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6-2.Equilibrium-II (Ionic Equilibrium)
medium
What would be the concentration of ${H_2}S{O_4}$ necessary to precipitate $BaS{O_4}$ from a solution of $0.01\,M\,B{a^{2 + }}$ions ($K_sp=$ $1.0 \times {10^{ - 9}}$ )
A
${10^{ - 9}}$
B
${10^{ - 8}}$
C
${10^{ - 7}}$
D
${10^{ - 6}}$
Solution
(c) $BaS{O_4}⇌\mathop {\mathop {B{a^{ + 2 }}}\limits_{(S)\,\,\,\,\,\,\,} }\limits_{0.01\,\,\,\,} + \mathop {\mathop {SO_4^{ – \, – }}\limits_{(S)\,\,\,\,} }\limits_{5\,\,\,\,} $
${K_{sp}} = {S^2} = S \times S = 0.01 \times S$
${S_{(SO_4^{2 – })}} = \frac{{{K_{sp}}}}{{{S_{(B{a^{ + + }})}}}} = \frac{{1 \times {{10}^{ – 9}}}}{{0.01}} = {10^{ – 7}}$ $mole/litre$
Standard 11
Chemistry
Similar Questions
The solubility product $(K_{sp})$ of the following compounds are given at $25\,^oC$
| Compound | $K_{sp}$ |
| $AgCl$ | $1.1\times10^{-10}$ |
| $AgI$ | $1.0\times10^{-16}$ |
| $PbCrO_4$ | $4.0\times10^{-14}$ |
| $Ag_2CO_3$ | $8.0\times10^{-12}$ |
The most soluble and least soluble compounds are respectively.
