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What pH would you raise a water sample to, to decrease the concentration of dissolved Mg2+ from 100 mg Mg2+/L to 30 mg Mg2+/L? Use the following values and the integrated Van Hoff equation to solve. Hof (Mg+2(aq)) = -466.8 kJ/mol Hof (Mg(OH)2(s)) = -924.5 kJ/mol In[(K (2))/(K_(1))]=(\Delta H^ (0))/(R)\times ((1)/(T-(1))-(1)/(T (2))) To solve this problem, you must use temperature adjusted values for all equilibrium constants, including Kw. K ΔΗ 1 1 In ✗ K₁₁ R T₁ T₂

What pH would you raise a water sample to, to decrease the concentration of dissolved Mg2+ from 100 mg Mg2+/L to 30 mg Mg2+/L? Use the following values and the integrated Van Hoff equation to solve. Hof (Mg+2(aq)) = -466.8 kJ/mol Hof (Mg(OH)2(s)) = -924.5 kJ/mol In[(K (2))/(K_(1))]=(\Delta H^ (0))/(R)\times ((1)/(T-(1))-(1)/(T (2))) To solve this problem, you must use temperature adjusted values for all equilibrium constants, including Kw. K ΔΗ 1 1 In ✗ K₁₁ R T₁ T₂

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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What pH would you raise a water sample to, to decrease the concentration of dissolved Mg2+ from 100 mg Mg2+/L to 30 mg Mg2+/L? Use the following values and the integrated Van Hoff equation to solve. Hof (Mg+2(aq)) = -466.8 kJ/mol Hof (Mg(OH)2(s)) = -924.5 kJ/mol In[(K (2))/(K_(1))]=(\Delta H^ (0))/(R)\times ((1)/(T-(1))-(1)/(T (2))) To solve this problem, you must use temperature adjusted values for all equilibrium constants, including Kw. K ΔΗ 1 1 In ✗ K₁₁ R T₁ T₂
Transcribed Image Text:What pH would you raise a water sample to, to decrease the concentration of dissolved Mg2+ from 100 mg Mg2+/L to 30 mg Mg2+/L? Use the following values and the integrated Van Hoff equation to solve. Hof (Mg+2(aq)) = -466.8 kJ/mol Hof (Mg(OH)2(s)) = -924.5 kJ/mol In[(K (2))/(K_(1))]=(\Delta H^ (0))/(R)\times ((1)/(T-(1))-(1)/(T (2))) To solve this problem, you must use temperature adjusted values for all equilibrium constants, including Kw. K ΔΗ 1 1 In ✗ K₁₁ R T₁ T₂
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