Report: Chemical Reaction and Solution

Topics: Chemical reaction, PH, Hydrochloric acid Pages: 29 (4801 words) Published: November 12, 2013


LAB REPORT

Group: 6
Section:
Group member: Phạm Thanh Thủy ID: BTARIU12005
Course name : GENERAL CHEMISTRY LABORATORY
Period : 2012-2013
Date performed : 11-03-2013
Date submitted : 02-05-2013
INSTRUCTOR’S NAME : Hoàng Lê Sơn

EXPERIMENT 1:
CHEMICAL REACTIONS

I. INTRODUCTION – OBJECTIVES
In this first experiment, we will perform 8 chemical reactions and 1 flame test in order to determine 2 things : a) firstly, we can know whether a reaction occurred or not. To complete our mission, we need to observe carefully some signs of chemical reaction’s appearance such as the change in color of solution, precipitate’s existence, the release of gas, also check the change of heat and light. b) secondly, we need to have knowledge about 5 types of reactions and then put experiments below into practice classify type of each reaction. Furthermore, we also learn how to describe chemical changes carefully, beside that we will practice again writing and balancing chemical equations skills.

II. MATERIALS AND EQUIPMENTS
EQUIPMENT

Thirty test tubes
One test tube rack
Two test tube holders
Two spatulas
Three 250 mL beakers
One stirring rod

One medicine dropper
Alcohol lamp or Busen burner
Water bath
One looped platinum or nichrome wire
Label

REAGENTS

0.5 M CaCl2
0.5 M BaCl2
M NaOH
0.1 M AgNO3
0.5 M KCl
0.5 M KBr
0.5 M KI
2 M NH4OH
M KCN
% H2O2
2 M H2SO4
MnO2
Saturated FeSO4
0.1 M NaNO3

CH3COOH
0.5 M Na2SO3
0.1 M KSCN
2 N KOH
0.5 M K4[Fe(CN)6]
0.5 M FeSO4
0.5 M FeCl3
0.5 M Al2(SO4)3
2 N HCl
0.5 M LiCl
0.5 M NaCl
0.5 M KCl
0.5 M K2Cr2O7
96% H2SO4

III. EXPERIMENTAL PROCEDURE
1. Reactions of Cu2+
10 drops of 2 M NaOH, 2 M NH4OH, 0.5 M K4[Fe(CN)6] was added in turn order into each of test tube which had contained 10 drops of 0.5 M CuSO4. Record the change solution’s color and precipitate’s existence.

2. Reactions of silver halides
Step1: 10 drops of three 0.5 M solution of KCl, KBr, KI was firstly added into each test tubes, then 10 drops of 0.1 M AgNO3 was added into these salt solutions. Observe the change solution’s color, forming of precipitation. Step2: Solution in each of test tube was devided into two equal parts. 5 drops of 2 M NH4OH was added to 3 tubes from step1. Other 5 drops of 2 M KCN was added to 3 remaining tubes. Then record the signs of reaction such as solution’s discolorment and existence of precipitates. 3. Reactions of H2O2

Step1: A test tube which contained 5 drops of 0.1 M KMnO4 was acidified with 5 drops of 2 M H2SO4, then 5 drops of 3% H2O2 also was added to this solution. The color change of solution and gas’s release are recorded. Step2: 5 drops of 0.1 M KI was substituted for KMnO4 . then both the solution’s change of color and the release of gas also be recorded again. Step3: A piece of solid MnO2 was released into 1 mL of H2O2 solution. The release of gas must be observed carefully. 4. Reactions of Nitrate

Step1: A 1 mL of saturated FeSO4 was added into a test tube which had contained 1 mL of 1 M NaNO3 solution. Sufficient amount of concentrated sulfuric acid (96%) was poured carefully down the inside wall of this test tube. Observe and record the change of color at the interface between the nitrate solution and the concentrated sulfuric acid after a few seconds. Step2: NaNO2 was substituted for FeSO4

Step3: acetic acid was substitute for H2SO4
Record the observation and then compare with the system.
5. Reactions of KMnO4
5 drops of 2 M H2SO4, 6N NaOH, distilled water was added in turn order into each of test tube which had contained 10 drops of 0.5 M Na2SO3. Then 5 drops of 0.1 M KMnO4 was added to each of test tube finally. Record the change solution’s color and precipitate existence. 6. Reaction of Potassium Dichromate (K2Cr2O7)

10 drops of 0.5 M K2Cr2O7 was added into a test tube, then next 10 drops of H2SO4 was added. Finally, 5 drops of...
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