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Consider the insoluble compound zine hydroxide , Zn(OH), . The zinc ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of Za(OH), (9) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH,),", K- 2.9x10". Be sure to specify states such as (aq) or (8).

Consider the insoluble compound zine hydroxide , Zn(OH), . The zinc ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of Za(OH), (9) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH,),", K- 2.9x10". Be sure to specify states such as (aq) or (8).

Principles of Modern Chemistry
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 37P
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Consider the insoluble compound zine hydroxide , Zn(OH), . The zince ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Zn(OH), (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH,)," , K= 2.9x10°. Be sure to specify states such as (aq) or (s).
Transcribed Image Text:Consider the insoluble compound zine hydroxide , Zn(OH), . The zince ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Zn(OH), (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH,)," , K= 2.9x10°. Be sure to specify states such as (aq) or (s).
Consider the insoluble compound iron(II) sulfide , Fes. The iron(II) ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Fes (s) increases in the presence of eyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN),*, K- 7.7x10. Be sure to specify states such as (aq) or (s).
Transcribed Image Text:Consider the insoluble compound iron(II) sulfide , Fes. The iron(II) ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Fes (s) increases in the presence of eyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN),*, K- 7.7x10. Be sure to specify states such as (aq) or (s).
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