Write balanced equations for the reactions of (a) H3PO4 and (b) B1OH23 with water. Classify each acid as a Brønsted–Lowry acid or a Lewis acid.

Verified step by step guidance

Step 1: Identify the chemical formulas for the given acids. For (a) H3PO4 is phosphoric acid, and for (b) B1OH23, it seems like a typo or unconventional notation. Assuming it refers to a boron compound, let's consider a typical boron compound like B(OH)3, boric acid.

Step 2: Write the balanced chemical equation for the reaction of H3PO4 with water. H3PO4 is a Brønsted–Lowry acid, which donates a proton (H+) to water, forming H2PO4- and H3O+.

Step 3: Write the balanced chemical equation for the reaction of B(OH)3 with water. B(OH)3 acts as a Lewis acid, accepting a pair of electrons from water to form a complex, typically B(OH)4- and H+.

Step 4: Classify each acid. H3PO4 is a Brønsted–Lowry acid because it donates a proton to water. B(OH)3 is a Lewis acid because it accepts an electron pair from water.

Step 5: Review the definitions: A Brønsted–Lowry acid is a substance that donates a proton (H+), while a Lewis acid is a substance that accepts an electron pair.

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