Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of AgCl (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ag(CN)₂, Kf = 5.6x10¹8. Be sure to specify states such as (aq) or (s). K = + +

Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of AgCl (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ag(CN)₂, Kf = 5.6x10¹8. Be sure to specify states such as (aq) or (s). K = + +

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 70AP

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