AgCl(s) --------------------------> Ag^+ (aq) + Cl^- (aq) s s ksp = [Ag^+][Cl^-]
ID: 700201 • Letter: A
Question
AgCl(s) --------------------------> Ag^+ (aq) + Cl^- (aq)
s s
ksp = [Ag^+][Cl^-]
1.77*10^-10 = s*s
s^2 = 1.77*10^-10
s = 1.33*10^-5 M
the molar solubility of solution is 1.33*10^-5 M in water
b. NaCl(aq) ------------------> Na^+ (aq) + Cl^- (aq)
0.08 M 0.08M
AgCl(s) --------------------------> Ag^+ (aq) + Cl^- (aq)
s s+0.08
ksp = [Ag^+][Cl^-]
1.77*10^-10 = s*(s+0.08)
1.77*10^-10 = s*0.08 [0.08>>>s ,S+ 0.08 = 0.08]
s = 1.77*10^-10/0.08 = 2.2125*10^-9 M
The solubility of AgCl in NaCl is 2.2125*10^-9 M
Explanation / Answer
Calculate the molar solubility of AgCl (Ksp 1.77 x 10-10) in (a) pure water. (b) 0.08 M NaCl