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Calculate the molar solubility of  Mg(OH)2 in water in 0.25M NaOH(aq)

Calculate the molar solubility of  Mg(OH)2 in water in 0.25M NaOH(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
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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Calculate the molar solubility of  Mg(OH)2

  1. in water
  2. in 0.25M NaOH(aq)
### Acid Dissociation Constants (Ka): - **HF (Hydrofluoric acid):** \( K_a = 7.1 \times 10^{-4} \) - **HNO₂ (Nitrous acid):** \( K_a = 4.5 \times 10^{-4} \) - **HCOOH (Formic acid):** \( K_a = 1.7 \times 10^{-4} \) - **HC₃H₆O₃ (Lactic acid):** \( K_a = 1.4 \times 10^{-4} \) - **CH₃CH₂COOH (Propionic acid):** \( K_a = 1.3 \times 10^{-5} \) - **CH₃COOH (Acetic acid):** \( K_a = 1.8 \times 10^{-5} \) - **C₆H₅COOH (Benzoic acid):** \( K_a = 6.3 \times 10^{-5} \) - **HCN (Hydrocyanic acid):** \( K_a = 4.9 \times 10^{-10} \) ### Base Dissociation Constants (Kb): - **CH₃NH₂ (Methylamine):** \( K_b = 4.4 \times 10^{-4} \) - **NH₃ (Ammonia):** \( K_b = 1.8 \times 10^{-5} \) - **C₅H₅N (Pyridine):** \( K_b = 1.7 \times 10^{-9} \) ### Solubility Product Constants (Ksp): - **PbCl₂ (Lead(II) chloride):** \( K_{sp} = 1.7 \times 10^{-5} \) - **CuCl (Copper(I) chloride):** \( K_{sp} = 1.9 \times 10^{-7} \) - **Mg(OH)₂ (Magnesium hydroxide):** \( K_{sp} = 1.8 \times 10^{-11} \) This table provides valuable constants used for calculating the degree of ionization of acids and bases in solution, and for determining the solubility of compounds in aqueous solutions.
Transcribed Image Text:### Acid Dissociation Constants (Ka): - **HF (Hydrofluoric acid):** \( K_a = 7.1 \times 10^{-4} \) - **HNO₂ (Nitrous acid):** \( K_a = 4.5 \times 10^{-4} \) - **HCOOH (Formic acid):** \( K_a = 1.7 \times 10^{-4} \) - **HC₃H₆O₃ (Lactic acid):** \( K_a = 1.4 \times 10^{-4} \) - **CH₃CH₂COOH (Propionic acid):** \( K_a = 1.3 \times 10^{-5} \) - **CH₃COOH (Acetic acid):** \( K_a = 1.8 \times 10^{-5} \) - **C₆H₅COOH (Benzoic acid):** \( K_a = 6.3 \times 10^{-5} \) - **HCN (Hydrocyanic acid):** \( K_a = 4.9 \times 10^{-10} \) ### Base Dissociation Constants (Kb): - **CH₃NH₂ (Methylamine):** \( K_b = 4.4 \times 10^{-4} \) - **NH₃ (Ammonia):** \( K_b = 1.8 \times 10^{-5} \) - **C₅H₅N (Pyridine):** \( K_b = 1.7 \times 10^{-9} \) ### Solubility Product Constants (Ksp): - **PbCl₂ (Lead(II) chloride):** \( K_{sp} = 1.7 \times 10^{-5} \) - **CuCl (Copper(I) chloride):** \( K_{sp} = 1.9 \times 10^{-7} \) - **Mg(OH)₂ (Magnesium hydroxide):** \( K_{sp} = 1.8 \times 10^{-11} \) This table provides valuable constants used for calculating the degree of ionization of acids and bases in solution, and for determining the solubility of compounds in aqueous solutions.
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