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).
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 cyanide ions and calculate the equilibrium constant for this
reaction.
For Fe(CN),+ , Kf= 7.7×1036 . Be sure to specify states such as (aq) or (s).
K =
+
Transcribed Image Text:Consider the insoluble compound zinc carbonate , ZnCO3 . The zinc ion also forms a complex with ammonia . Write a balanced net ionic
equation to show why the solubility of ZnCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this
reaction.
For Zn(NH3),* , Kf=2.9×10° . Be sure to specify states such as (aq) or (s).
+
K=
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