(A) First,calculate the solubility $S$ in $mol / L$:$S = \frac{2.34 \times 10^{-3} \, g}{78 \, g/mol} \times \frac{1}{0.1 \, L} = \frac{0.03 \times 10

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(A) First,calculate the solubility $S$ in $mol / L$:$S = \frac{2.34 \times 10^{-3} \, g}{78 \, g/mol} \times \frac{1}{0.1 \, L} = \frac{0.03 \times 10^{-3}}{0.1} = 3 \times 10^{-4} \, mol / L$.The dissociation of $CaF_{2}$ is $CaF_{2} \rightleftharpoons Ca^{2+} + 2F^-$.$K_{sp} = [Ca^{2+}][F^-]^{2} = (S)(2S)^{2} = 4S^{3}$.$K_{sp} = 4 \times (3 \times 10^{-4})^{3} = 4 \times 27 \times 10^{-12} = 108 \times 10^{-12} = 0.0108 \times 10^{-8} \, (mol / L)^{3}$.Thus,$x = 0.0108$.

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

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At $310 \, K$,the solubility of $CaF_{2}$ in water is $2.34 \times 10^{-3} \, g / 100 \, mL$. The solubility product of $CaF_{2}$ is $x \times 10^{-8} \, (mol / L)^{3}$. Find the value of $x$. (Given molar mass: $CaF_{2} = 78 \, g \, mol^{-1}$)

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A
$0.0108$
B
$0.108$
C
$1.08$
D
$10.8$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Which of the following has the maximum solubility? ($K_{sp}$ values are given in parentheses.)

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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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At $310 \, K$,the solubility of $CaF_{2}$ in water is $2.34 \times 10^{-3} \, g / 100 \, mL$. The solubility product of $CaF_{2}$ is $x \times 10^{-8} \, (mol / L)^{3}$. Find the value of $x$. (Given molar mass: $CaF_{2} = 78 \, g \, mol^{-1}$)

Similar Questions

The solubility product of silver bromide is $5.0 \times 10^{-13}$. The quantity of potassium bromide (molar mass taken as $120 \ g \ mol^{-1}$) to be added to $1 \ L$ of $0.05 \ M$ solution of silver nitrate to start the precipitation of $AgBr$ is

Which of the following has the maximum solubility? ($K_{sp}$ values are given in parentheses.)

The $K_{sp}$ of $AgCl$ is $1.8 \times 10^{-10}$. The concentration of $Cl^-$ required to initiate the precipitation of $AgCl$ in a solution containing $4 \times 10^{-3} \ M \ Ag^+$ is:

Solubility product constants $(K_{sp})$ of silver salts are given as $AgCl = 2 \times 10^{-10}$,$AgBr = 5 \times 10^{-13}$,$Ag_2CO_3 = 8 \times 10^{-12}$,and $AgI = 8 \times 10^{-17}$. Which salt shows the highest solubility?

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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