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JEE Main 2007
Exam
JEE Main
Year
2007
Subject
Chemistry
Chapter
Ionic Equilibrium

JEE Main 2007 · Chemistry · Ionic Equilibrium

In a sautrated solution of the sparingly soluble strong electrolyte...

In a sautrated solution of the sparingly soluble strong electrolyte AgIO3\mathrm{AgIO}_3 (Molecular mass =283=283) the equilibrium which sets in is AgIO3(s)⇌Ag(aq)++IO3(aq)−\mathrm{AgIO}_{3(\mathrm{s})} \rightleftharpoons \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{IO}_{3(\mathrm{aq})}^{-} If the solubility product constant Ksp\mathrm{K}_{\mathrm{sp}} of AgIO3\mathrm{AgIO}_3 at a given temperature is 1.0×10−81.0 \times 10^{-8}, what is the mass of AgIO3\mathrm{AgIO}_3 contained in 100 ml100 \mathrm{~ml} of its saturated solution?

Options

  1. A28.3×10−2 g28.3 \times 10^{-2} \mathrm{~g}
  2. B2.83×10−3 g2.83 \times 10^{-3} \mathrm{~g}
  3. C1.0×10−7 g1.0 \times 10^{-7} \mathrm{~g}
  4. D1.0×10−4 g1.0 \times 10^{-4} \mathrm{~g}

Correct answer

B. 2.83×10−3 g2.83 \times 10^{-3} \mathrm{~g}

Step-by-step solution

AgIO3(s)⇌Ag+(aq)+IO3−(aq)\mathrm{AgIO}_3(\mathrm{s}) \rightleftharpoons \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{IO}_3^{-}(\mathrm{aq}) Let the solubility of AgIO3\mathrm{AgIO}_3 be s\mathrm{s} Ksp=\mathrm{K}_{\mathrm{sp}}=\left[\mathrm{Ag}^{+}\right][IO3−]\left[\mathrm{IO}_3^{-}\right] 1.0×10−8=s21.0 \times 10^{-8}=\mathrm{s}^2 s=10−4 mol/litre\mathrm{s}=10^{-4} \mathrm{~mol} / \mathrm{litre} =10−4×2831000×100=\frac{10^{-4} \times 283}{1000} \times 100 =283×10−5=283 \times 10^{-5} =2.83×10−3 g/100 ml=2.83 \times 10^{-3} \mathrm{~g} / 100 \mathrm{~ml} Hence, (B) is correct.
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