MY and ${\rm{N}}{{\rm{Y}}_{\rm{3}}}$, two nearly insoluble salts, have the same ${{\rm{K}}_{{\rm{sp}}}}$ values of $6.2 \times {\rm{1}}{{\rm{0}}^{ - 13}}$ at room temperature. Which statement would be true in regard to MY and ${\rm{N}}{{\rm{Y}}_{\rm{3}}}$?

The molar solubility of MY in water is less than that of ${\rm{N}}{{\rm{Y}}_{\rm{3}}}$.

The molar solubilities of MY and ${\rm{N}}{{\rm{Y}}_{\rm{3}}}$ in water are identical.

The salts MY and ${\rm{N}}{{\rm{Y}}_{\rm{3}}}$ are more soluble in 0.5 M KY than in pure water.

The addition of the salt of KY to solution of MY and ${\rm{N}}{{\rm{Y}}_{\rm{3}}}$ will have no effect on their solubilities.

NEET UG CHEMISTRY MCQ: Equilibrium

1 Hard

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Analyzing +4 | -1

MY and

\mathrm{N}{\mathrm{Y}_\mathrm{3}}

, two nearly insoluble salts, have the same

{\mathrm{K}_{\mathrm{sp}}}

values of

6.2 \times \mathrm{1}{\mathrm{0}^{ - 13}}

at room temperature. Which statement would be true in regard to MY and

\mathrm{N}{\mathrm{Y}_\mathrm{3}}

View answer and explanation

Correct option: B

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

\mathrm{N}{\mathrm{Y}_\mathrm{3}}

Option B (The molar solubility of MY in water is less than that of

\mathrm{N}{\mathrm{Y}_\mathrm{3}}

) is correct because, for the same

K_{sp}

, salts with more ions have higher molar solubility.