(C) The solubility $S$ in $mol \, L^{-1}$ is calculated as: $S = \frac{0.7 \, g \, L^{-1}}{461.2 \, g \, mol^{-1}} \approx 1.5178 \times 10^{-3} \, mo

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(C) The solubility $S$ in $mol \, L^{-1}$ is calculated as: $S = \frac{0.7 \, g \, L^{-1}}{461.2 \, g \, mol^{-1}} \approx 1.5178 \times 10^{-3} \, mol \, L^{-1}$.For the salt $PbI_2$,the dissociation is $PbI_2(s) \rightleftharpoons Pb^{2+}(aq) + 2I^-(aq)$.The solubility product expression is $K_{sp} = [Pb^{2+}][I^-]^2 = (S)(2S)^2 = 4S^3$.Substituting the value of $S$: $K_{sp} = 4 \times (1.5178 \times 10^{-3})^3$.$K_{sp} = 4 \times (3.50 \times 10^{-9}) = 14.0 \times 10^{-9}$.

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

Medium

The solubility of $PbI_2$ at $25 \, ^\circ C$ is $0.7 \, g \, L^{-1}$. What is the solubility product $(K_{sp})$ of $PbI_2$ at this temperature? (Molar mass of $PbI_2 = 461.2 \, g \, mol^{-1}$)

A
$0.14 \times 10^{-9}$
B
$1.40 \times 10^{-9}$
C
$14.0 \times 10^{-9}$
D
$140 \times 10^{-9}$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Solubility product

The solubility of $AgCl$ is $1.435 \times 10^{-5} \ g \ L^{-1}$ at $30^{\circ} C$. Calculate its solubility product $(K_{sp})$. (Molar mass of $AgCl = 143.5 \ g \ mol^{-1}$)

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If the solubility product of $PbS$ is $3.4 \times 10^{-28}$,what is the minimum concentration of sulfide ions required to precipitate $PbS$ from a $0.001 \ M \ Pb^{2+}$ solution?

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What volume of water in $L$ is required to dissolve $1 \, g$ of $BaSO_4$ at $25 \, ^\circ C$? $(K_{sp} = 1.1 \times 10^{-10})$

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The solubility of a sparingly soluble salt $AB_2$ is $18.78 \times 10^{-4} \text{ g/dm}^3$. What is its solubility product? (Molar mass of $AB_2 = 187.8 \text{ g mol}^{-1}$)

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For the equilibrium reaction: $Fe(OH)_3(s) \rightleftharpoons Fe^{3+}(aq) + 3OH^-(aq)$,if the concentration of $OH^-$ is reduced to $\frac{1}{4}$ of its initial value,by what factor will the concentration of $Fe^{3+}$ increase at equilibrium?

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The solubility of $PbI_2$ at $25 \, ^\circ C$ is $0.7 \, g \, L^{-1}$. What is the solubility product $(K_{sp})$ of $PbI_2$ at this temperature? (Molar mass of $PbI_2 = 461.2 \, g \, mol^{-1}$)

Similar Questions

The solubility of $AgCl$ is $1.435 \times 10^{-5} \ g \ L^{-1}$ at $30^{\circ} C$. Calculate its solubility product $(K_{sp})$. (Molar mass of $AgCl = 143.5 \ g \ mol^{-1}$)

If the solubility product of $PbS$ is $3.4 \times 10^{-28}$,what is the minimum concentration of sulfide ions required to precipitate $PbS$ from a $0.001 \ M \ Pb^{2+}$ solution?

What volume of water in $L$ is required to dissolve $1 \, g$ of $BaSO_4$ at $25 \, ^\circ C$? $(K_{sp} = 1.1 \times 10^{-10})$

The solubility of a sparingly soluble salt $AB_2$ is $18.78 \times 10^{-4} \text{ g/dm}^3$. What is its solubility product? (Molar mass of $AB_2 = 187.8 \text{ g mol}^{-1}$)

For the equilibrium reaction: $Fe(OH)_3(s) \rightleftharpoons Fe^{3+}(aq) + 3OH^-(aq)$,if the concentration of $OH^-$ is reduced to $\frac{1}{4}$ of its initial value,by what factor will the concentration of $Fe^{3+}$ increase at equilibrium?

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