For each of the following reactions, identify the Brønsted-Lowry acid and base on the reactant side of the equation, and the conjugate acid and conjugate base on the product side.

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∻Solution∻ ‖ 1 ⋮ **Identify the Brønsted-Lowry acid and base in the reactants**: According to the Brønsted-Lowry theory, an acid is a substance that can donate a proton (H⁺), and a base is a substance that can accept a proton. ‖ ‖ 2 ⋮ **Identify the conjugate acid and conjugate base in the products**: After a Brønsted-Lowry acid donates a proton, it becomes a conjugate base. Similarly, after a Brønsted-Lowry base accepts a proton, it becomes a conjugate acid. ‖ ‖ 3 ⋮ **Apply the concept to the given reaction**: In the reaction between NH₄⁺ (ammonium) and CN⁻ (cyanide), NH₄⁺ donates a proton to become NH₃ (ammonia), making it the acid, and CN⁻ accepts a proton to become HCN (hydrogen cyanide), making it the base. Therefore, NH₃ is the conjugate base of NH₄⁺, and HCN is the conjugate acid of CN⁻. ‖ ∻Answer∻ ⚹ Acid: NH₄⁺ ⚹ Base: CN⁻ ⚹ Conjugate Base: NH₃ ⚹ Conjugate Acid: HCN ⚹ ∻Key Concept∻ ⚹ Brønsted-Lowry acids and bases ⚹ ∻Explanation∻ ⚹ An acid donates a proton to become a conjugate base, and a base accepts a proton to become a conjugate acid. ⚹◊What is the chemical equation for the reaction between NH₄⁺ and CN⁻ ions?⍭ Generate me a similar question◊⚹

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