Math

QuestionAccording to the Bronsted-Lowry theory, an acid is any substance (molecule or ion) that can transfer a proton ( H+\mathrm{H}^{+}ion) to another substance, and a base is any substance that can accept a proton. Acid-base reactions are proton-transfer reactions, as follows: HA+BBH++A acid acid base \begin{array}{l} \mathrm{HA}+\mathrm{B} \rightleftharpoons \mathrm{BH}^{+}+\underset{\text { acid }}{\mathrm{A}^{-}} \\ \text {acid base } \end{array}
Chemical species whose formulas differ only by one proton are said to be conjugate acid-base pairs. Thus, A\mathrm{A}^{-}is the conjugate base of the acid HA, and HA is the conjugate acid of the base A\mathrm{A}^{-}. Similarly, B is the conjugate base of the acid BH+\mathrm{BH}^{+}, and BH+\mathrm{BH}^{+}is the conjugate acid of the base B . The stronger the acid, the weaker the conjugate base, and the stronger the base, the weaker the conjugate acid.
What is the conjugate base of HSO3\mathrm{HSO}_{3}{ }^{-}? Express your answer as a chemical formula. View Available Hint(s) \square Submit
Part C
What is the conjugate acid of HPO22\mathrm{HPO}_{2}{ }^{2-} ? Express your answer as a chemical formula. View Available Hint(s) \square \qquad A chemical reaction does not occur for this question.

Studdy Solution
The conjugate base of HSO3\mathrm{HSO}_{3}{ }^{-} is SO32\mathrm{SO}_{3}{ }^{2-}.
The conjugate acid of HPO22\mathrm{HPO}_{2}{ }^{2-} is H2PO2\mathrm{H}_{2}\mathrm{PO}_{2}{ }^{-}.

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