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 0.03mol X 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%.
第二篇：化学实验预习报告
化学实验预习报告
班级 小组成员
实验名称：海带中碘元素的分离及提存（检验）
一、实验目的：
二、实验原理：
1、查资料知海带中碘元素主要为I-形式存在， 少量以有机碘和IO3- 存在。
2、可使用某些 剂（如 ）将I-转化为I2，然后检验I2的存在，并分离I2，有关反应的离子方程式为（任写一条）：
3、可使用 溶液检验I2，用 萃取并 方法分离出I2。
三、实验步骤：
实验几个注意之处
１、海带已经称取好
２、灼烧灰化的过程大约需要5—6分钟，干海带逐渐变成黑色粉末或细小颗粒即可
３、用坩埚钳夹持坩埚，边加热边用玻璃棒搅拌，以使海带充分灼烧，加快灰化的速度。
４、移动坩埚时必须使用坩埚钳，避免烫伤
５、灼烧完毕，应将坩埚、玻璃棒放在石棉网上冷却，不可直接放在冷的实验台上，防止温度很高的坩埚骤冷而破裂
６、过滤操作应注意“一贴、二低、三靠”
７、用约1mL蒸馏水洗涤沉淀得滤液
８、使用分液漏斗之前应先检漏和洗涤
９、萃取后打开上口的塞子或将旋塞的凹槽对准上口的小孔，静置，待完全分层后，分液。