(B) The dissociation of calcium carbonate is given by: $CaCO_3(s) \rightleftharpoons Ca^{2+}(aq) + CO_3^{2-}(aq)$.Let the solubility be $s = 6.4 \time

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(B) The dissociation of calcium carbonate is given by: $CaCO_3(s) \rightleftharpoons Ca^{2+}(aq) + CO_3^{2-}(aq)$.Let the solubility be $s = 6.4 \times 10^{-5} \ mol \ dm^{-3}$.The solubility product constant is given by: $K_{sp} = [Ca^{2+}][CO_3^{2-}] = s \times s = s^2$.Substituting the value of $s$: $K_{sp} = (6.4 \times 10^{-5})^2$.$K_{sp} = 40.96 \times 10^{-10} = 4.096 \times 10^{-9}$.

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

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The solubility of calcium carbonate $(CaCO_3)$ at $298 \ K$ is $6.4 \times 10^{-5} \ mol \ dm^{-3}$. Calculate the value of solubility product $(K_{sp})$ at the same temperature.

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A
$5.06 \times 10^{-10}$
B
$4.096 \times 10^{-9}$
C
$3.05 \times 10^{-10}$
D
$2.8 \times 10^{-9}$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Solubility product

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The solubility of $BaSO_4$ in pure water (in $g \, L^{-1}$) is closest to
[Given: $K_{sp}$ for $BaSO_4$ is $1.0 \times 10^{-10}$ at $25^{\circ} C$. Molecular weight of $BaSO_4$ is $233 \, g \, mol^{-1}$]

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

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Which of the following would increase the solubility of $Pb(OH)_2$?

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The solubility product constant $K_{sp}$ of $Mg(OH)_2$ is $9.0 \times 10^{-12}.$ If a solution is $0.010 \ M$ with respect to $Mg^{2+}$ ion,what is the maximum hydroxide ion concentration which could be present without causing the precipitation of $Mg(OH)_2$?

Medium

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$A$ salt $MX$ has $K_{sp} = 4 \times 10^{-10}$. What value of $K_{sp}$ must another salt $MX_3$ have if the molar solubility of the two salts is to be identical?

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The solubility of calcium carbonate $(CaCO_3)$ at $298 \ K$ is $6.4 \times 10^{-5} \ mol \ dm^{-3}$. Calculate the value of solubility product $(K_{sp})$ at the same temperature.

Similar Questions

The solubility of $BaSO_4$ in pure water (in $g \, L^{-1}$) is closest to[Given: $K_{sp}$ for $BaSO_4$ is $1.0 \times 10^{-10}$ at $25^{\circ} C$. Molecular weight of $BaSO_4$ is $233 \, g \, mol^{-1}$]

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?

Which of the following would increase the solubility of $Pb(OH)_2$?

The solubility product constant $K_{sp}$ of $Mg(OH)_2$ is $9.0 \times 10^{-12}.$ If a solution is $0.010 \ M$ with respect to $Mg^{2+}$ ion,what is the maximum hydroxide ion concentration which could be present without causing the precipitation of $Mg(OH)_2$?

$A$ salt $MX$ has $K_{sp} = 4 \times 10^{-10}$. What value of $K_{sp}$ must another salt $MX_3$ have if the molar solubility of the two salts is to be identical?

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The solubility of $BaSO_4$ in pure water (in $g \, L^{-1}$) is closest to
[Given: $K_{sp}$ for $BaSO_4$ is $1.0 \times 10^{-10}$ at $25^{\circ} C$. Molecular weight of $BaSO_4$ is $233 \, g \, mol^{-1}$]

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?