Solid Ba(NO₃)₂ is gradually dissolved in 1×10^{-4}, M, Na₂CO₃ solution. At what concentrati

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6-2.Equilibrium-II (Ionic Equilibrium)

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Solid $Ba(NO_3)_2$ is gradually dissolved in $1\times10^{-4}\, M\, Na_2CO_3$ solution. At what concentration of $Ba^{+2}$ the precipitation of $BaCO_3$ will start? (If $K_{sp}$ of $BaCO_3 = 5.1\times10^{-9}$)

A

$4.1\times10^{-5}\, M$

B

$5.1\times10^{-5}\, M$

C

$1.6\times10^{-4}\, M$

D

$8.1\times10^{-7}\, M$

Solution

$\left[\mathrm{Ba}^{+2}\right]\left(10^{-4}\right)=5.1 \times 10^{-9}$

$\boxed{\left[ {{\text{B}}{{\text{a}}^{ + 2}}} \right] = 5.1 \times {{10}^{ – 5}}{\mkern 1mu} {\text{M}}}$

Standard 11

Chemistry

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