the mixture to approximately 78°C, which is the boiling point of ethanol. Ethanol will vaporize and be collected in the receiving flask.7. Collect the distillate and transfer it to a test tube. Add 5 mL of water to the test tube and observe the appearance of the liquid.8. To identify the presence of ammonia, add a few drops of potassium permanganate to the test tube. If the solution turns brown, it indicates the presence of ammonia.9. To confirm the purity of the ethanol, add a few drops of barium chloride to the test tube. If a white precipitate forms, it indicates the presence of sodium chloride, which was used as a catalyst in the reaction.10. Dispose of the waste products and clean the equipment.Results:- The reaction mixture was heated to 60°C for 2 hours, and the distillation was performed at approximately 78°C.- Ethanol was collected in the receiving flask, and the distillate was observed to be a clear liquid.- A brown color was observed in the test tube when potassium permanganate was added, indicating the presence of ammonia.- A white precipitate formed when barium chloride was added, indicating the presence of sodium chloride.Discussion:The dehydration reaction of ethanolamine to produce ethanol was successfully achieved in this experiment. The reaction mixture was heated to 60°C for 2 hours to facilitate the dehydration process. Ethanol was collected in the receiving flask, and the distillate was observed to be a clear liquid, indicating the successful synthesis of ethanol.The presence of ammonia was confirmed by the brown color observed when potassium permanganate was added. This suggests that the dehydration reaction also produced ammonia as a byproduct.The formation of a white precipitate when barium chloride was added confirms the presence of sodium chloride, which was used as a catalyst in the reaction. The sodium chloride did not affect the purity of the ethanol product.Conclusion:The objective of synthesizing ethanol from ethanolamine using the dehydration reaction was successfully achieved in this experiment. Ethanol was produced, and the purity of the product was confirmed by observing the color changes and precipitate formation. This experiment provided a practical approach to understanding the dehydration reaction and its application in the synthesis of organic compounds.。

化学性质实验报告

糖、氨基酸和蛋白质的鉴定糖类化合物：又称碳水化合物，是多羟基醛或多羟基酮及其缩聚物和某些衍生物的总称，一般由碳、氢与氧三种元素所组成。

实验目的：（1）进一步了解糖的化学性质；（2）掌握鉴定糖的方法及其原理。

（一）-萘酚试验（molish)糖类化合物一个比较普遍的定性反应是molish 反应。

即在浓硫酸存在下，糖与-萘酚(molish试剂）作用生成紫色环。

实验方法取3支试管，编号，分别加入 ml %的各待测糖水溶液，滴入2滴molish 试剂（ -萘酚的乙醇溶液），摇匀。

把试管倾斜450，沿管壁慢慢加入约1ml 浓硫酸（切勿摇动），小心竖直后仔细观察两层液面交界处的颜色变化。

硫酸在下层,试液在上层样品：葡萄糖、蔗糖及淀粉解释:糖被浓硫酸脱水生成糠醛或糠醛衍生物，后者进一步与-萘酚缩合生成紫红色物质，在糖液和浓硫酸的液面间形成紫色环。

（二） fehling试验（1）实验原理fehling试剂：含有硫酸铜和酒石酸钾钠的氢氧化钠溶液。

硫酸铜与碱溶液混合加热，生成黑色的氧化铜沉淀。

若同时有还原糖存在，则产生黄色或砖红色的氧化亚铜沉淀。

为防止铜离子和碱反应生成氢氧化铜或碱性碳酸铜沉淀，fehling试剂中需加入酒石酸钾钠，它与cu2＋形成的酒石酸钾钠络合铜离子是可溶性的络离子。

（2）操作方法取4支试管，编号，分别加入fehling试剂i和ii 各。

摇匀并置于水浴中微热后，分别加入5滴待测糖溶液，振荡后置于沸水浴中加热2 ~ 3min，取出冷却，观察颜色变化及有无沉淀析出。

fehling试剂 i：称取 g硫酸铜溶于100 ml蒸馏水中, 得淡蓝色的 fehling试剂 i。

fehling试剂 ii：将17g酒石酸钾钠溶于20ml热水中，然后加入20 ml 含5 g naoh的水溶液，稀释至100 ml得无色透明的fehling试剂 ii。

样品：葡萄糖、果糖、蔗糖及麦芽糖解释: 硫酸铜与碱溶液混合加热，生成黑色的氧化铜沉淀。

生物化学实验报告参考模板

实验一考马斯亮蓝G-250染色法测定蛋白质的含量（p24）一、目的要求掌握考马斯亮蓝（Coomassie Brilliant Blue）法测定蛋白质含量原理和方法。

二、实验原理考马斯亮蓝法测定蛋白质浓度，是利用蛋白质─染料结合的原理，定量的测定微量蛋白浓度的快速、灵敏的方法。

这种蛋白质测定法具有超过其他几种方法的突出优点，因而正在得到广泛的应用。

这一方法是目前灵敏度最高的蛋白质测定法。

考马斯亮兰G-250染料在酸性溶液中为棕红色，当它与蛋白质通过范德华键结合后，变为蓝色。

在酸性溶液中与蛋白质结合，使染料的最大吸收峰（lmax）的位置，由465nm变为595nm。

且在蛋白质一定浓度范围内符合比尔定律，通过测定595nm处光吸收的增加量可知与其结合蛋白质的量。

研究发现，染料主要是与蛋白质中的碱性氨基酸（特别是精氨酸）和芳香族氨基酸残基相结合。

考马斯亮蓝染色法的突出优点是：（1）灵敏度高，据估计比Lowry法约高四倍，其最低蛋白质检测量可达1mg。

这是因为蛋白质与染料结合后产生的颜色变化很大，蛋白质－染料复合物有更高的消光系数，因而光吸收值随蛋白质浓度的变化比Lowry法要大的多。

（2）测定快速、简便，只需加一种试剂。

完成一个样品的测定，只需要5分钟左右。

由于染料与蛋白质结合的过程，大约只要2分钟即可完成，其颜色可以在1小时内保持稳定，且在5分钟至20分钟之间，颜色的稳定性最好。

因而完全不用像Lowry法那样费时和严格地控制时间。

（3）干扰物质少。

如干扰Lowry法的K+、Na+、Mg2+离子、Tris缓冲液、糖和蔗糖、甘油、巯基乙醇、EDTA等均不干扰此测定法。

此法的缺点是：（1）由于各种蛋白质中的精氨酸和芳香族氨基酸的含量不同，因此考马斯亮蓝染色法用于不同蛋白质测定时有较大的偏差，在制作标准曲线时通常选用g—球蛋白为标准蛋白质，以减少这方面的偏差。

（2）仍有一些物质干扰此法的测定，主要的干扰物质有：去污剂、Triton X-100、十二烷基硫酸钠（SDS）等。

化学实验报告英文版

Title: Synthesis of Ethyl Acetate from Ethanol and Acetic AcidDate: [Date of Experiment]Student Name: [Your Name]Lab Section: [Your Lab Section Number]Objective: The objective of this experiment was to synthesize ethyl acetate, a volatile organic compound, by the esterification of ethanol and acetic acid. This reaction is a classic example of a nucleophilic acyl substitution reaction, where the alcohol attacks the carbonyl carbon of the acid to form the ester.Introduction:Esters are organic compounds derived from carboxylic acids by the replacement of the hydroxyl group with an alkyl or aryl group. Ethyl acetate is a widely used solvent in the pharmaceutical, food, and perfume industries due to its pleasant smell and volatility. The synthesis of ethyl acetate is typically achieved through the esterification reaction between acetic acid and ethanol in the presence of an acid catalyst.Materials:- Ethanol (CH3CH2OH)- Acetic acid (CH3COOH)- Concentrated sulfuric acid (H2SO4) - Catalyst- Sodium chloride (NaCl) - Dehydrating agent- Water - Solvent- Distillation apparatus- thermometer- glassware (beakers, flasks, etc.)- pH meterProcedure:1. Preparation of Reactants:- Measure 10 mL of ethanol and 10 mL of acetic acid into a round-bottom flask.- Add 1 mL of concentrated sulfuric acid as a catalyst.- Swirl the flask gently to mix the contents.2. Heating and Stirring:- Place the flask on a hot plate and heat the mixture to approximately 50-60°C. Maintain the temperature for about 30 minutes, ensuring the mixture is well-stirred.- The reaction is exothermic, so be cautious when heating.3. Adding Sodium Chloride:- After the reaction time, remove the flask from the heat.- Add a small amount of sodium chloride to the mixture. This helps to remove water from the reaction mixture, which can be a byproduct of the reaction.4. Observation:- The reaction mixture should now have a noticeable odor of ethyl acetate.- The mixture may also turn a light yellow due to the formation of the ester.5. Distillation:- Set up the distillation apparatus as per the instructor's instructions.- Heat the mixture to about 78°C, which is the boiling point ofethyl acetate.- Collect the distillate in a receiving flask. The distillate should have a fruity odor characteristic of ethyl acetate.6. Analysis:- Use a pH meter to check the pH of the distillate. Ethyl acetate is a neutral compound, so the pH should be close to 7.Results:- The reaction mixture turned a light yellow after the addition of sodium chloride.- The distillation process yielded approximately 5 mL of distillate with a fruity odor.- The pH of the distillate was measured to be 6.8.Discussion:The synthesis of ethyl acetate from ethanol and acetic acid was successful, as evidenced by the formation of a volatile distillate with the characteristic odor of ethyl acetate. The use of concentrated sulfuric acid as a catalyst facilitated the esterification reaction by protonating the carbonyl oxygen of acetic acid, making it more electrophilic and susceptible to nucleophilic attack by the alcohol. The addition of sodium chloride helped to remove water, which could potentially interfere with the reaction by acting as a nucleophile.The distillation process was crucial for isolating the ethyl acetate from the reaction mixture. By carefully controlling the temperature, we were able to collect the desired compound while leaving behind the unreacted starting materials and byproducts.Conclusion:In conclusion, the synthesis of ethyl acetate from ethanol and acetic acid was successfully achieved through the esterification reaction. The use of concentrated sulfuric acid as a catalyst and the distillation process allowed for the isolation of the desired compound. Thisexperiment provided a practical understanding of esterification reactions and the techniques involved in organic synthesis.Appendix:- Chemical Equation:\[ \text{CH}_3\text{CH}_2\text{OH} + \text{CH}_3\text{COOH}\xrightarrow{\text{H}_2\text{SO}_4} \text{CH}_3\text{COOCH}_2\text{CH}_3 + \text{H}_2\text{O} \]- Safety Precautions:- Wear safety goggles and gloves at all times.- Avoid contact with concentrated sulfuric acid and acetic acid.- Do not inhale the vapors of the distillate.。

分析化学实验报告范文(完整版)

报告编号：YT-FS-8612-63分析化学实验报告范文(完整版)After Completing The T ask According To The Original Plan, A Report Will Be Formed T o Reflect The Basic Situation Encountered, Reveal The Existing Problems And Put Forward Future Ideas.互惠互利共同繁荣Mutual Benefit And Common Prosperity分析化学实验报告范文(完整版)备注：该报告书文本主要按照原定计划完成任务后形成报告，并反映遇到的基本情况、实际取得的成功和过程中取得的经验教训、揭露存在的问题以及提出今后设想。

文档可根据实际情况进行修改和使用。

实验题目:草酸中h2c2o4含量的测定实验目的:学习naoh标准溶液的配制、标定及有关仪器的使用;学习碱式滴定管的使用，练习滴定操作。

实验原理:h2c2o4为有机弱酸，其ka1=5、9×10-2，ka2=6、4×10-5、常量组分分析时cka1>10-8，cka2>10-8，ka1/ka2<105，可在水溶液中一次性滴定其两步离解的h+:h2c2o4+2naoh===na2c2o4+2h2o计量点ph值8、4左右，可用酚酞为指示剂。

naoh标准溶液采用间接配制法获得，以邻苯二甲酸氢钾标定:-cook-cooh+naoh===-cook-coona+h2o此反应计量点ph值9、1左右，同样可用酚酞为指示剂。

实验方法:一、naoh标准溶液的配制与标定用台式天平称取naoh1g于100ml烧杯中，加50ml 蒸馏水，搅拌使其溶解。

移入500ml试剂瓶中，再加200ml蒸馏水，摇匀。

准确称取0、4~0、5g邻苯二甲酸氢钾三份，分别置于250ml锥形瓶中，加20~30ml蒸馏水溶解，再加1~2滴0、2%酚酞指示剂，用naoh标准溶液滴定至溶液呈微红色，半分钟不褪色即为终点。

英文实验报告化学

Abstract:The synthesis of nanocrystalline copper phthalocyanine (CuPc) wascarried out using a solvothermal method. The reaction conditions, including the choice of solvent, temperature, and time, were optimized to achieve the highest yield and purity of CuPc. The synthesized CuPc was characterized using various techniques such as UV-Vis spectroscopy, X-ray diffraction (XRD), scanning electron microscopy (SEM), and transmission electron microscopy (TEM). The results indicate that the solvothermal method is an efficient and effective approach for the synthesis of CuPc nanocrystals with high purity and excellent optical properties.1. Introduction:Copper phthalocyanine (CuPc) is a well-known blue pigment with significant applications in various fields, including optoelectronics, catalysis, and medicine. The unique optical and electronic properties of CuPc, such as its strong absorption in the visible region and high thermal stability, make it an attractive material for many applications. In recent years, the development of nanocrystalline CuPc has gained considerable attention due to its enhanced properties compared to its bulk counterpart. The solvothermal method has been widely used for the synthesis of various inorganic and organic nanomaterials due to its simplicity, cost-effectiveness, and environmentally friendly nature.2. Materials and Methods:2.1 Materials:- Copper(II) sulfate pentahydrate (CuSO4·5H2O)- Potassium phthalocyanine (K3Pc)- Sodium hydroxide (NaOH)- Ethanol (EtOH)- Deionized water2.2 Synthesis of CuPc Nanocrystals:The synthesis of CuPc nanocrystals was carried out using the solvothermal method. The detailed procedure is as follows:1. Dissolve 0.5 g of CuSO4·5H2O and 0.5 g of K3Pc in 10 mL of ethanol under magnetic stirring for 1 hour.2. Add 0.5 g of NaOH to the solution and continue stirring for another hour.3. Transfer the reaction mixture into a Teflon-lined autoclave and heat it at 180°C for 12 hours.4. Cool the autoclave to room temperature and centrifuge the reaction mixture at 5000 rpm for 30 minutes.5. Wash the precipitate with ethanol and deionized water several times to remove impurities.6. Dry the precipitate in an oven at 60°C for 12 hours to obtain the final product.2.3 Characterization Techniques:The synthesized CuPc nanocrystals were characterized using the following techniques:- UV-Vis spectroscopy (Shimadzu UV-2600)- X-ray diffraction (XRD) (Bruker D8 Advance)- Scanning electron microscopy (SEM) (Hitachi S-4800)- Transmission electron microscopy (TEM) (JEOL JEM-2100)3. Results and Discussion:3.1 UV-Vis Spectroscopy:The UV-Vis absorption spectrum of the synthesized CuPc nanocrystals is shown in Figure 1. The spectrum exhibits a strong absorption peak at 640 nm, which is characteristic of CuPc. The shoulder peak at 690 nm is attributed to the transition of π-π.Figure 1: UV-Vis absorption spectrum of CuPc nanocrystals3.2 XRD Analysis:The XRD pattern of the synthesized CuPc nanocrystals is shown in Figure 2. The diffraction peaks are well matched with the standard JCPDS card No. 12-0465, indicating the presence of CuPc in the crystalline form. The crystal size of the CuPc nanocrystals was calculated to be approximately 20 nm.Figure 2: XRD pattern of CuPc nanocrystals3.3 SEM Analysis:The SEM image of the synthesized CuPc nanocrystals is shown in Figure 3. The image reveals the spherical shape of the nanocrystals with an average diameter of 20 nm.Figure 3: SEM image of CuPc nanocrystals3.4 TEM Analysis:The TEM image of the synthesized CuPc nanocrystals is shown in Figure 4. The image confirms the spherical shape of the nanocrystals with a size of approximately 20 nm. The high-resolution image shows the crystalline structure of the CuPc nanocrystals.Figure 4: TEM image of CuPc nanocrystals4. Conclusion:In this study, the solvothermal method was employed for the synthesis of nanocrystalline CuPc. The optimized reaction conditions, including the choice of solvent, temperature, and time, resulted in the formation of CuPc nanocrystals with high purity and excellent optical properties. The synthesized CuPc nanocrystals were characterized using various techniques, including UV-Vis spectroscopy, XRD, SEM, and TEM. Theresults indicate that the solvothermal method is an efficient and effective approach for the synthesis of CuPc nanocrystals with high purity and excellent optical properties.5. Acknowledgments:The authors would like to acknowledge the financial support from the National Natural Science Foundation of China (Grant No. 123456) and the China Scholarship Council (Grant No. 789012).References:1. A. G. Aliev, V. I. Gerasimchuk, A. A. Shevchenko, and A. V. Shevchenko, "Preparation and properties of CuPc/CdS core-shell quantum dots," Journal of Nanomaterials, vol. 2012, Article ID 682318, 2012.2. S. M. Y. Y. Ahamed, S. S. Al-Asfour, and A. A. Al-Asfour, "Synthesis and characterization of copper phthalocyanine thin films using chemical bath deposition method," Journal of Nanomaterials, vol. 2013, Article ID 982916, 2013.3. X. J. Wang, Z. Y. Chen, Y. J. Gao, Y. J. Li, and J. P. Zhang, "Preparation and characterization of CuPc nanocrystals using a microwave-assisted solvothermal method," Journal of Nanomaterials, vol. 2013, Article ID 916402, 2013.4. M. A. E. Al-Asfour, S. S. Al-Asfour, and A. G. Aliev, "Preparation and characterization of copper phthalocyanine/CdS core-shell quantum dots using a solvothermal method," Journal of Nanomaterials, vol. 2014, Article ID 382594, 2014.5. M. A. E. Al-Asfour, S. S. Al-Asfour, and A. G. Aliev, "Preparation and characterization of copper phthalocyanine nanocrystals using a microwave-assisted solvothermal method," Journal of Nanomaterials, vol. 2014, Article ID 382594, 2014.。

【优质文档】化学英语实验报告-实用word文档 (5页)

本文部分内容来自网络整理，本司不为其真实性负责，如有异议或侵权请及时联系，本司将立即删除！== 本文为word格式，下载后可方便编辑和修改！ ==化学英语实验报告篇一：英文版化学实验报告Preparation of ethyl acetateFirst, the purpose of the experiment:1、 Learn from the general principles of organic synthetic esters and methods2、 Master distillation, extraction, drying and other experimental techniques and its application in aspecific experimentSecond, the experimental principle:Main reaction：CH3COOH+CH3CH2OH=CH3COOCH2CH3+H2OConditions: heating to 120 to 125 °C in concentratedsulfuric acid catalyzedSide effects：浓H2SO4CH3CH2OH--------->CH2=CH2+H2O170度浓H2SO4CH3CH2OH--------->CH3CH2OCH2CH3+H2O140度Third, the instruments and reagents:1、 Instruments and materials: Round-bottomed flask,Spherical condenser, Straight condenser，Distillationhead, a separatory funnel, measuring beakers, dropper, conical flask, thermometer, electric2、 drugs: Glacial acetic acid (AR), absolute ethanol (AR),concentrated sulfuric acid, saturated brine, a saturated sodium carbonate solution, a saturated calcium chloride solution, dried over anhydrous magnesium sulfate, litmusFourth,Reactor：Fifth,Experimental procedure:Adding 50ml round bottom flask 3ml 5ml ethanol and acetic acid, in shaking batch of concentrated sulfuric acid was added1.3ml mixed, and add a few grains of zeolite, and then install the instrument responseLow heat, slowly reflux for 30 minutes. Coolish, reflux device to the distillation apparatus, wetted with cold water to cool the bottle. Heating distillation until the distillate liquid volume is about half the volume of the reaction so far to give the crude product in ethyl acetateThe distillate was slowly saturated sodium carbonate solution was added portionwise, and oscillate until the evolution of carbondioxide gas without using litmus paper test acetate layer was neutral. The mixture was then transferred to a separatory funnel, andseparated aqueous layer was washed once with saturated aqueous saline solution 3ml The organic layer was washed with a saturated solutionof calcium chloride 3ml, washed with water and finally once. The organic layer in a dry Erlenmeyer flask filled with anhydrous magnesium sulfate. The crude ethyl acetate, dried on a water bath heated to distill, collecting fractions 73 to 78°C. Weigh or measure product volume, and calculate the yield point or refractive index measurement products。

化学实验报告_英文

Experiment Title: Determination of the Molar Mass of a Volatile CompoundDate: October 1, 2021Objective:The objective of this experiment is to determine the molar mass of a volatile compound by using the ideal gas law and the known density of the compound.Introduction:The molar mass of a substance is the mass of one mole of that substance. It is an important property used to identify and characterize compounds. In this experiment, we will determine the molar mass of a volatile compound using the ideal gas law and the known density of the compound.Materials:1. Sample of volatile compound2. Graduated cylinder3. Balance4. Beaker5. Thermometer6. Ice bath7. Gas syringe8. Data tableProcedure:1. Measure the mass of the sample using a balance and record the value.2. Pour a known volume of water into a graduated cylinder and record the initial volume.3. Add the sample to the graduated cylinder and record the final volume.4. Calculate the volume of the sample by subtracting the initial volume from the final volume.5. Measure the temperature of the sample using a thermometer and record the value.6. Transfer the sample to a beaker and cool it in an ice bath until the temperature reaches 0°C.7. Use a gas syringe to measure the volume of the gas at 0°C and record the value.8. Calculate the density of the sample by dividing the mass of the sample by the volume of the sample.9. Use the ideal gas law to calculate the molar mass of the compound.Results:1. Mass of the sample: 1.23 g2. Volume of the sample: 2.45 mL3. Temperature of the sample: 25°C4. Volume of the gas at 0°C: 1.20 mL5. Density of the sample: 0.51 g/mLCalculation:1. Molar mass = (mass of the sample / volume of the gas) x (temperature of the gas / pressure of the gas) x (1 atm / 22.4 L/mol)2. Molar mass = (1.23 g / 1.20 mL) x (273.15 K / 298.15 K) x (1 atm / 1.20 mL) x (22.4 L/mol)3. Molar mass = 108.0 g/molDiscussion:In this experiment, we determined the molar mass of a volatile compound by using the ideal gas law and the known density of the compound. Thecalculated molar mass was 108.0 g/mol, which is in good agreement with the literature value of 106.0 g/mol. This indicates that the experimental method used in this experiment is reliable and accurate.Conclusion:The molar mass of the volatile compound was determined to be 108.0 g/mol using the ideal gas law and the known density of the compound. This experiment demonstrates the effectiveness of using the ideal gas law to determine the molar mass of volatile compounds.References:1. Silberberg, M. S. (2012). Chemistry: The Central Science (10th ed.). Boston, MA: McGraw-Hill.2. Atkins, P. W., & de Paula, J. (2014). Atkins' Physical Chemistry(11th ed.). New York, NY: Oxford University Press.。

关于英文版化学实验报告

篇一：英文版化学实验报告Title: Preparation of Fe scrap from waste(NH4)The purpose of the experimentLearn the method used scrap iron preparation of ferrous ammonium sulfate.Familiar with the water bath, filtered, and evaporated under reduced pressure and crystallization basic working.The experimental principle, the iron and sulfuric acid to generate reactive ferrous sulfate, ferrous sulfate and ammonium sulfate in an aqueous solution of equal molar interaction, becomes less soluble blue generate ferrous ammonium sulfate.Fe+H2SO4=FeSO4+H2 (gas)FeSO4+ (NH4)2SO4+6H2O=(NH4) Usually ferrous rocks are easily oxidized in air, but after the formation of relatively stable perfunctory, not to be oxidized.Experiment to use instruments, scales, constant temperature water bath, pumps, basins, cups, 10ml graduated cylinder, asbestos mesh, glass, tripod, alcohol lamp, funnel.Iron pieces to a solid pharmaceutical use, use of acid ammonium sulfate and 3mol / l of sulfuric acid, concentrated sulfuric acid.The experiment was divided into four steps.The first step Said iron powder 4g into a beaker and then 50ml10ml, 3mol / L H2SO4 was added to the same beaker. The second step will be the beaker is heated to no more bubbles, and then filtered hot and the filtrate was then filled in 100ml beaker. The third step, called 4g (NH4)2SO4, and the resultingammonium sulfate and of water to form a saturated solution, and then add it to the ferrous sulfate solution, adjusted with concentrated sulfuric acid to PH = 1. A fourth step, the third step the solution was heated in a water bath to the surface until the film is crystallized, it was slowly cooled andthen filtered under reduced pressure to stand finally dried, weighed and the yield was calculated. The results obtained bluish powderycrystals. Have this result we can calculate yield, starting with the first step we tried to know the amount of iron, should this wecan calculate the theoretical sulfate ferrous sulfate is , thenferrous sulfate obtained by thetheoretical value of ammonium. FeSO4+（NH4）2SO4+6H2O=FeSO4.(NH4) molX=m=XM=ⅹ392g/mol=Yield = the actual value of the formula is divided by the theoretical value by 100%.it will be calculated into the dataobtained in a yield of %.篇二：英文版化学实验报告The preparation of alkali type copper carbonateThe first:the experiment purposethe methods of alkali type copper carbonate prepared andprinciplethe design experiment to cultivate independent design abilityand chemical research thinkingThe second:the experimental principleThe solubility of Cu(OH)2and CuCO3 are similar, With Cu2(OH)2CO3 solid precipitation in the solution.2CuSO4+2Na2CO3+H2O==Cu2(OH)2CO3↓+2Na2SO4+CO2↑The third:the experimental stepspreparationDisposes mole of each litre acid sour coppers and sodiumcarbonate solution each 100 milliliters.feeding order and raw material compare the explorationAccording to 2:,2:2,2:,2: allocated proportion, is accepted after passing an examination the surface disposition acid sour copper and the sodium carbonate solution, joins in separately 8 test tubes,joins rapidly the sulfuric acid copper solutions in the sodium carbonate solution, vibrates about other constant temperature ten minutes as for 75 degrees Celsius water baths in, the inversion feeding order recreates one time, the observation has the precipitation speed, quantity how many and the color,discovers the optimum condition.explorationAccording to the above optimum condition, takes the acid sour copper solutions and the sodium carbonate solution separately under 50, 75 and 100 degrees Celsius responded that, discovers the optimum temperature.to 2, 3 step exploration optimum condition prepares the final product, and with the distilled water lavation, finally dries and calls heavily.(Enlarges ten times with conical flask to do)The fourth:the experimental itemsInstrument and material: The balance, the beaker, the glass rod, the Volumetric flask, the test tube, the filter flask,the Buchner funnel, the Erlenmeyer flaskChemicals: Copper carbonate, sodium sulfateThe fifth:the experimental resultthe step 2, the observation phenomenon optimum condition is equal to for the cupric sulfate compared to the sodium carbonate 2:, the feeding order for joins the sulfuric acid copper solutions to the sodium carbonate solution in.the step 3, the observation phenomenon optimum temperature is 75 degrees Celsiusto the copper sulfate solution than sodium carbonatesolution is 2:2. 4, ten times magnification, alkali type copper carbonate was zero point five grams, according to the reaction equation calculation yield.2CuSO4+2Na2CO3+H2O==Cu2(OH)2CO3↓+2Na2SO4+CO2↑2 1* X2/(*)=1/XX=M[Cu2(OH)2CO3]=*222=Productive rate:/*100%=45%The sixth : Questions1. Which cupric salt suit the system to take the cupric basic carbonate? Answer:Cu(NO)3 or CuSO42. The reaction temperature has what influence to this experiment?.Answer:The temperature excessively is low, the response speed is slow; The hyperpyrexia, the Cu2(OH)2CO3 decomposition is CuO.3. Reaction is carried out at what temperature will appear Brown product? What is the brown substance?Answer: The temperature is equal to 100 degrees Celsius and this brown material is CuO.篇三：化学专业英语实验报告In the physiological saline the sodium chloride content determinationone, the experimental goal1、 the study silver nitrate standard solution configuration and the demarcation method2、 the grasping law raises Si Fa to determine the chloride ion the method principle two, the experimental principleWith AgNO3 standard solution titration Cl - Ag + + Cl - = = AgCl，At ph - available fluorescent yellow do indicator (HFIn)HFIn = = FIn (yellow) + H +Sp before: excessive, AgCl precipitation adsorption of Cl - AgCl Cl - + FIn - (yellow-green)After Sp: Ag +, excessive AgCl precipitation Ag + adsorption, adsorption FIn - reprecipitation AgCl, Ag + + FIn - = = AgCl, Ag +, FIn - (pink) The finish color changes: from yellowish green to orange Three, instruments and reagentsEquipment and materials：Acid type buret (150 ml), taper bottle (250 ml), volumetric flask (100 ml), pipette (20 ml, 10 ml), measuring cylinder (100 ml, 10 ml), beaker (100 ml), brown reagent bottles (500 ml), analytical balance, platform scale. The reagent and drug: Analysis of AgNO3 (s, pure), NaCl (s,analysis of pure), physiological saline, fluorescent yellow - starch. Fourth, the experimental stepsAccurately moving 25 ml co ncentration is mol ╱ L of silver nitrate standard solution in the middle of 250 ml volumetric flask, dilute to scale as a standard solution titration.Accurately moving saline ml to 250 ml conical flask, add 50 ml water, 3 drops of fluorescent yellow indicator, 5% starch indicator 5 ml, under continuous agitation, using silver nitratestandard solution titration to solution from yellow to pink is the end point. Record the consumption volume of silver nitratestandard solution, parallel determination of 3, calculate the sodium chloride content in saline and relative mean deviation.Fifth, data recording and processingFormula: ρ = V×MrNaCl×CAgNO3 x 100The average deviation d= dr=d/ρ×100%=%实验名称：硅片的清洗实验目的：1.熟悉清洗设备2.掌握清洗流程以及清洗前预准备实验设备：1.半导体兆声清洗机（SFQ-1006T）；SC-2实验背景及原理：清洗的目的在于清除表面污染杂质，包括有机物和无机物。

英文版的化学实验报告

Experiment Title: Synthesis of Ethyl AcetateObjective:The objective of this experiment is to synthesize ethyl acetate, an important ester used in various applications such as perfumes, flavors, and solvents. The reaction involves the esterification of acetic acid and ethanol in the presence of an acid catalyst.Experimental Procedure:1. Materials:- Acetic acid (CH3COOH)- Ethanol (C2H5OH)- Concentrated sulfuric acid (H2SO4)- Sodium chloride (NaCl)- Ice- Sodium bicarbonate (NaHCO3)- Ethyl acetate (product)- Distilled water- Erlenmeyer flask (100 mL)- Conical flask (500 mL)- Round-bottom flask (1000 mL)- Distillation apparatus- Heat source- Stirring rod- Thermometer- pH meter- Safety goggles- Lab coat- Gloves2. Procedure:a. Weigh 10.0 g of acetic acid and 5.0 g of ethanol using an analytical balance and transfer them into an Erlenmeyer flask.b. Add 2 mL of concentrated sulfuric acid to the flask and mix the contents thoroughly using a stirring rod.c. Place the flask in an ice bath to maintain a low temperature throughout the reaction.d. After 1 hour, remove the flask from the ice bath and observe the formation of a cloudy solution.e. Add 10 g of sodium chloride to the flask and mix well.f. Slowly add 50 mL of distilled water to the flask while stirring continuously to dilute the solution.g. Transfer the solution to a conical flask and add 10 g of sodium bicarbonate.h. Stir the solution until the acid is neutralized, as indicated by the disappearance of effervescence.i. Set up the distillation apparatus, ensuring that the distillation flask is connected to the condenser and the receiver.j. Heat the mixture slowl y and maintain a temperature between 70°C and 80°C.k. Collect the distillate in the receiver and observe the formation of ethyl acetate.l. Stop the distillation when the temperature rises above 80°C.m. Remove the receiver and allow the ethyl acetate to cool to room temperature.n. Filter the distillate through a filter paper to remove any impurities.Results:1. The reaction mixture was cloudy after 1 hour of reaction, indicating the formation of ethyl acetate.2. The addition of sodium bicarbonate neutralized the acid, causing the disappearance of effervescence.3. The distillation process yielded approximately 10 mL of ethyl acetate, as observed in the receiver.4. The pH of the reaction mixture before neutralization was 2.5, indicating the presence of excess acid.5. The pH of the neutralized mixture was 7, indicating complete neutralization.Discussion:The synthesis of ethyl acetate involves the esterification reaction between acetic acid and ethanol in the presence of an acid catalyst. The reaction proceeds via the formation of an intermediate, the acetyl ethoxide, which then reacts with water to produce ethyl acetate andacetic acid. The addition of concentrated sulfuric acid serves as a catalyst to facilitate the reaction.The formation of a cloudy solution after 1 hour of reaction suggests the successful formation of ethyl acetate. The addition of sodiumbicarbonate neutralizes the excess acid, allowing the ethyl acetate tobe isolated as a distillate. The distillation process is essential for separating the ethyl acetate from the remaining impurities and water.The yield of ethyl acetate obtained in this experiment is approximately 10 mL, which is consistent with the expected yield based on the stoichiometry of the reaction. The reaction conditions, such astemperature and reaction time, play a crucial role in achieving the desired yield and purity of the product.Conclusion:In this experiment, the synthesis of ethyl acetate was successfully achieved through the esterification reaction of acetic acid and ethanol in the presence of an acid catalyst. The reaction mixture was neutralized using sodium bicarbonate, and the ethyl acetate was isolated by distillation. The yield of ethyl acetate obtained was consistent with the expected yield, and the reaction conditions were optimized to achieve the desired results.References:- Advanced Organic Chemistry: Reactions, Mechanisms, and Structure by Francis A. Carey and Richard J. Sundberg- Organic Chemistry by Jonathan Clayden, Nick Greeves, Stuart Warren, and Peter Wothers。

化学实验报告英语作文(3篇)

第1篇Experiment Name: Preparation of Sodium Chloride from SaltwaterDate: [Date]Objective: The objective of this experiment was to prepare sodium chloride from saltwater by the process of evaporation and crystallization.Introduction:Saltwater is a mixture of water and sodium chloride (NaCl), which is commonly found in oceans, seas, and lakes. The concentration of sodium chloride in saltwater can vary, but it is typically around 3.5% by weight. The process of evaporation and crystallization is used to separate sodium chloride from saltwater and obtain pure sodium chloride crystals.Materials:- Saltwater- Evaporating dish- Bunsen burner- Glass stirring rod- Weighing balance- Filter paper- Funnel- Beaker- Test tube- Microscope- Sodium chloride crystals (for comparison)Procedure:1. Measure 100 mL of saltwater using a graduated cylinder and transfer it to an evaporating dish.2. Place the evaporating dish on a hot plate and heat it using a Bunsen burner. Stir the saltwater continuously with a glass stirring rod to prevent localized boiling and ensure even evaporation.3. Observe the evaporation process until the saltwater is reduced to a small volume, approximately 20 mL. At this point, the concentration of sodium chloride has increased significantly.4. Remove the evaporating dish from the hot plate and allow it to cool down to room temperature.5. Once the evaporating dish is cool, observe the crystallization process. Sodium chloride crystals will start to form as the solution cools down.6. Use a filter paper and funnel to collect the sodium chloride crystals from the evaporating dish. Wash the crystals with distilled water to remove any impurities.7. Transfer the sodium chloride crystals to a beaker and dry them usinga Bunsen burner. Allow the crystals to cool down to room temperature before weighing them.8. Compare the weight of the sodium chloride crystals obtained from the experiment with the known weight of sodium chloride crystals (for comparison).Results:- Initial weight of the sodium chloride crystals: [Weight]- Weight of the sodium chloride crystals obtained from the experiment: [Weight]- Known weight of sodium chloride crystals (for comparison): [Weight]Discussion:In this experiment, we successfully prepared sodium chloride from saltwater using the process of evaporation and crystallization. As the saltwater was heated, the water evaporated, leaving behind the sodium chloride crystals. The concentration of sodium chloride in the saltwater increased as the water evaporated, leading to the formation of crystals. The purity of the sodium chloride crystals was determined by comparing the weight of the obtained crystals with the known weight of sodium chloride crystals.The experiment demonstrated the effectiveness of the evaporation and crystallization process in separating sodium chloride from saltwater. However, it is important to note that the purity of the obtained sodium chloride crystals can be affected by various factors such as impurities in the saltwater and the conditions of evaporation and crystallization.Conclusion:The objective of this experiment was achieved by successfully preparing sodium chloride from saltwater using the process of evaporation and crystallization. The obtained sodium chloride crystals were compared with the known weight of sodium chloride crystals, and the experiment was found to be successful in obtaining pure sodium chloride. Further optimization of the experimental conditions could potentially improve the purity of the obtained sodium chloride crystals.第2篇Experiment Title: Synthesis of Ethanol from EtheneDate: October 15, 2023Objective: The objective of this experiment was to synthesize ethanol from ethene using the hydration reaction. The experiment aimed to demonstrate the principles of chemical reactions, the use of laboratory equipment, and the application of safety protocols.Materials:- Ethene (C2H4)- Concentrated sulfuric acid (H2SO4)- Water (H2O)- Sodium chloride (NaCl) solution- Potassium dichromate (K2Cr2O7) solution- Iron (III) chloride (FeCl3) solution- Ethanol (C2H5OH) standard solution- Chloroform (CHCl3)- Distillation apparatus- Gas burner- Test tubes- Beakers- Pipettes- Thermometer- Stirring rod- Safety goggles- Lab coat- GlovesProcedure:1. Preparation of Ethene Solution:- Ethene was passed through a column filled with sodium chloride solution to remove impurities.- The purified ethene was collected in a test tube.2. Hydration Reaction:- A beaker containing concentrated sulfuric acid was heated gently.- The ethene was then passed through the hot sulfuric acid, where it underwent hydration to form ethanol.- The resulting solution was allowed to cool.3. Purification of Ethanol:- The mixture was separated using a separating funnel to remove unreacted ethene and sulfuric acid.- The organic layer, containing ethanol, was collected in a clean beaker.4. Confirmation of Ethanol Formation:- A small amount of the organic layer was mixed with potassium dichromate and iron (III) chloride solutions.- A color change indicated the presence of alcohol, confirming the formation of ethanol.5. Distillation:- The organic layer was transferred to a distillation apparatus.- Ethanol, with a boiling point of 78.37°C, was distilled off a nd collected in a receiver.6. Analysis:- The purity of the distilled ethanol was determined using a gas chromatograph.- The yield of ethanol was calculated based on the initial amount of ethene used.Results:- Ethanol Formation:- The reaction mixture turned yellow upon addition of potassium dichromate and iron (III) chloride, indicating the presence of alcohol.- Distillation:- The distillation process yielded approximately 50 mL of ethanol, corresponding to a yield of 40%.- Gas Chromatography:- The gas chromatography analysis confirmed the purity of the ethanol to be 95%.Discussion:The experiment successfully synthesized ethanol from ethene through the hydration reaction. The use of concentrated sulfuric acid as a catalyst facilitated the reaction, and the distillation process allowed for the separation of pure ethanol. The yield of 40% was reasonable, considering the limitations of the experimental setup and the potential for side reactions. The purity of the ethanol, as determined by gas chromatography, was satisfactory, indicating a successful synthesis.Conclusion:This experiment provided a practical demonstration of the hydration reaction and the synthesis of ethanol from ethene. The use of laboratory techniques and safety protocols was crucial in ensuring the success of the experiment. The results indicate that the synthesis of ethanol is a feasible process, and further optimization could potentially increase the yield and purity of the product.Safety Precautions:- All chemicals were handled with care, and appropriate personal protective equipment, including safety goggles, lab coat, and gloves, was worn at all times.- Concentrated sulfuric acid and other hazardous chemicals were handled using proper techniques to avoid spills and inhalation of vapors.- The gas burner was used with caution, and the distillation apparatus was securely fastened to prevent any accidents.References:- Smith, J. M. (2020). Introduction to Organic Chemistry. New York: Oxford University Press.- Johnson, R. L. (2019). Principles of Chemical Engineering. Boston: McGraw-Hill Education.第3篇Experiment Title: Synthesis of Silver NitrateDate: [Date]Time: [Time]Lab Section: [Lab Section]Lab Partner: [Partner's Name]Abstract:The objective of this experiment was to synthesize silver nitrate by reacting silver with concentrated nitric acid. The experiment aimed to understand the chemical reaction involved, the properties of the products, and the safety precautions associated with the use of hazardous chemicals.Introduction:Silver nitrate is a compound with the chemical formula AgNO3. It is a white crystalline solid that is highly soluble in water. Silver nitrate is used in various applications, including photography, medicine, and the preparation of other silver compounds. In this experiment, we synthesized silver nitrate by reacting silver with concentrated nitric acid.Materials:- Silver metal (shiny silver coins or pellets)- Concentrated nitric acid (HNO3)- Distilled water- Test tubes- Beakers- Glass rods- Safety goggles- Lab coat- Gloves- Bunsen burner- Heat sourceProcedure:1. Wear safety goggles, lab coat, and gloves to ensure personal safety.2. Measure 2-3 silver coins or pellets and place them in a test tube.3. Add 2-3 mL of concentrated nitric acid to the test tube containing the silver.4. Observe the reaction. The silver will react with the nitric acid to form a brown gas (NO2) and a white precipitate (silver nitrate).5. Continue adding concentrated nitric acid to the reaction mixture until the precipitate stops forming.6. Allow the reaction mixture to cool to room temperature.7. Once cooled, carefully add 10 mL of distilled water to the test tube.8. Stir the solution with a glass rod to dissolve the silver nitrate.9. Transfer the solution to a beaker and heat it gently over a Bunsen burner to remove any remaining nitric acid fumes.10. Once the fumes have dissipated, allow the solution to cool to room temperature.11. Transfer the solution to a clean, labeled container for storage.Results:The reaction between silver and concentrated nitric acid produced a white precipitate, which was identified as silver nitrate. The solution turned light brown due to the formation of nitrogen dioxide gas (NO2). The precipitate was observed to be insoluble in water.Discussion:In this experiment, the reaction between silver and concentrated nitric acid was a single displacement reaction. The silver atoms replaced the hydrogen atoms in the nitric acid, forming silver nitrate and nitrogen dioxide gas. The balanced chemical equation for the reaction is:2Ag(s) + 4HNO3(aq) → 2AgNO3(aq) + 2NO2(g) + 2H2O(l)The white precipitate observed was silver nitrate, which is a sparingly soluble salt. The light brown color of the solution was due to the formation of nitrogen dioxide gas, which is a colorless gas under normal conditions but turns brown when dissolved in water.Conclusion:The experiment successfully synthesized silver nitrate by reactingsilver with concentrated nitric acid. The reaction produced a white precipitate, which was identified as silver nitrate. The experiment demonstrated the principles of single displacement reactions and the properties of silver nitrate. It also emphasized the importance of safety precautions when handling hazardous chemicals.References:1. Chang, R. (2016). Chemistry. 13th ed. New York, NY: McGraw-Hill Education.2. Silberberg, M. S. (2016). Chemistry: The Central Science. 14th ed. New York, NY: McGraw-Hill Education.。

英文版化学实验报告(最新整理)

Preparation of n -bromobutane一、Purpose1、Study the principle and method of preparing n-butyl bromide from n-butyl alcohol by treatment with sodium bromide and concentrated sulfuric acid2、Learn the technique of reflux with a gas trap apparatus and washing.二、Principlen-Butyl bromide can be easily prepared by allowing n-butyl alcohto react with sodium bromide and concentrated sulfuric acid.Main reactions ：NaBr + H 2SO4 → HBr + NaHSO424H SO 322232222CH CH CH CH OH HBr CH CH CH CH Br H O+−−−→+Secondary reactions ：；24H SO 32223222CH CH CH CH OH CH CH CH=CH H O−−−→+()24H SO 32223222222CH CH CH CH OH CH CH CH CH O H O−−−→+24222H SO HBr Br SO H O+−−→++三、Materials n-butyl alcohol ：4mL Sodium bromide ：5gConcentrated sulfuric acid ：2.5mL/6mL Anhydrous calcium chloride:0.5g 10% aqueous sodium hydroxide:5mL四、Primary reagent And Product physical constantsNameRelativemolecularmassCharacter RelativedensityMeltingpointBoilingpointRefractiveindexn-bromobutane137.03colorless andtransparentliquid1.299-122.4101.6 1.4399n-butyl alcohol74.12colorless andtransparentliquid0.8098-89.2117.7 1.3993五、Apparatus六、Procedure（1）50mLboiling flask+50mLwater+6mLconcentrated sulfuric acid Cool down（2）Assembling equipment(3) Stop and simple distill(4)(5)七、Experimental records(1) Sulfuric acid soluble in water gives off a lot of heat(2) The solution of the distillation flask become yellow and the sodium bromide dissolve(3)Solution is divided into two layers and liquid of the distillation become clear(4) Liquid layer, upper as the water phase, the lower is positive bromobutane and liquid for the milky haze(5) Liquid at 99 ℃ and stable distillation, after rising to 103 ℃, 103 ℃after fractions and the former part of the don't mix.八、Data recordingOutput:1.3g theoretical yield:5.8g productivity:21.7% Character: colorless and transparent liquid Refractive index:1.4372九、Experiment Discussion1、Turbidity is because it contains a variety of organic phase to organicimpurities2、Plus the bottle stopper of calcium chloride anhydrous dry battery inorder to prevent the water vapor in the air into the conical flask, at the same time prevent product turbidity。

化学实验报告模板(完整版)

报告编号：YT-FS-8761-61化学实验报告模板(完整版)After Completing The T ask According To The Original Plan, A Report Will Be Formed T o Reflect The Basic Situation Encountered, Reveal The Existing Problems And Put Forward Future Ideas.互惠互利共同繁荣Mutual Benefit And Common Prosperity化学实验报告模板(完整版)备注：该报告书文本主要按照原定计划完成任务后形成报告，并反映遇到的基本情况、实际取得的成功和过程中取得的经验教训、揭露存在的问题以及提出今后设想。

文档可根据实际情况进行修改和使用。

实验步骤(1) 在试管中加入5mL5%的过氧化氢溶液，把带火星的木条伸入试管;(2) 加热实验(1)的试管，把带火星的木条伸入试管;(3) 在另一支试管中加入5mL5%的过氧化氢溶液，并加入2g二氧化锰，把带火星的木条伸入试管;(4) 待实验(3)的试管内液体不再有现象发生时，重新加热3mL5%的过氧化氢溶液，把带火星的木条伸入试管;(该步骤实验可以反复多次)(5) 实验后将二氧化锰回收、干燥、称量。

实验现象及现象解释：实验编号实验现象现象解释(1) 木条不复燃(2) 木条不复燃 H2O2分解O2速度太慢没足够的O2试木条复燃.(3) 3H2O2产生大量气泡木条复燃 MnO2使H2O2加速分解O2,O2使木条复然(4) 新加入的H2O2产生大量气泡因为MnO2继续作为催化挤的作用!H2O2继续分解(5) 5MnO2的质量不变因为MnO2是催化剂所以只是改变化学反应速度,不改变其化学性质和质量这里填写您企业或者单位的信息Fill In The Information Of Your Enterprise Or Unit Here。

化学英语实验报告

化学英语实验报告Title: Experiment Report: Investigating the Effects of pH on Enzyme Activity Introduction:Enzymes are biological catalysts that play a crucial role in the chemical reactions occurring within living organisms. The activity of enzymes is influenced by various factors, including pH. In this experiment, we aimed to investigate the effects of pH on enzyme activity using the enzyme catalase and hydrogen peroxide as the substrate.Materials and Methods:1. Catalase solution2. Hydrogen peroxide solution3. Test tubes4. pH buffer solutions (pH 4, 7, and 10)5. Graduated cylinder6. Stopwatch7. Water bath8. PipettesThe experiment was carried out by preparing three sets of test tubes, each containing catalase solution and hydrogen peroxide solution. To each set, a different pH buffer solution (pH 4, 7, or 10) was added to create the desired pH environment. The reactions were then initiated by adding the hydrogen peroxide solution to the catalase solution, and the time taken for thedisappearance of bubbles (indicating the breakdown of hydrogen peroxide by catalase) was recorded using a stopwatch. This process was repeated for each pH condition.Results:The results of the experiment showed that the rate of enzyme activity varied with pH. The fastest reaction occurred at pH 7, while the reaction rates at pH 4 and pH 10 were slower.Discussion:The findings of this experiment demonstrate the significant impact of pH on enzyme activity. Enzymes have an optimal pH at which they exhibit maximum activity, and deviations from this pH can lead to a decrease in enzyme efficiency. In the case of catalase, the optimal pH is around 7, which is close to the physiological pH of most living organisms.Conclusion:In conclusion, this experiment highlights the importance of pH in regulating enzyme activity. Understanding the effects of pH on enzyme function is essential for various fields, including medicine, biochemistry, and biotechnology. Further research in this area could lead to the development of novel enzyme-based technologies and therapies.。

1、下载文档前请自行甄别文档内容的完整性，平台不提供额外的编辑、内容补充、找答案等附加服务。
2、"仅部分预览"的文档,不可在线预览部分如存在完整性等问题,可反馈申请退款(可完整预览的文档不适用该条件!)。
3、如文档侵犯您的权益，请联系客服反馈,我们会尽快为您处理(人工客服工作时间：9:00-18:30)。

Preparation of n -bromobutane
一、Purpose
1、Study the principle and method of preparing n-butyl bromide from n-butyl alcohol by treatment with sodium bromide and concentrated sulfuric acid
2、Learn the technique of reflux with a gas trap apparatus and washing.
二、Principle
n-Butyl bromide can be easily prepared by allowing n-butyl alcohto react with sodium bromide and concentrated sulfuric acid. Main reactions ：
NaBr + H 2SO4 → HBr + NaHSO4
24
H SO 322232222CH CH CH CH OH HBr CH CH CH CH Br H O +−−−→+
Secondary reactions ：
24H SO 32223222CH CH CH CH OH CH CH CH=CH H O
−−−→+； ()24H SO 32223222222CH CH CH CH OH CH CH CH CH O H O
−−−→+
24222H SO HBr Br SO H O
+−−→++
三、Materials n-butyl alcohol ：4mL Sodium bromide ：5g
Concentrated sulfuric acid ：2.5mL/6mL Anhydrous calcium chloride:0.5g 10% aqueous sodium hydroxide:5mL
四、Primary reagent And Product physical constants
五、Apparatus
六、Procedure
（1）50mLboiling flask+50mLwater+6mLconcentrated sulfuric acid Cool down
（2）Assembling equipment
(3) Stop and simple distill (4)
(5)
七、Experimental records
(1) Sulfuric acid soluble in water gives off a lot of heat
(2) The solution of the distillation flask become yellow and the sodium bromide dissolve
(3)Solution is divided into two layers and liquid of the distillation become clear
(4) Liquid layer, upper as the water phase, the lower is positive bromobutane and liquid for the milky haze
(5) Liquid at 99 ℃ and stable distillation, after rising to 103 ℃, 103 ℃after fractions and the former part of the don't mix.
八、Data recording
Output:1.3g theoretical yield:5.8g productivity:21.7% Character: colorless and transparent liquid Refractive index:1.4372
九、Experiment Discussion
1、Turbidity is because it contains a variety of organic phase to organic
impurities
2、Plus the bottle stopper of calcium chloride anhydrous dry battery in
order to prevent the water vapor in the air into the conical flask, at the same time prevent product turbidity。

英文版化学实验报告

化学震荡实验报告（完整版）

化学实验报告全英

化学实验报告 英文版

化学实验报告英语

英文版化学实验报告

化学实验报告常见英文

化学性质实验报告

生物化学实验报告参考模板

最新有机化学实验实验报告

化学实验报告英文版

分析化学实验报告范文(完整版)

英文实验报告化学

【优质文档】化学英语实验报告-实用word文档 (5页)

化学实验报告_英文

关于英文版化学实验报告

英文版的化学实验报告

化学实验报告英语作文(3篇)

英文版化学实验报告(最新整理)

化学实验报告模板(完整版)

化学英语实验报告

化学实验报告英文版