First slide

Solubility product(KSP)

Question

Solubility product of AgCl is $1.8 \times 10^{- 10} M^{2}$ . Molar solubility of AgCl in 0.1 M NaCl solution will be

Moderate

A

$1.8 \times 10^{- 11}$
B

$1.8 \times 10^{- 9}$
C

$1.8 \times 10^{- 12}$
D

$1.8 \times 10^{- 6}$

Solution

$\begin{matrix} AgCl (s) ⇌ \underset{S}{{Ag}^{+}} (aq) + \underset{S}{{Cl}^{-}} (aq); \\ NaCl (aq) \to {Na}^{+} (0.1 M) + {Cl}^{-} (0.1 M); \end{matrix}$
$\begin{matrix} K_{sp} = [{Ag}^{+}] [{Cl}^{-}] \\ 1.8 \times 10^{- 10} = [s] [s + 0.1 M] \\ s < < < 0.1 M \\ 1.8 \times 10^{- 10} = [s] [0.1 M]; \\ s = 1.8 \times 10^{- 9} M; \end{matrix}$

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