Question
Identify the two Bronsted-Lowry acids and two bases in the reaction$$\mathrm{NH}_{2} \mathrm{OH}+\mathrm{CH}_{3} \mathrm{NH}_{3}+\rightleftharpoons \mathrm{NH}_{3} \mathrm{OH}^{+}+\mathrm{CH}_{3} \mathrm{NH}_{2}$$
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According to this definition, an acid is a species that donates a proton (H+) to another species, while a base is a species that accepts a proton from an acid. Show more…
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Identify the two Brønsted-Lowry acids and two bases in the reaction $$ \mathrm{NH}_{2} \mathrm{OH}+\mathrm{CH}_{3} \mathrm{~N}^{+} \rightleftharpoons \mathrm{NH}_{3} \mathrm{OH}^{+}+\mathrm{CH}_{3} \mathrm{NH}_{2} $$
Identify the Bronsted-Lowry acids and bases in these reactions and group them into conjugate acid-base pairs. (a) $\mathrm{NH}_{3}+\mathrm{HI} \rightleftharpoons \mathrm{NH}_{4}^{+}+\mathrm{I}^{-}$ (b) $\mathrm{NH}_{4}^{+}+\mathrm{HS}^{-} \rightleftharpoons \mathrm{NH}_{3}+\mathrm{H}_{2} \mathrm{~S}$ (c) $\mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{PO}_{4}{ }^{3-} \rightleftharpoons \mathrm{HPO}_{4}^{2-}+\mathrm{H}_{2} \mathrm{O}$ (d) $\mathrm{HSO}_{3}^{-}+\mathrm{CN}^{-} \rightleftharpoons \mathrm{HCN}+\mathrm{SO}_{3}^{2-}$ (e) $\mathrm{O}^{2-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{OH}^{-}+\mathrm{OH}^{-}$.
Identify the Bronsted-Lowry acids and bases in these reactions and group them into conjugate acid-base pairs. (a) $\mathrm{NH}_{3}+\mathrm{HBr} \rightleftharpoons \mathrm{NH}_{4}^{+}+\mathrm{Br}^{-}$ (b) $\mathrm{NH}_{4}^{+}+\mathrm{HS}^{-} \rightleftharpoons \mathrm{NH}_{3}+\mathrm{H}_{2} \mathrm{~S}$ (c) $\mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{PO}_{4}^{3-} \rightleftharpoons \mathrm{HPO}_{4}^{2-}+\mathrm{H}_{2} \mathrm{O}$ (d) $\mathrm{HSO}_{3}^{-}+\mathrm{CN}^{-} \rightleftharpoons \mathrm{HCN}+\mathrm{SO}_{3}^{2-}$ (e) $\mathrm{O}^{2-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{OH}^{-}+\mathrm{OH}^{-}$
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