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Topic: Solubility product· Equilibrium

MY and NY_3, two nearly insoluble salts, have the same K_sp values of 6.2×10^-13 at room temperature. Which statement would be true in regard to MY and NY_3 ?

1. The molar solubilities of MY and \(NY_3\) in water are identical.

2. The molar solubility of MY in water is less than that of \(NY_3\).

3. The salts MY and \(NY_3\) are more soluble in 0.5 M KY than in pure water.

4. The addition of the salt of KY to solution of MY and \(NY_3\) will have no effect on their solubilities.

1 answer

Best answer

Answer: 2. The molar solubility of MY in water is less than that of \(NY_3\).

Key idea: compare solubilities from the \(K_{sp}\) expression for each salt type.

  • MY: \(K_{sp}=s^2\), so \(s=\sqrt{6.2\times10^{-13}}\approx 7.9\times10^{-7}\) M.
  • \(\mathrm{NY_3}\): \(K_{sp}=s(3s)^3=27s^4\), so \(s=(6.2\times10^{-13}/27)^{1/4}\approx 3.9\times10^{-4}\) M.

So MY is less soluble than \(\mathrm{NY_3}\) (option 2). Option 1 is wrong. Options 3 and 4 are wrong because KY adds the common ion \(\mathrm{Y^-}\), which lowers solubility.

Doubtly AI · 30 Oct 2026 AI-generated · not yet verified Report
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