Choose the correct statement(s) A) If the solubility of ${Sb}_2 S_3$ is $1.0 \times 10^{-5} {~mol} / {L}$ at $298 {~K}$, its solubility product will be $108 \times 10^{-25}$ B) ${pH}$ of an aqueous solution having $\left[{H}^{+}\right]=10^{-8} {M}$ is 8 . C) Ammonia is a leveling solvent for stronger acids like ${HCl}, {HBr}, {HI}$ while glacial acetic acid is differentiating solvent.

JEE CHEMISTRY MCQ: Equilibrium

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Application +4 | -1

Choose the correct statement(s)

A) If the solubility of

{Sb}_2 S_3

1.0 \times 10^{-5} {~mol} / {L}

298 {~K}

, its solubility product will be

108 \times 10^{-25}

{pH}

of an aqueous solution having

\left[{H}^{+}\right]=10^{-8} {M}

is 8 .

C) Ammonia is a leveling solvent for stronger acids like

{HCl}, {HBr}, {HI}

while glacial acetic acid is differentiating solvent.

View answer and explanation

Correct option: D

A, B and C

Option D (A, B and C) is correct because all three statements are correct regarding solubility product, pH calculation, and solvent leveling/differentiating effects.

More Questions from Equilibrium

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The indicator used in titrating oxalic acid with caustic soda solution is:

\mathrm{K}_1

and

\mathrm{K}_2

are equilibrium constant for reactions (i) and (ii)

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

(i)

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

(ii)

Then,

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

are the respective ionisation constants for the following reactions

\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}

The correct relationship between

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

is The

\mathrm{pH}

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

solution is (For

\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

) Reaction

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

In equilibrium condition pressure of

\text{O}_2

depends on: A : At equilibrium concentration of the reactant and product does not change with time for a chemical reaction.
R: The rate of reaction is zero at equilibrium.