Laboratory work

 

La Chatelier's Principle

Purpose of the work:

The purpose of this lab was to observe the effects of concentration and temperature on equilibrium and to visualize how balance can be restored based on La Chatelier's Principle.

 

Materials:

·         Cobalt (II) chloride hexahydrate

·         Hydrochloric acid concentrated

·         Beaker

·         Cold water

·         Heat water

 

Procedures:

1.      Take 4 g of solid cobalt(II) chloride-6-water and dissolve it in 40 ml of water in a 250 ml heat resistant beaker. You have a light pink solution.

2.      Put the beaker on a magnetic mixer, dip a stir bar into the solution and turn on the mixing and heating. Effect of concentration:

3.      Add about 60 mL of concentrated hydrochloric acid to the beaker. You have a violet or blue solution. The color of the mixture depends on the ration between the acid and cobalt(II) chloride.

4.      Add a small amount of water to the beaker to make the solution pink.

5.      Add a small amount of hydrochloric acid to the beaker to make the solution blue. Effect of temperature:

6.      Make the solution pink. Place the beaker in the hot water. The solution became blue.

7.      Place the beaker in the ice. The solution became pink.

8.      Write the chemical equation for this reaction, in which complex ions form between CO2+ and either water molecules or chloride ions

 

Questions:

1.      Name these complex compounds and specify the complex constructor ions. Determine the charge and coordination numbers of complex-forming ions: K2[Cu(CN)4];   [Ni(NH3)6]SO4;   K2[PtCI6]; K[AuCI4]; [Cr(NH3)4CO3]CI;  Zn[Ni(CN)4]; [Co(NH3)4(SCN)2]CI

2.      Please indicate and describe the cationic, anionic, and neutral complex salts from these salts:          K3 [ AI(OH)6]; [ Cd ( NH3)4] CI2; [ Ag ( NH3)2] NO3; [ Cо (NН3)3 (NО2)3]; [Pt CI4(NH3)2]; Na3 [FeF6]