Reference no: EM132573892

1)Calculate the molar solubility of AgBr and the concentration of [Ag+] and [Br-] in the water solution.  

Ksp = 7.7 x 10^-13

2)Using Q, determine if PbI₂ precipitates from a solution that has the concentrations indicated?  Ksp = 1.4 x 10^-8 

PbI₂  in a solution with

[Pb²⁺] = 0.003 M and [I^-] = 1.3 ×10^-3 M

a)Q < Ksp

b)Q > Ksp

3)Using Q, determine if Ag₂S precipitates from a solution that has the concentrations indicated?

Ksp = 1.6 x 10^-49

[Ag⁺] = 1 ×10^-10 M

[S^2-] = 1 × 10^-13 M

a)Q > Ksp means a precipitate will form

b)Q < Ksp means a precipitate will not form

4)If we had a reaction, like below, determine what would happen if you added PO₄^3- ion to the solution?

FePO₄(s)  Fe³⁺(aq) + PO₄^3- (aq)

a)Reaction would go forwards to reach equilibrium. →

b)Reaction would go backwards to reach equilibrium. ←

5)Which is the Lewis Acid and Lewis Base in the following equation?

I^-+SnI₂?SnI₃^-

a) I^- is the Lewis Base

SnI₂   is the Lewis Acid

b)I^- is the Lewis Acid

SnI₂   is the Lewis Base