(B) For $CuI_{(s)} \rightleftharpoons Cu^{+}_{(aq)} + I^{-}_{(aq)}$:$K_{sp} = [Cu^{+}][I^{-}] = x^{2} = 4 \times 10^{-12}$$x = \sqrt{4 \times 10^{-12}

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(B) For $CuI_{(s)} \rightleftharpoons Cu^{+}_{(aq)} + I^{-}_{(aq)}$:$K_{sp} = [Cu^{+}][I^{-}] = x^{2} = 4 \times 10^{-12}$$x = \sqrt{4 \times 10^{-12}} = 2 \times 10^{-6} \ M$For $Ag_{2}CrO_{4(s)} \rightleftharpoons 2Ag^{+}_{(aq)} + Cr{O_{4}}^{2-}_{(aq)}$:$K_{sp} = [Ag^{+}]^{2} [CrO_{4}^{2-}] = (2y)^{2}(y) = 4y^{3} = 4 \times 10^{-12}$$y^{3} = 10^{-12} \implies y = 10^{-4} \ M$Ratio of solubilities $x/y = (2 \times 10^{-6}) / (10^{-4}) = 2 \times 10^{-2} = 0.02$.

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

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Solubility products of $CuI$ and $Ag_{2}CrO_{4}$ have almost the same value $(\sim 4 \times 10^{-12})$. The ratio of solubilities of the two salts $(CuI : Ag_{2}CrO_{4})$ is closest to $....$

KVPY 2019 All KVPY

A
$0.01$
B
$0.02$
C
$0.03$
D
$0.10$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Solubility product

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Solid $Ba(NO_3)_2$ is gradually dissolved in a $1.0 \times 10^{-4} \ M$ $Na_2CO_3$ solution. At what concentration of $Ba^{2+}$ will a precipitate begin to form? ($K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)

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If $K_{sp}$ of $Ag_2CO_3$ is $8 \times 10^{-12},$ the molar solubility of $Ag_2CO_3$ in $0.1 \ M \ AgNO_3$ is

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Solubility products of $CuI$ and $Ag_{2}CrO_{4}$ have almost the same value $(\sim 4 \times 10^{-12})$. The ratio of solubilities of the two salts $(CuI : Ag_{2}CrO_{4})$ is closest to $....$

Similar Questions

The volume of the water needed to dissolve $1 \ g$ of $BaSO_4$ $(K_{sp} = 1.1 \times 10^{-10})$ at $25 \ ^oC$ is ..... $litre$.

Which of the following pairs of ions would be expected to form a precipitate when their dilute solutions are mixed?

Equal volumes of $0.02 \ M$ $CaCl_2$ and $0.00004 \ M$ $Na_2SO_4$ solutions are mixed. Will a precipitation of $CaSO_4$ occur? $(K_{sp} = 2.4 \times 10^{-5})$

Solid $Ba(NO_3)_2$ is gradually dissolved in a $1.0 \times 10^{-4} \ M$ $Na_2CO_3$ solution. At what concentration of $Ba^{2+}$ will a precipitate begin to form? ($K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)

If $K_{sp}$ of $Ag_2CO_3$ is $8 \times 10^{-12},$ the molar solubility of $Ag_2CO_3$ in $0.1 \ M \ AgNO_3$ is

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