JEE CHEMISTRY MCQ: Equilibrium

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Analyzing +4 | -1

The correct increasing order of solubility of the following substances in

\mathrm{g} / 100 \mathrm{~ml}

\mathrm{PbSO}_4\left(K_{\mathrm{sp}}=2 \times 10^{-9}\right), \operatorname{ZnS}\left(K_{\mathrm{sp}}=1 \times 10^{-22}\right), \operatorname{AgBr}\left(K_{\mathrm{sp}}=4 \times 10^{-13}\right),

\mathrm{CuCO}_3\left(K_{\mathrm{sp}}=1 \times 10^{-8}\right).

(Atomic masses:

\mathrm{Pb}=208, \mathrm{Zn}=65, \mathrm{Ag}=108, \mathrm{Br}=80, \mathrm{Cu}=63)

View answer and explanation

Correct option: C

\mathrm{ZnS} < \mathrm{AgBr} < \mathrm{CuCO}_3 < \mathrm{PbSO}_4

Option C (

\mathrm{ZnS} < \mathrm{AgBr} < \mathrm{CuCO}_3 < \mathrm{PbSO}_4

) is correct because it represents the increasing order of solubility based on the calculated solubility from the given Ksp values.

More Questions from Equilibrium

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\mathrm{K}_1

\mathrm{K}_2

\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})\quad\ldots

\mathrm{NO}(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{~N}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})\quad\ldots

K{a_1},\,\,\,K{a_2}\,\,\,\mathrm{and}\,\,\,K{a_3}

\begin{array}{l} {H_2}S\leftrightharpoons{H^ + } + H{S^ - }\\ H{S^ - }\leftrightharpoons{H^ + } + {S^{2 - }}\\ {H_2}S\leftrightharpoons2{H^ + } + {S^{2 - }} \end{array}

K{a_1},\,\,K{a_2}\,,K{a_3}

\mathrm{pH}

0.1 \mathrm{~M}-\mathrm{N}_2 \mathrm{H}_4

\mathrm{N}_2 \mathrm{H}_4,

K_{{b}_1}=3.6 \times 10^{-6}, K_{{b}_2}=6.4 \times 10^{-12}, \log 2=0.3

\log 3=0.48

{\text{Ba}}{{\text{O}}_2}(s) \rightleftharpoons {\text{BaO}}(s) + {{\text{O}}_2}(g);\Delta H = - {\text{ve}}.

\text{O}_2