Solid Ba(NO₃)₂ is gradually dissolved in 1.0 × 10^{-4} ,M ,Na₂CO₃ solution. At which

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6-2.Equilibrium-II (Ionic Equilibrium)

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Solid $Ba(NO_3)_2$ is gradually dissolved in $1.0 \times 10^{-4} \,M \,Na_2CO_3$ solution. At which concentration of $Ba^{2+}$ the precipition will begin? ( $K_{sp}$ $BaCO_3 = 5.1 \times 10^{-9}$)

A

$4.1 \times 10^{-5} \,M$

B

$5.1 \times 10^{-5} \,M$

C

$8.1 \times 10^{-8} \,M$

D

$8.1 \times 10^{-7} \,M$

Solution

$\mathrm{K}_{\mathrm{sp}}=\left[\mathrm{Ba}^{2+}\right]\left[\mathrm{CO}_{3}^{-}\right]$

$5.1 \times 10^{-9}=\left[\mathrm{Ba}^{2+}\right] \times 1 \times 10^{-4}$

$5.1 \times 10^{-5}=\left[\mathrm{Ba}^{2+}\right]$

Standard 11

Chemistry

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