Question

What is the pH of a saturated solution of silver hydroxide, given Ksp = 1.53×10-8?

Answer 1

$AgOH\leftrightharpoons$ Ag⁺ + OH^-

K_Sp= [Ag⁺][OH^-]

1.53×10^-8=(s)(s)

1.53×10^-8=s²

s=(1.53×10^-8)^1/2=1.23×10^-4 M=[OH^-]=[Ag⁺]

pH + pOH =14

pH = 14 - pOH = ?

First we calculate pOH= -log(OH^-)=

pOH = -log(1.23×10^-4)=3.91

pH + pOH =14

pH + 3.91=14

pH = 14-3.91=10.08 is the pH of a saturated solution of silver hydroxide