4. For the following reaction, identify the Bronsted-Lowry acid and base and the conjugate acid-base pairs: H2PO3-(aq) + H2O(l) ? HPO3 2-(aq) + H3O+(aq) a) the Bronsted Acid ______ and its conjugate base ______ b) the Bronsted Base ______ and its conjugate acid ______
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In this reaction, HPO4-(aq) donates a proton (H+) to H2O(l). Therefore, HPO4-(aq) is acting as the Bronsted-Lowry acid. H2O(l) accepts the proton (H+) from HPO4-(aq). Therefore, H2O(l) is acting as the Bronsted-Lowry base. Show more…
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