\"In this experiment, you will study the equilibrium conditions of six different

Question

"In this experiment, you will study the equilibrium conditions of six different reactions. You will first establish the equilibrium by mixing the solutions provided for each reaction and then add reagents in order to perturb the established equilibrium. Each time that you cause a change in the equilibrium, you will observe the changes (look for evidence of reaction), write a net ionic equation illustrating the changes and then comment on how the reaction rate is affected, either the forward or reverse reaction rate. The goal is to learn how equilibria respond to changes in concentrations and changes in temperature"

Here is the 3rd reaction

Just solve A through J. Each answer is like a line, so should be straight forward:

I already did one for reference:

3. Reagents 0.1 MAgNO, 6 MNaci, 6 MNH3 AgCl 22 NH 3 (aq) (aa) ion diamminesilver(I) white a. Silver chloride produced by b. Net Ionic Equation c. Equilibrium shifted to the right by d. Observation e. Net Ionic Equation Reason for shift g. Equilibrium shifted to the left by h. Observation i. Net Ionic Equation Reason for shift CT aq) (EQ 17.13)

Explanation / Answer

3. For the reaction,

AgCl + 2NH3 <==> [Ag(NH3)2]+ + Cl-

a. Silver chloride produced by reaction of [Ag(NH3)]+ and HCl

b. Net ionic equation : [Ag(NH3)2]+ + Cl- <==> AgCl(s) + 2NH3

c. Equilibrium shifted to right by addition of NH3 to the solution.

d. Observation : solubilization of AgCl(s) occured and [Ag(NH3)2]+ is formed.

e. Nei-ionic equation : AgCl(s) + 2NH3 ----> [Ag(NH3)2]+ + Cl-

f. As more NH3 is added, it forces formation of soluble complex by dissolution of AgCl.

q. Equilibrium shifted to the left by adding more HCl to the solution.

h. More precipitation of AgCl occurs.

i. As more Cl- is added, the reaction is pushed to right and more AgCl(s) is generated. This is according to LeChatellier's principle.

j. net ionic equation : [Ag(NH3)2]+ + Cl- <==> AgCl(s) + 2NH3

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