WBJEE · Chemistry · Ionic Equilibrium
A saturated solution of \(\mathrm{BaSO}_{4}\) at \(25^{\circ} \mathrm{C}\) is \(4 \times 10^{-5} \mathrm{M}\). The solubility of \(\mathrm{BaSO}_{4}\) in \(0.1 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}\) at this temperature will be
- A \(1.6 \times 10^{-9} \mathrm{M}\)
- B \(1.6 \times 10^{-8} \mathrm{M}\)
- C \(4 \times 10^{-6} \mathrm{M}\)
- D \(4 \times 10^{-4} \mathrm{M}\)
Answer & Solution
Correct Answer
(D) \(4 \times 10^{-4} \mathrm{M}\)
Step-by-step Solution
Detailed explanation
\(\begin{array}{r} \mathrm{BaSO}_{4} \rightleftharpoons \mathrm{Ba}^{2+}+\mathrm{SO}_{4}^{2-} \\ \mathrm{s} \quad \mathrm{s}+0.1 \\ \mathrm{Na}_{2} \mathrm{SO}_{4} \rightarrow 2 \mathrm{Na}^{+}+\mathrm{SO}_{4}^{2-} \\ 0.2 \quad 0.1 \end{array}\)…
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