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]