A cyanide solution with a volume of 10.33 mL was treated with 22.00 mL of Ni2+ solution (containing excess Ni2+) to convert the cyanide into tetracyanonickelate(II): 4CN−+Ni2+⟶Ni(CN)(2−)/4 The excess Ni2+ was then titrated with 11.85 mL of 0.01303 M ethylenediaminetetraacetic acid (EDTA): Ni2++EDTA4−⟶Ni(EDTA)2− Ni(CN)(2−)/4 does not react with EDTA. If 38.80 mL of EDTA were required to react with 30.47 mL of the original Ni2+ solution, calculate the molarity of CN− in the 10.33 mL cyanide sample. [CN-] = ________________________________M
A cyanide solution with a volume of 10.33 mL was treated with 22.00 mL of Ni2+ solution (containing excess Ni2+) to convert the cyanide into tetracyanonickelate(II): 4CN−+Ni2+⟶Ni(CN)(2−)/4 The excess Ni2+ was then titrated with 11.85 mL of 0.01303 M ethylenediaminetetraacetic acid (EDTA): Ni2++EDTA4−⟶Ni(EDTA)2− Ni(CN)(2−)/4 does not react with EDTA. If 38.80 mL of EDTA were required to react with 30.47 mL of the original Ni2+ solution, calculate the molarity of CN− in the 10.33 mL cyanide sample. [CN-] = ________________________________M
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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A cyanide solution with a volume of 10.33 mL was treated with 22.00 mL of Ni2+ solution (containing excess Ni2+) to convert the cyanide into tetracyanonickelate(II):
4CN−+Ni2+⟶Ni(CN)(2−)/4
The excess Ni2+ was then titrated with 11.85 mL of 0.01303 M ethylenediaminetetraacetic acid (EDTA):
Ni2++EDTA4−⟶Ni(EDTA)2−
Ni(CN)(2−)/4 does not react with EDTA. If 38.80 mL of EDTA were required to react with 30.47 mL of the original Ni2+ solution, calculate the molarity of CN− in the 10.33 mL cyanide sample.
[CN-] = ________________________________M
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