G.288. Consider the insoluble compound aluminum phosphate, AIPO4 The aluminum ion also forms acomplex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of AIPO4(s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction.For Al(OH)4, K= 7.7x1033. Be sure to specify states such as (aq) or (s).K=Ag(s)+K= 5.6x10^182Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex withcyanide ions. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases inthe presence of cyanide ions and calculate the equilibrium constant for this reaction.For Ag (CN)₂, K₁= 5.6x1018. Be sure to specify states such as (aq) or (s).++2CN(aq) Ag(CN)₂ (aq) + OH(aq)

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Consider the insoluble compound aluminum phosphate, AIPO4 The aluminum ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of AIPO4 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Al(OH)4, K = 7.7x1033. Be sure to specify states such as (aq) or (s). K= Ag(s) + K= 5.6x10^18 12 Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ag(CN)₂, K₁= 5.6x1018. Be sure to specify states such as (aq) or (s). + + 2CN(aq) Ag(CN)₂ (aq) + OH(aq)

Consider the insoluble compound aluminum phosphate, AIPO4 The aluminum ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of AIPO4 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Al(OH)4, K = 7.7x1033. Be sure to specify states such as (aq) or (s). K= Ag(s) + K= 5.6x10^18 12 Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ag(CN)₂, K₁= 5.6x1018. Be sure to specify states such as (aq) or (s). + + 2CN(aq) Ag(CN)₂ (aq) + OH(aq)

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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