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olid iron(II) nitrate is slowly added to 175 mL of a 0.0363 M ammonium sulfide solution. The oncentration of iron(II) ion required to just initiate precipitation is M. Submit Answer Retry Entire Group 9 more group attempts remaining

olid iron(II) nitrate is slowly added to 175 mL of a 0.0363 M ammonium sulfide solution. The oncentration of iron(II) ion required to just initiate precipitation is M. Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.98QE
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Solid iron(II) nitrate is slowly added to 175 mL of a 0.0363 M ammonium sulfide solution. The concentration of iron(II) ion required to just initiate precipitation is M. Submit Answer Retry Entire Group 9 more group attempts remaining 7
Transcribed Image Text:Solid iron(II) nitrate is slowly added to 175 mL of a 0.0363 M ammonium sulfide solution. The concentration of iron(II) ion required to just initiate precipitation is M. Submit Answer Retry Entire Group 9 more group attempts remaining 7
Consider the insoluble compound iron(II) hydroxide, Fe(OH)2. The iron(II) ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Fe(OH)2 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN)64, K₁= 7.7×1036. Be sure to specify states such as (aq) or (s). K= +
Transcribed Image Text:Consider the insoluble compound iron(II) hydroxide, Fe(OH)2. The iron(II) ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Fe(OH)2 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN)64, K₁= 7.7×1036. Be sure to specify states such as (aq) or (s). K= +
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