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).

[latex]HNO_{2}[/latex] is an Arrhenius acid because it dissociates in water to produce [latex]H^{+}[/latex] ions: [latex]HNO_{2}(aq) \rightleftharpoons H^{+}(aq) + NO_{2}^{-}(aq)[/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_{3}O^{+}[/latex]: [latex]\underbrace{\underset{Acid}HNO_{2}(aq) + \underbrace{\underset{Base}{H_{2}O(l)} \rightleftharpoons \underset{Acid}{H_{3}O^{+}(aq)} }_{Conjugate acid–base pairs} + \underset{Base}{NO_{2}^{-}(aq)}} _{} [/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.

Question 14.1: EXPLAINING ACIDITY WITH THE ARRHENIUS AND BRØNSTED–LOWRY THE...

Chemistry

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).

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$HNO_{2}$ is an Arrhenius acid because it dissociates in water to produce $H^{+}$ ions:

HNO_{2}(aq)  \rightleftharpoons  H^{+}(aq)  +  NO_{2}^{-}(aq)

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, $H_{3}O^{+}$ :