Question 14.1: Explaining Acidity with the Arrhenius and Brønsted–Lowry The......

General Chemistry: Atoms First [1015060]

Explaining Acidity with the Arrhenius and Brønsted–Lowry Theories

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

STRATEGY

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

Step-by-Step

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$HNO_2$ is an Arrhenius acid because it dissociates in water to produce $H^+$ ions:

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

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, $H_3O^+$ :

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

working example 14.1

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