Explaining Acidity with the Arrhenius and Brønsted–Lowry Theories Account for the acidic properties of nitrous acid (HNO2) using the Arrhenius theory and the Brønsted–Lowry theory, and identify the conjugate base of HNO2.

Question

Explaining Acidity with the Arrhenius and Brønsted–Lowry Theories

Account for the acidic properties of nitrous acid ([latex]HNO_2[/latex]) using the Arrhenius theory and the Brønsted–Lowry theory, and identify the conjugate base of [latex]HNO_2[/latex].

STRATEGY

To account for the acidity of a substance, consider how it can produce [latex]H^+[/latex] ions in water (Arrhenius theory) and how it can act as a proton donor (Brønsted–Lowry theory).

Accepted Answer

[latex]HNO_2[/latex] is an Arrhenius acid because it dissociates in water to produce [latex]H^+[/latex] ions:

[latex]\mathrm{HNO}_2(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{NO}_2^{-}(a q)[/latex]

Nitrous acid is a Brønsted–Lowry acid because it acts as a proton donor when it dissociates, transferring a proton to water to give the hydronium ion, [latex]H_3O^+[/latex]:

The conjugate base of [latex]HNO_2[/latex] is [latex]NO_{2}^{-}[/latex], the species that remains after [latex]HNO_2[/latex] has lost a proton

Chapter 14

Q. 14.1

Q. 14.1

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