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] = 1.7E7Include at least 3 significant figures in your answer.MGrade This Exercise5. 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. DGrade This Exercise6. Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.71. The solubility product of magnesium hydroxide is 1.2E-11Include at least 3 significant figures in your answer. DM

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Answered: If 283.0 mg of AgBr is completely…

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 for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.11PAE

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Question

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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