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Chapter 12: Q14P (page 283)

State the purpose of an auxiliary complexing agent and give an example of its use.

Short Answer

Expert verified

The bond between metal cation and the auxiliary complexing agent must be strong enough so that precipitation of hydroxide can be prevented as well as without interference with EDTA titration.

NH3 retains Zn2+ in solution at high pH , but easily displaced by EDTA

Step by step solution

01

Introduction

If an auxiliary complexing agent is induced while EDTA titration, formation of hydroxide became restricted. This agent is added if any of the titration solution is a metal cation.

02

Purpose

The bond between metal cation and the auxiliary complexing agent must be strong enough so that precipitation of hydroxide can be prevented as well as without interference with EDTA titration.

03

Example

NH3 retains Zn2+ in solution at high pH , but easily displaced by EDTA

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Most popular questions from this chapter

According to Appendix I, Cu2+ forms two complexes with acetate:

Cu2++CH3CO2鈭�鈬�Cu(CH3CO2)+鈥夆赌夆赌夆赌夆赌夆赌夆赌�尾1(=K1)Cu2++2CH3CO2鈭�鈬�Cu(CH3CO2)2鈥夆赌夆赌夆赌夆赌夆赌夆赌�尾2

(a) Referring to Box 6-2, find K2 for the reaction

Cu(CH3CO2)++CH3CO2鈭�鈬�Cu(CH3CO2)2(aq)鈥夆赌夆赌�K2

(b) Consider 1.00 L of solution prepared by mixing 1.00 脳 10-4 mol Cu(ClO4)2 and 0.100 mol CH3CO2Na. Use Equation 12-16 to find the fraction of copper in the form Cu2+

Describe what is done in a displacement titration and give an Example

If back titration required 13.00 mL Zn2+, what was the original concentration of Ni2+?

A 1.000-mL sample of unknown containing Co2+ and Ni2+ was treated with 25.00 mL of 0.038 72 M EDTA. Back titration with 0.021 27 M Zn2+ at pH 5 required 23.54 mL to reach the xylenol orange end point. A 2.000-mL sample of unknown was passed through an ion-exchange column that retards Co2+ more than Ni2+. The Ni2+ that passed through the column was treated with 25.00 mL of 0.038 72 M EDTA and required 25.63 mL of 0.021 27 M Zn2+ for back titration. The Co2+ emerged from the column later. It, too, was treated with 25.00 mL of 0.038 72 M EDTA. How many milliliters of 0.021 27 M Zn2+ will be required for back titration?

Cyanide solution (12.73 mL) was treated with 25.00 mL of Ni2+ solution (containing excess Ni2+) to convert the cyanide into tetracyano nickelate (II):

4CN-+Ni2+鈫�Ni(CN)42-

Excess Ni2+ was then titrated with 10.15 mL of 0.01307 M EDTA. Ni(CN)42-does not react with EDTA. If 39.35 mL of EDTA were required to react with 30.10 mL of the original Ni2+ solution, calculate the molarity of CN- in the 12.73-mL sample.
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