MHT CET 2025 22nd April Evening Shift | Ionic Equilibrium Question 15 | Chemistry

$$ \mathrm{HSO}_{3(\mathrm{aq})}^{-}+\mathrm{H}_3 \mathrm{O}_{(\mathrm{aq})}^{+} \rightleftharpoons \mathrm{H}_2 \mathrm{SO}_3+\mathrm{H}_2 \mathrm{O} $$

$\quad \mathrm{H}_2 \mathrm{SO}_3$ and $\mathrm{HSO}_3^{-}$

$\mathrm{HSO}_3^{-}$and $\mathrm{H}_3 \mathrm{O}^{+}$

$\mathrm{H}_2 \mathrm{SO}_3$ and $\mathrm{H}_2 \mathrm{O}$

$\mathrm{H}_3 \mathrm{O}^{+}$and $\mathrm{H}_2 \mathrm{SO}_3$

MHT CET 2025 22nd April Evening Shift

MCQ (Single Correct Answer)

-0

A weak monoacidic base dissociates to $1.5 \%$ in 0.001 M solution at 298 K . Calculate the dissociation constant of weak base.

$2.25 \times 10^{-7}$

$3.05 \times 10^{-7}$

$2.5 \times 10^{-5}$

$3.725 \times 10^{-6}$

MHT CET 2025 22nd April Evening Shift

MCQ (Single Correct Answer)

-0

The solubility product of NiS is $4.9 \times 10^{-5}$ at 298 K . Calculate its solubility in $\mathrm{mol} \mathrm{dm}^{-3}$ at the same temperature?

$1.69 \times 10^{-3}$

$7.0 \times 10^{-3}$

$2.45 \times 10^{-3}$

$6.18 \times 10^{-3}$

MHT CET 2025 22nd April Morning Shift

MCQ (Single Correct Answer)

-0

Identify the conjugate acid-base pair respectively from following equilibrium reaction.

$$ \mathrm{HPO}_{4(\mathrm{aq})}^{2-}+\mathrm{H}_2 \mathrm{O}_{(\ell)} \rightleftharpoons \mathrm{PO}_{4(\mathrm{aq})}^{3-}+\mathrm{H}_3 \mathrm{O}_{(\mathrm{eq})}^{+} $$

$\mathrm{H}_3 \mathrm{O}^{+}$and $\mathrm{H}_2 \mathrm{O}$

$\mathrm{H}_2 \mathrm{O}$ and $\mathrm{HPO}_4^{2-}$

$\mathrm{PO}_4^{3-}$ and $\mathrm{H}_3 \mathrm{O}^{+}$

$\mathrm{H}_3 \mathrm{O}^{+}$and $\mathrm{HPO}_4^{2-}$

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