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# The following equilibrium is established when $~HCl{{O}_{4}}$ is dissolved in weak acid $HF.$  $HF+HCl{{O}_{4}}\rightleftharpoons ClO_{4}^{-}+{{H}_{2}}{{F}^{+}}.$ Which of the following is the correct set of conjugate acid base pairs?(A) $HF\text{ }and\text{ }HCl{{O}_{4}}.$ (B) $HF\text{ }and\text{ }ClO_{4}^{-}.$ (C) $HF\text{ }and\text{ }H{{F}_{2}}.$ (D) $HCl{{O}_{4}}\text{ }and\text{ }{{H}_{2}}{{F}^{+}}.$

Last updated date: 24th Jul 2024
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Hint: We know that this question is based on Bronsted-Lowry theory of acid and base. According to this compound that gives off ion in solution is considered as acid and compound that accepts in solution is considered as base. After giving off proton species that form is the conjugate base of the acid and after accepting proton species that form is the conjugate acid of the base.

$\underset{acid}{\mathop{HX}}\,+\underset{base}{\mathop{B}}\,\rightleftharpoons \underset{\begin{smallmatrix} Conjugate \\ acid \end{smallmatrix}}{\mathop{H{{B}^{+}}}}\,+\underset{\begin{smallmatrix} Conjugate \\ base \end{smallmatrix}}{\mathop{{{X}^{-}}}}\,$
Conjugate acid base pair differ by a proton $\left( {{H}^{+}} \right)$ ;
$\underset{\begin{smallmatrix} \text{Bronsted-Lowry } \\ \text{Acid } \end{smallmatrix}}{\mathop{HA}}\,+\underset{\begin{smallmatrix} \text{Bronsted-Lowry } \\ \text{Acid } \end{smallmatrix}}{\mathop{B}}\,\rightleftharpoons \underset{\begin{smallmatrix} \text{Conjugate } \\ \text{Base } \end{smallmatrix}}{\mathop{A}}\,+\text{ }\underset{\begin{smallmatrix} \text{Conjugate } \\ \text{Acid } \end{smallmatrix}}{\mathop{H{{B}^{+}}}}\,.$ ’