show why the solubility of Ag3PO4 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Consider only the FIRST STEP in the reaction with strong acid. Be sure to specify states such as (aq)

show why the solubility of Ag3PO4 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Consider only the FIRST STEP in the reaction with strong acid. Be sure to specify states such as (aq)

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 68QAP

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Question

Write a balanced net ionic equation to show why the solubility of Ag₃PO₄ (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.

Consider only the FIRST STEP in the reaction with strong acid. Be sure to specify states such as (aq) or (s).

K =

(K net= K sp / K a = )

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