(A) The dissociation of the salt $B_3A_2$ is given by: $B_3A_{2(s)} \rightleftharpoons 3B^{2+} + 2A^{3-}$ Let the solubility be $S \ mol \ L^{-1}$. Th

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$S = \left( \frac{K_{sp}}{108} \right)^{\frac{1}{5}}$

(A) The dissociation of the salt $B_3A_2$ is given by: $B_3A_{2(s)} \rightleftharpoons 3B^{2+} + 2A^{3-}$ Let the solubility be $S \ mol \ L^{-1}$. Then,$[B^{2+}] = 3S$ and $[A^{3-}] = 2S$. The solubility product expression is: $K_{sp} = [B^{2+}]^3 [A^{3-}]^2$ Substituting the values: $K_{sp} = (3S)^3 (2S)^2$ $K_{sp} = (27S^3) \times (4S^2)$ $K_{sp} = 108S^5$ Solving for $S$: $S^5 = \frac{K_{sp}}{108}$ $S = \left( \frac{K_{sp}}{108} \right)^{\frac{1}{5}}$

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Solubility product

Easy

Which from the following equations represents the relation between solubility ($S$ in $mol \ L^{-1}$) and solubility product $(K_{sp})$ for a salt $B_3A_2$?

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A
$S = \left( \frac{K_{sp}}{108} \right)^{\frac{1}{5}}$
B
$S = \left( 108 \times K_{sp} \right)^{\frac{1}{5}}$
C
$S = \left( \frac{K_{sp}}{27} \right)^{\frac{1}{5}}$
D
$S = \left( 27 \times K_{sp} \right)^{\frac{1}{5}}$

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If the $pH$ of a $0.001 \, M \, Mg(NO_3)_2$ solution is $9$,will precipitation occur? Given the $K_{sp}$ of $Mg(OH)_2 = 8.9 \times 10^{-12}$.

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The solubility product of Lead sulphate,$PbSO_4$ is $1.3 \times 10^{-8}$. Calculate its solubility in pure water. The molecular mass of $PbSO_4 = 303 \ g \ mol^{-1}$.

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$A$ solution is saturated with $SrCO_3$ and $SrF_2$. The $[CO_3^{2-}]$ is found to be $1.2 \times 10^{-3} \ M$. The concentration of $F^{-}$ in the solution would be:
Given: $K_{sp}(SrCO_3) = 7.0 \times 10^{-10}$,$K_{sp}(SrF_2) = 7.9 \times 10^{-10}$

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If the solubility product of $PbS$ is $8 \times 10^{-28}$,then the solubility of $PbS$ in pure water at $298 \ K$ is $x \times 10^{-16} \ mol \ L^{-1}$. The value of $x$ is $\dots$.
[Given $\sqrt{2} = 1.41$]

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Formula Solubility product $(K_{sp})$
$AgBrO_3$ $2.5 \times 10^{-10}$
$MgSO_4$ $2.7 \times 10^{-27}$
$CaCO_3$ $2.7 \times 10^{-18}$
$FeC_2O_4$ $2.4 \times 10^{-15}$
Which of the following salts has the maximum solubility?

Formula	Solubility product $(K_{sp})$
$AgBrO_3$	$2.5 \times 10^{-10}$
$MgSO_4$	$2.7 \times 10^{-27}$
$CaCO_3$	$2.7 \times 10^{-18}$
$FeC_2O_4$	$2.4 \times 10^{-15}$

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Which from the following equations represents the relation between solubility ($S$ in $mol \ L^{-1}$) and solubility product $(K_{sp})$ for a salt $B_3A_2$?

Similar Questions

If the $pH$ of a $0.001 \, M \, Mg(NO_3)_2$ solution is $9$,will precipitation occur? Given the $K_{sp}$ of $Mg(OH)_2 = 8.9 \times 10^{-12}$.

The solubility product of Lead sulphate,$PbSO_4$ is $1.3 \times 10^{-8}$. Calculate its solubility in pure water. The molecular mass of $PbSO_4 = 303 \ g \ mol^{-1}$.

$A$ solution is saturated with $SrCO_3$ and $SrF_2$. The $[CO_3^{2-}]$ is found to be $1.2 \times 10^{-3} \ M$. The concentration of $F^{-}$ in the solution would be: Given: $K_{sp}(SrCO_3) = 7.0 \times 10^{-10}$,$K_{sp}(SrF_2) = 7.9 \times 10^{-10}$

If the solubility product of $PbS$ is $8 \times 10^{-28}$,then the solubility of $PbS$ in pure water at $298 \ K$ is $x \times 10^{-16} \ mol \ L^{-1}$. The value of $x$ is $\dots$.[Given $\sqrt{2} = 1.41$]

FormulaSolubility product $(K_{sp})$$AgBrO_3$$2.5 \times 10^{-10}$$MgSO_4$$2.7 \times 10^{-27}$$CaCO_3$$2.7 \times 10^{-18}$$FeC_2O_4$$2.4 \times 10^{-15}$Which of the following salts has the maximum solubility?

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$A$ solution is saturated with $SrCO_3$ and $SrF_2$. The $[CO_3^{2-}]$ is found to be $1.2 \times 10^{-3} \ M$. The concentration of $F^{-}$ in the solution would be:
Given: $K_{sp}(SrCO_3) = 7.0 \times 10^{-10}$,$K_{sp}(SrF_2) = 7.9 \times 10^{-10}$

If the solubility product of $PbS$ is $8 \times 10^{-28}$,then the solubility of $PbS$ in pure water at $298 \ K$ is $x \times 10^{-16} \ mol \ L^{-1}$. The value of $x$ is $\dots$.
[Given $\sqrt{2} = 1.41$]

Formula Solubility product $(K_{sp})$
$AgBrO_3$ $2.5 \times 10^{-10}$
$MgSO_4$ $2.7 \times 10^{-27}$
$CaCO_3$ $2.7 \times 10^{-18}$
$FeC_2O_4$ $2.4 \times 10^{-15}$
Which of the following salts has the maximum solubility?