Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgCl (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3)2+, Kf = 1.6x107. Be sure to specify states such as (aq) or (s). K = + +

Chemistry: Principles and Practice
3rd Edition
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.70QE
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Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with ammonia.
Write a balanced net ionic equation to show why the solubility of AgCl (s) increases in the presence of ammonia
and calculate the equilibrium constant for this reaction.
1.6x107. Be sure to specify states such as (aq) or (s).
For Ag(NH3)2+, Kf
=
K=
+
Use the References to access important values if needed for this question.
Submit Answer
+
Retry Entire Group 2 more group attempts remaining
Transcribed Image Text:Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgCl (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. 1.6x107. Be sure to specify states such as (aq) or (s). For Ag(NH3)2+, Kf = K= + Use the References to access important values if needed for this question. Submit Answer + Retry Entire Group 2 more group attempts remaining
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