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If 283.0 mg of AgBr is completely dissolved in 143.0 mL of 0.2 M NH3, what is the equilibrium concentration of Ag* (aq) in the final solution? K[Ag(NH3)2] = 1.7E7

If 283.0 mg of AgBr is completely dissolved in 143.0 mL of 0.2 M NH3, what is the equilibrium concentration of Ag* (aq) in the final solution? K[Ag(NH3)2] = 1.7E7

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
Problem 76QAP
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4. If 283.0 mg of AgBr is completely dissolved in 143.0 mL of 0.2 M NH3, what is the equilibrium concentration of Ag* (aq) in the final solution? K[Ag(NH3)2] = 1.7E7 Include at least 3 significant figures in your answer. M Grade This Exercise 5. The acid ionization constant of Fe(H₂O)2+ (aq) is 3E-6. Compute the pH of a 0.11 M aqueous solution of Fe(NO3)2- Include at least 3 significant figures in your answer. D Grade This Exercise 6. Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.71. The solubility product of magnesium hydroxide is 1.2E-11 Include at least 3 significant figures in your answer. D M
Transcribed Image Text:4. If 283.0 mg of AgBr is completely dissolved in 143.0 mL of 0.2 M NH3, what is the equilibrium concentration of Ag* (aq) in the final solution? K[Ag(NH3)2] = 1.7E7 Include at least 3 significant figures in your answer. M Grade This Exercise 5. The acid ionization constant of Fe(H₂O)2+ (aq) is 3E-6. Compute the pH of a 0.11 M aqueous solution of Fe(NO3)2- Include at least 3 significant figures in your answer. D Grade This Exercise 6. Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.71. The solubility product of magnesium hydroxide is 1.2E-11 Include at least 3 significant figures in your answer. D M
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