Question

The equilibrium constant for the reaction below has the value K a = 3.5 × 10–4. In this reaction the
Brønsted-Lowry acid is ________.
HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq)

Express your answer as a chemical formula.

Answer 1

Answer on Question #41600, Chemistry, Other

Task:

The equilibrium constant for the reaction below has the value $Ka = 3.5 \times 10^{-4}$. In this reaction the Brønsted-Lowry acid is ________.

$$HF(aq) + H_2O(l) \rightleftharpoons H_3O^+(aq) + F^-(aq)$$

Express your answer as a chemical formula.

Answer:

A Bronsted-Lowry acid is defined as anything that releases $H^+$ ions. In this case a Fluorine acid dissociates to:

$$HF = H^+ + F^-$$

At the same time $H_2O$ molecule accepts the $H^+$ proton.

$$H_2O + H^+ = H_3O^+$$

So if the HF releases the $H^+$, it is the Brønsted-Lowry acid in this reaction.

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