First slide

Solubility product(KSP)

Question

In a saturated aqueous solution of AgBr, conc. of Ag⁺ ion is 1× 10^–6 mol/lit. If K_sp for AgBr is 1×10^–12, then concentration of Br^– in the solution is

Easy

A

$1 \times 10^{- 6} mol / lit$
B

$4 \times 10^{- 8} mol / lit$
C

$4 \times 10^{- 7} mol / lit$
D

$4 \times 10^{- 19} mol / lit$

Solution

$[{Ag}^{+}] [{Br}^{-}] = K_{sp}$
At saturation, K_IP=K_SP
$\Rightarrow 10^{- 6} \times [{Br}^{-}] = 10^{- 12}$
$\Rightarrow [{Br}^{-}] = 10^{- 6}$

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