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Q.

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

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a

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

b

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

c

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

d

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

answer is A.

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Detailed 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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