Concentration of Ba^{2+} when BaF₂,(K_{sp} = 1.0 × 10^{-6} ) begins to precipitate from a solutio

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6-2.Equilibrium-II (Ionic Equilibrium)

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What is the concentration of $Ba^{2+}$ when $BaF_2\,(K_{sp} = 1.0 \times 10^{-6}$) begins to precipitate from a solution that is $0.30\, M\, F^-$ ?

A

$9.0 \times {10^{ - 7}}$

B

$3.3 \times {10^{ - 5}}$

C

$1.1 \times {10^{ - 5}}$

D

$3.0 \times {10^{ - 7}}$

Solution

$BaF _2( s ) \rightleftharpoons Ba ^{2 + }( aq )+2 F ( aq )$

$s\quad 0.3\, m$

Let $S$ be the concentration of $Ba ^{2+}$,

$K _{ sp }=\left[ Ba^{2+}\right]\left[ F ^{-}\right]^2$

$1.0 \times 10^{-6}= S \times(0.3)^2$

$1.1 \times 10^{-5}= S$

Standard 11

Chemistry

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