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Write the equilibrium constant expression for the following reaction: H3PO4(aq) + 3 H20(1) = PO*(aq) + 3 H3O*(aq)

Write the equilibrium constant expression for the following reaction: H3PO4(aq) + 3 H20(1) = PO*(aq) + 3 H3O*(aq)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Topic: Equilibrium Constant Expression** *Write the equilibrium constant expression for the following reaction:* \[ \text{H}_3\text{PO}_4(\text{aq}) + 3 \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{PO}_4^{3-}(\text{aq}) + 3 \text{H}_3\text{O}^+(\text{aq}) \] --- **Explanation:** To write the equilibrium constant expression (\(K_c\)) for a given reaction, follow these steps: >The general form of the equilibrium constant expression for a reaction: \[ aA + bB \rightleftharpoons cC + dD \] is given by: \[ K_c = \frac{[\text{C}]^c [\text{D}]^d}{[\text{A}]^a [\text{B}]^b} \] For the given reaction: \[ \text{H}_3\text{PO}_4(\text{aq}) + 3 \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{PO}_4^{3-}(\text{aq}) + 3 \text{H}_3\text{O}^+(\text{aq}) \] >The equilibrium constant expression is: \[ K_c = \frac{[\text{PO}_4^{3-}] [\text{H}_3\text{O}^+]^3}{[\text{H}_3\text{PO}_4]} \] Note that the concentration of water (\( \text{H}_2\text{O} \)) is not included in the equilibrium expression because it is a pure liquid, and its concentration is considered constant. --- **Key Points to Remember:** 1. The products of the reaction appear in the numerator. 2. The reactants of the reaction appear in the denominator. 3. Each concentration term is raised to the power of its coefficient in the balanced chemical equation. 4. Pure solids and pure liquids do not appear in the equilibrium constant expression.
Transcribed Image Text:**Topic: Equilibrium Constant Expression** *Write the equilibrium constant expression for the following reaction:* \[ \text{H}_3\text{PO}_4(\text{aq}) + 3 \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{PO}_4^{3-}(\text{aq}) + 3 \text{H}_3\text{O}^+(\text{aq}) \] --- **Explanation:** To write the equilibrium constant expression (\(K_c\)) for a given reaction, follow these steps: >The general form of the equilibrium constant expression for a reaction: \[ aA + bB \rightleftharpoons cC + dD \] is given by: \[ K_c = \frac{[\text{C}]^c [\text{D}]^d}{[\text{A}]^a [\text{B}]^b} \] For the given reaction: \[ \text{H}_3\text{PO}_4(\text{aq}) + 3 \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{PO}_4^{3-}(\text{aq}) + 3 \text{H}_3\text{O}^+(\text{aq}) \] >The equilibrium constant expression is: \[ K_c = \frac{[\text{PO}_4^{3-}] [\text{H}_3\text{O}^+]^3}{[\text{H}_3\text{PO}_4]} \] Note that the concentration of water (\( \text{H}_2\text{O} \)) is not included in the equilibrium expression because it is a pure liquid, and its concentration is considered constant. --- **Key Points to Remember:** 1. The products of the reaction appear in the numerator. 2. The reactants of the reaction appear in the denominator. 3. Each concentration term is raised to the power of its coefficient in the balanced chemical equation. 4. Pure solids and pure liquids do not appear in the equilibrium constant expression.
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