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

  • Option 1)

    The molar solubilities of MY and NY_3 in water are identical.

  • Option 2)

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

  • Option 3)

    The salts MY and NY_3 are more soluble in 0.5M KY than in pure water

  • Option 4)

    The addition of the salt of KY to solution of MY and NY_3 will have no effect on their solubilities

 

Answers (1)

 

General expression of solubility product -

M_{x}X_{y}\rightleftharpoons xM^{p+}(aq)+yX^{2-}(aq)


(x.p^{+}=y.\bar{q})

- wherein

Its solubility product is 
 

K_{sp}=[M^{p+}]^{x}\:[X^{2-}]^{y}

 

 For MY Ksp= S{_{1}}^{2}

or S_{1}= \sqrt{K_{sp}}=\sqrt{6.2 \times 10^{-13}}=7.87 \times 10^{-7} mol ^{-1}

For NY_{3} \ K_{sp}=27{S_{2}}^{4}

\Rightarrow S_{2}=\sqrt{\frac{6.2\times 10^{-13}}{27}}= 3.89 \times 10^{-4} mol L^{-1}


Option 1)

The molar solubilities of MY and NY_3 in water are identical.

incorrect

Option 2)

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

correct

Option 3)

The salts MY and NY_3 are more soluble in 0.5M KY than in pure water

incorrect

Option 4)

The addition of the salt of KY to solution of MY and NY_3 will have no effect on their solubilities

incorrect

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