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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

Find [Ca2+] in 0.10 M CaY2- at pH 8.00

Calculate the concentration of H2Y2- at the equivalence point in Exercise 12-C

Calculate pCu2+ at each of the following points in the titration of 50.00 mL of 0.001 00 M Cu2+ with 0.00100 M EDTA at pH 11.00 in a solution with [NH3] fixed at 1.00 M:

(a) 0 mL(b) 1.00 mL (c) 45.00 mL (d) 50.00 mL (e) 55.00 mL

Indirect EDTA determination of cesium. Cesium ion does not form a strong EDTA complex, but it can be analyzed by adding a known excess of NaBiI4 in cold concentrated acetic acid containing excess NaI. Solid Cs3Bi2I9 is precipitated, filtered, and removed. The excess yellow is then titrated with EDTA. The end point occurs when the yellow color disappears. (Sodium thiosulfate is used in the reaction to prevent the liberated from being oxidized to yellow aqueous I2 by O2 from the air.) The precipitation is fairly selective for Cs+. The ions Li+, Na+, K+, and low concentrations of Rb+ do not interfere, although Tl+ does. Suppose that 25.00 mL of unknown containing Cs+ were treated with 25.00 mL of 0.08640 M NaBiI4 and the unreacted Bil4-required 14.24 mL of 0.0437 M EDTA for complete titration. Find the concentration of Cs+ in the unknown.

Spreadsheet equation for auxiliary complexing agent. Consider the titration of metal M (initial concentration = CM, initial volume = VM) with EDTA (concentration = CEDTA, volume added = VEDTA) in the presence of an auxiliary complexing ligand (such as ammonia). Follow the derivation in Section 12-4 to show that the master equation for the titration is

蠒=CEDTAVEDTACMVM=1+Kf鈥测赌�[M]free鈭�[M]free+Kf鈥测赌�[M]freeCMKf鈥测赌�[M]free+[M]free+Kf鈥测赌�[M]free2CEDTA

where Kf''is the conditional formation constant in the presence of auxiliary complexing agent at the fixed pH of the titration (Equation 12-18) and [M]free is the total concentration of metal not bound to EDTA. [M]free is the same as [M] in Equation 12-15. The result is equivalent to Equation 12-11, with [M] replaced by [M]free andKfreplaced by Kf''.
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