Consider the insoluble compound silver chloride , AgCI. The silver ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of AgCI (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ag(CN),", Kp= 5.6×1018 . Use the pull-down boxes to specify states such as (aq) or (s). Consider the insoluble compound copper(II) hydroxide , Cu(OH)2 . The copper(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Cu(OH), (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3),* , K = 6.8×1012 . Use the pull-down boxes to specify states such as (aq) or (s). K=

Consider the insoluble compound silver chloride , AgCI. The silver ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of AgCI (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ag(CN),", Kp= 5.6×1018 . Use the pull-down boxes to specify states such as (aq) or (s). Consider the insoluble compound copper(II) hydroxide , Cu(OH)2 . The copper(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Cu(OH), (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3),* , K = 6.8×1012 . Use the pull-down boxes 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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