Question

Determine the Ksp. This is what I have.

AgC2H3O2(s)↔ Ag+(aq) + C2H3O2-(aq)

[Ag+] = (12mL)(0.250M) = (M2)(20mL) = 0.15M

[C2H3O2-] = (8mL)(0.300M) = (M2)(20mL) = 0.12M

AgC2H3O2 ↔ Ag+(aq) + C2H3O2-(aq) Titrated with 42.31mL KSCN

I --    0.15 0.12

C. +x -x -x

E -- 0.11

Ag+(aq) + SCN-(aq) → AgSCN(s)

Moles SCN = 0.04231L * 0.05M = 0.002116

Moles Ag+ = 0.002116 [Ag+] = 0.002116 / 0.020L = 0.11

Ksp = [Ag+] = 1.1*10^-1

Answer 1

Let us consider the chemical reaction

	AgC2H3O2(s	↔	Ag+(aq) +	+ C2H3O2-(aq)
Initial	0		0.15M	0.12M
Reacted with KSCN			0.11
concetration present at equilibrium	0.04		0.11M	0.08 M

Moles of Ag+ present in solution at equilibrium = moles of Ag+ reacted with KSCN=0.002116

So concentation of Ag+ in solution at equilibrium =0.11 M (given)

Cooncentration of Ag+ reacted with C₂H₃O₂^-(aq) per liter= Initial concentration Ag+ - concentration of Ag+ remaining in the solution= 0.15-0.11 =0.04

Concentration of C₂H₃O₂^- reacted to form ppt =0.04 M

So concentation of C₂H₃O₂^- in solution at equilibrium = Initial concentration C₂H₃O₂^- - Concentration of C₂H₃O₂^- reacted= 0.12-0.04 M= 0.08

Now Ksp=Ag+C2H3O2-

Ksp=0.11×0.08= 0.0088