Calculate the solubility of AgI in a solution containing 0.30 M NaI (Ksp = 8.3 × 10^-17).
I can't seem to get this problem right.
I can't seem to get this problem right.
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Ksp=[Ag+][I-]
8.3 × 10^17=0.30M*s
s=2.8 x10^18
(2.8 x10^18/1L)(234.8g AgI/1mol)=6.57x10^20g/L solubility of AgI in NaI
solution.
Hope this helps
8.3 × 10^17=0.30M*s
s=2.8 x10^18
(2.8 x10^18/1L)(234.8g AgI/1mol)=6.57x10^20g/L solubility of AgI in NaI
solution.
Hope this helps