**Solubility and Ksp Calculation**At 25 °C, only 0.0330 mol of the generic salt AB₃ is soluble in 1.00 L of water.**Question:**What is the \( K_{sp} \) of the salt at 25 °C?**Dissolution Reaction:**\[ \text{AB}_3(s) \rightleftharpoons \text{A}^{3+}(aq) + 3 \text{B}^-(aq) \]**Calculation:**\[ K_{sp} = \]**Explanation:**The solubility product constant (\( K_{sp} \)) is an equilibrium constant that measures the solubility of a compound. It is determined by how much of the salt dissolves into its ions in water. 1. **Stoichiometry**: - For every 1 mole of AB₃ that dissolves, 1 mole of A³⁺ is produced and 3 moles of B⁻ are produced.2. **Ionic Concentrations**: - [A³⁺] = 0.0330 M - [B⁻] = 3 × 0.0330 M = 0.0990 M3. **Expression for \( K_{sp} \)**: - \( K_{sp} = [A^{3+}][B^-]^3 \)Substitute the concentrations into the expression to calculate \( K_{sp} \).

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Answered: At 25 °C, only 0.0330 mol of the…

At 25 °C, only 0.0330 mol of the generic salt AB3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB,(s) = A+(aq) + 3 B¯(aq) Ksp %3D

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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