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Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)4². Calculate the concentration of free Zn2+ ion when 1.49x102 mol Zn(CH3COO)₂(s) is added to 1.00 L of solution in which [OH ] is held constant (buffered at pH 12.70). For Zn(OH)42, Kr= 4.6x1017. [Zn²+] = M

Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)4². Calculate the concentration of free Zn2+ ion when 1.49x102 mol Zn(CH3COO)₂(s) is added to 1.00 L of solution in which [OH ] is held constant (buffered at pH 12.70). For Zn(OH)42, Kr= 4.6x1017. [Zn²+] = M

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 65E: Sometimes equilibria fur complex ions are described in terms of dissociation constants. Kd . For the...
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Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH, the Zn2+ (aq) ion forms a hydroxide complex ion, Zn(OH)42. Calculate the concentration of free Zn2+ ion when 1.49x102 mol Zn(CH3COO)₂(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.70). For Zn(OH)42, K = 4.6x1017. [Zn²+] = M
Transcribed Image Text:Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH, the Zn2+ (aq) ion forms a hydroxide complex ion, Zn(OH)42. Calculate the concentration of free Zn2+ ion when 1.49x102 mol Zn(CH3COO)₂(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.70). For Zn(OH)42, K = 4.6x1017. [Zn²+] = M
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