(D) For $MY$: $K_{sp} = s_1^2$$\Rightarrow s_1 = \sqrt{K_{sp}} = \sqrt{6.2 \times 10^{-13}} = 7.87 \times 10^{-7} \ mol \ L^{-1}$For $NY_3$: $K_{sp} =

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The molar solubility of $MY$ in water is less than that of $NY_3$.

(D) For $MY$: $K_{sp} = s_1^2$$\Rightarrow s_1 = \sqrt{K_{sp}} = \sqrt{6.2 \times 10^{-13}} = 7.87 \times 10^{-7} \ mol \ L^{-1}$For $NY_3$: $K_{sp} = [N^{3+}][Y^-]^3 = (s_2)(3s_2)^3 = 27s_2^4$$\Rightarrow s_2 = \sqrt[4]{\frac{6.2 \times 10^{-13}}{27}} = 3.89 \times 10^{-4} \ mol \ L^{-1}$Comparing the values,$s_1 Therefore,the molar solubility of $MY$ in water is less than that of $NY_3$.

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

Difficult

$MY$ and $NY_3$,two nearly insoluble salts,have the same $K_{sp}$ values of $6.2 \times 10^{-13}$ at room temperature. Which statement would be true in regard to $MY$ and $NY_3$?

NEET 2016 All NEET

A
The salts $MY$ and $NY_3$ are more soluble in $0.5 \ M \ KY$ than in pure water.
B
The addition of the salt of $KY$ to solution of $MY$ and $NY_3$ will have no effect on their solubilities.
C
The molar solubilities of $MY$ and $NY_3$ in water are identical.
D
The molar solubility of $MY$ in water is less than that of $NY_3$.

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6-2.Equilibrium-II (Ionic Equilibrium)

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Solubility product

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$MY$ and $NY_3$,two nearly insoluble salts,have the same $K_{sp}$ values of $6.2 \times 10^{-13}$ at room temperature. Which statement would be true in regard to $MY$ and $NY_3$?

Similar Questions

Which of the following compounds is insoluble in acetic acid?

How many grams of $CaC_2O_4$ (molecular weight $= 128$) on dissolving in $1 \ L$ of distilled water will give a saturated solution? $[K_{sp}(CaC_2O_4) = 2.5 \times 10^{-9} \ mol^2 L^{-2}]$

Assign $A$,$B$,$C$,$D$ from the given type of reaction.$HgS \downarrow + HNO_3 \text{ (Conc.)} \longrightarrow \text{No dissolution}$

Which of the following is least soluble in water?

Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.Reason : $K_{sp}$ of $AgCl < K_{sp}$ of $AgBr$.

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$HgS \downarrow + HNO_3 \text{ (Conc.)} \longrightarrow \text{No dissolution}$

Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.
Reason : $K_{sp}$ of $AgCl < K_{sp}$ of $AgBr$.