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Silver ions form a complex ion in the presence of cyanide ions, according to the following equation: Ag (aq) + 2 CN (aq) = [Ag(CN)₂] M If 0.090 mol of AgNO3 is added to one liter of 1.0 M KCN, what are the equilibrium concentrations of each species in the reaction? [Agt] = [CN] = [[Ag(CN)₂]]= 0.090 M Ke 1.1 x 10¹8 M Question #

Silver ions form a complex ion in the presence of cyanide ions, according to the following equation: Ag (aq) + 2 CN (aq) = [Ag(CN)₂] M If 0.090 mol of AgNO3 is added to one liter of 1.0 M KCN, what are the equilibrium concentrations of each species in the reaction? [Agt] = [CN] = [[Ag(CN)₂]]= 0.090 M Ke 1.1 x 10¹8 M Question #

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section: Chapter Questions
Problem 65PS: You have a solution that has a lead(II) ion concentration of 0.0012 M. If enough soluble...
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Silver ions form a complex ion in the presence of cyanide ions, according to the following equation: Ag (aq) + 2 CN (aq) [Ag(CN)₂] M If 0.090 mol of AgNO3 is added to one liter of 1.0 M KCN, what are the equilibrium concentrations of each species in the reaction? [Agt] = [CN] = [[Ag(CN)₂]]= 0.090 M Ke 1.1 x 10¹8 M Question #6
Transcribed Image Text:Silver ions form a complex ion in the presence of cyanide ions, according to the following equation: Ag (aq) + 2 CN (aq) [Ag(CN)₂] M If 0.090 mol of AgNO3 is added to one liter of 1.0 M KCN, what are the equilibrium concentrations of each species in the reaction? [Agt] = [CN] = [[Ag(CN)₂]]= 0.090 M Ke 1.1 x 10¹8 M Question #6
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