both questions goes together.... thanks! Consider the insoluble compound iron(II) sulfide , FeS . The iron(II) ion also forms a complex with cyanide ions . Write a balanced netionic equation to show why the solubility of FeS (s) increases in the presence of cyanide ions and calculate the equilibrium constant for thisreaction.For Fe(CN),+ , Kf= 7.7×1036 . Be sure to specify states such as (aq) or (s).K =+ Consider the insoluble compound zinc carbonate , ZnCO3 . The zinc ion also forms a complex with ammonia . Write a balanced net ionicequation to show why the solubility of ZnCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for thisreaction.For Zn(NH3),* , Kf=2.9×10° . Be sure to specify states such as (aq) or (s).+K=

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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 cyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN),+ , K= 7.7×1036 . 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 cyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN),+ , K= 7.7×1036 . Be sure to specify states such as (aq) or (s).

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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