英文版化学实验报告

2020-10-08 报告

　　篇一：英文版化学实验报告

　　Title: Preparation of Fe scrap from waste

　　(NH4) 2SO4.FeSO4.6H2O

　　The purpose of the experiment

　　Learn 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)2SO4.FeSO4.6H2O 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 50ml 10ml, 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 resulting

　　ammonium sulfate and 5.3ml 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 and

　　then filtered under reduced pressure to stand finally dried, weighed and the yield was calculated. The results obtained 8.1g bluish powdery

　　crystals. Have this result we can calculate yield, starting with the first step we tried to know the amount of iron, should this we can calculate the theoretical sulfate ferrous sulfate is 0.03mol, then ferrous sulfate obtained by the

　　0.03molFeSO4 theoretical value of ammonium. FeSO4+（NH4）2SO4+6H2O=FeSO4.(NH4)2SO4.6H2O 0.03molX mol

　　X=0.03mol

　　m=XM=0.03molⅹ392g/mol=11.76g

　　Yield = the actual value of the formula is divided by the theoretical value by 100%.it will be calculated into the data obtained in a yield of 68.9%.

　　篇二：英文版化学实验报告

　　The preparation of alkali type copper carbonate

　　The first:the experiment purpose

　　1.Master the methods of alkali type copper carbonate prepared and principle

　　2.Through the design experiment to cultivate independent design ability and chemical research thinking

　　The second:the experimental principle

　　The 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 steps

　　1.Solution preparation

　　Disposes 0.5 mole of each litre acid sour coppers and sodium carbonate solution each 100 milliliters.

　　2.The feeding order and raw material compare the exploration

　　According to 2:1.6,2:2,2:2.4,2:2.8 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.

　　3.Temperature exploration

　　According 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.

　　4.According 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 items

　　Instrument and material: The balance, the beaker, the glass rod, the Volumetric flask, the test tube, the filter flask,the Buchner funnel, the Erlenmeyer flask

　　Chemicals: Copper carbonate, sodium sulfate

　　The fifth:the experimental result

　　1.By the step 2, the observation phenomenon optimum condition is equal to for the cupric sulfate compared to the sodium carbonate 2:2.4, the feeding order for joins the sulfuric acid copper solutions to the sodium carbonate solution in.

　　2.By the step 3, the observation phenomenon optimum temperature is 75 degrees Celsius

　　3.According to the copper sulfate solution than sodium carbonate

　　solution 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

　　0.5*0.02 X

　　2/(0.5*0.02)=1/X

　　X=0.005

　　M[Cu2(OH)2CO3]=0.005*222=1.11g

　　Productive rate:0.5/1.11*100%=45%

　　The sixth : Questions

　　1. Which cupric salt suit the system to take the cupric basic carbonate? Answer:Cu(NO)3 or CuSO4

　　2. 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 determination

　　one, the experimental goal

　　1、 the study silver nitrate standard solution configuration and the demarcation method

　　2、 the grasping law raises Si Fa to determine the chloride ion the method principle two, the experimental principle

　　With AgNO3 standard solution titration Cl - Ag + + Cl - = = AgCl，At ph 7.0 -10.5 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 reagents

　　Equipment 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 steps

　　Accurately moving 25 ml concentration is 0.7064 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 10.00 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 nitrate

　　standard solution titration to solution from yellow to pink is the end point. Record the consumption volume of silver nitrate

　　standard solution, parallel determination of 3, calculate the sodium chloride content in saline and relative mean deviation.

　　Fifth, data recording and processing

　　Formula: ρ = V×MrNaCl×CAgNO3 x 100

　　The average deviation d=0.01300 dr=d/ρ×100%=0.13%

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