(D) The dissociation of $BaSO_4$ is given by: $BaSO_4(s) ⇌ Ba^{2+}(aq) + SO_4^{2-}(aq)$ Let the solubility be $S \ mol \ L^{-1}$. Then,$[Ba^{2+}] = S$

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$3.6 \times 10^{-5} \ mol \ L^{-1}$

(D) The dissociation of $BaSO_4$ is given by: $BaSO_4(s) ⇌ Ba^{2+}(aq) + SO_4^{2-}(aq)$ Let the solubility be $S \ mol \ L^{-1}$. Then,$[Ba^{2+}] = S$ and $[SO_4^{2-}] = S$. The solubility product expression is: $K_{sp} = [Ba^{2+}][SO_4^{2-}] = S \times S = S^2$ Given $K_{sp} = 1.3 \times 10^{-9}$. $S^2 = 1.3 \times 10^{-9} = 13 \times 10^{-10}$ $S = \sqrt{13 \times 10^{-10}} \approx 3.6 \times 10^{-5} \ mol \ L^{-1}$

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium Solubility product

Medium

The solubility product of $BaSO_4$ is $1.3 \times 10^{-9}$. The solubility of this salt in pure water will be

A
$1.69 \times 10^{-9} \ mol \ L^{-1}$
B
$1.69 \times 10^{-18} \ mol \ L^{-1}$
C
$3.6 \times 10^{-18} \ mol \ L^{-1}$
D
$3.6 \times 10^{-5} \ mol \ L^{-1}$

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2 Equilibrium: Ionic Equilibrium

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Solubility product

$Mg(OH)_2$ is precipitated when $NaOH$ is added to a solution of $Mg^{2+}$. If the final concentration of $Mg^{2+}$ is $10^{-10} \ M$,the concentration of $OH^{-} \ (M)$ in the solution is (Given: Solubility product for $Mg(OH)_2 = 5.6 \times 10^{-12}$)

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In the reaction $Fe(OH)_{3(s)} \rightleftharpoons Fe^{3+}_{(aq)} + 3OH^{-}_{(aq)}$, if the concentration of $OH^{-}$ ions is decreased by $\frac{1}{4}$ times, then the equilibrium concentration of $Fe^{3+}$ will increase by: (in $\times$)

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Why is only $As^{3+}$ precipitated as $As_2S_3$ when $H_2S$ is passed through an acidic solution containing $As^{3+}$ and $Zn^{2+}$,while $Zn^{2+}$ is not precipitated as $ZnS$?

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The solubility product of $AgI$ at $25\,\text{°C}$ is $1.0 \times 10^{-16}\,\text{mol}^2\,\text{L}^{-2}$. The solubility of $AgI$ in $10^{-4}\,\text{N}$ solution of $KI$ at $25\,\text{°C}$ is approximately (in $\text{mol L}^{-1}$)

MediumAIPMT 2003

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Which of the following compounds is sparingly soluble in ammonia?

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The solubility product of $BaSO_4$ is $1.3 \times 10^{-9}$. The solubility of this salt in pure water will be

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$Mg(OH)_2$ is precipitated when $NaOH$ is added to a solution of $Mg^{2+}$. If the final concentration of $Mg^{2+}$ is $10^{-10} \ M$,the concentration of $OH^{-} \ (M)$ in the solution is (Given: Solubility product for $Mg(OH)_2 = 5.6 \times 10^{-12}$)

In the reaction $Fe(OH)_{3(s)} \rightleftharpoons Fe^{3+}_{(aq)} + 3OH^{-}_{(aq)}$, if the concentration of $OH^{-}$ ions is decreased by $\frac{1}{4}$ times, then the equilibrium concentration of $Fe^{3+}$ will increase by: (in $\times$)

Why is only $As^{3+}$ precipitated as $As_2S_3$ when $H_2S$ is passed through an acidic solution containing $As^{3+}$ and $Zn^{2+}$,while $Zn^{2+}$ is not precipitated as $ZnS$?

The solubility product of $AgI$ at $25\,\text{°C}$ is $1.0 \times 10^{-16}\,\text{mol}^2\,\text{L}^{-2}$. The solubility of $AgI$ in $10^{-4}\,\text{N}$ solution of $KI$ at $25\,\text{°C}$ is approximately (in $\text{mol L}^{-1}$)

Which of the following compounds is sparingly soluble in ammonia?

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