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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=

Chemistry for Engineering Students
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 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...
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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).
Transcribed Image Text: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=
Transcribed Image Text: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=
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