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Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumpH of Strong and Weak Acids and BasesMedium2 minQB

ChemistryMediumsingle choice

Passage / Comprehension

In water, HF behaves as a weak acid. The reactions involved are:

Reaction-I: $H F (a q) + H_{2} O (l) ⇌ H_{3} O^{+} (a q) + F^{-} (a q)$ ; $K_{1} = 1.1 \times 1 0^{- 3}$

Reaction-II: $H F (a q) + F^{-} (a q) ⇌ H F_{2}^{-} (a q)$ ; $K_{2} = 0.26$

Two chemists wanted to determine the acidity constant, $K_{1}$ , using the same HF solution and measuring the pH of the solution. One chemist was having the idea of reaction-I only while the other chemist was having the idea of both reactions. Surprisingly, both the chemist determined the same value of K₁ (as given above).

Which of the following must be incorrect?

Options:

Answer:

Solution:

For a weak acid, $[H_{3} O^{+}] < [HF]_{0}$ . Options B, C, D imply specific conditions, but A is generally incorrect.

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:pH of Strong and Weak Acids and Bases

⏱ 2mℹ️ Source: QB

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