A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 M Na2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer until the pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator. Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, on which the solution will turn red. Calculate for the molarity of the unknown.
A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 M Na2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer until the pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator. Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, on which the solution will turn red. Calculate for the molarity of the unknown.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
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 31PS: Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH...
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A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 M
Na2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer until
the pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator.
Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, on
which the solution will turn red. Calculate for the molarity of the unknown.
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