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Chapter 12: Q24P (page 285)

List four methods for detecting the end point of an EDTA Titration

Short Answer

Expert verified

The four methods for detecting the end point of an EDTA titration are

a) With metal ion indicators

b) With a glass electrode

c) With a mercury electrode

d) With an ion selective electrode.

Step by step solution

01

EDTA

EDTA, also known as ethylenediaminetetraacetic acid forms strong complexes with metal ions and plays a major role in quantitative analysis. In industries it is used as a metal binding agent and used in production of detergents, cleaning agents, food additives etc

02

EDTA titration

In most of the cases little amount of indicator is induced at the beginning of the titration experiment. EDTA is then added to the colorless metalcomplex solution and reacts until all the free metal ions are consumed.

03

List of methods

The four methods for detecting the end point of an EDTA titration are

a) With metal ion indicators

b) With a glass electrode

c) With a mercury electrode

d) With an ion selective electrode.

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Most popular questions from this chapter

A 50.0-mL sample containing Ni2+ was treated with 25.0 mL of 0.050 0 M EDTA to complex all the Ni2+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 5.00 mL of 0.050 0 M Zn2+. What was the concentration of Ni2+ in the original solution?

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

A 25.00-mL sample containing Fe3+ and Cu2+ required 16.06 mL of 0.050 83 M EDTA for complete titration. A 50.00-mL sample of the unknown was treated with NH4F to protect the Fe3+. Then Cu2+ was reduced and masked by thiourea. Addition of 25.00 mL of 0.050 83 M EDTA liberated Fe3+ from its fluoride complex to form an EDTA complex. The excess EDTA required 19.77 mL of 0.018 83 M Pb2+ to reach a xylenol orange end point. Find [Cu2+] in the unknown.

Consider the titration of 25.0 mL of 0.020 0 M MnSO4 with 0.010 0 M EDTA in a solution buffered to pH 8.00. Calculate pMn2+ at the following volumes of added EDTA and sketch the titration curve:

(a) 0 mL (b) 20.0 mL (c) 40.0 mL (d) 49.0 mL (e) 49.9 mL (f) 50.0 mL (g) 50.1 mL(h) 55.0 mL (i) 60.0 mL

Potassium ion in a 250.0 (卤0.1) mL water sample was precipitated with sodium tetraphenylborate:

K++(C6H5)4B-鈫�KB(C6H5)4(s)

The precipitate was filtered, washed, dissolved in an organic solvent, and treated with excess Hg (EDTA)2-:

4HgY2-+(C6H5)4B-+4H2O鈫�H3BO3+4C6H5Hg++4HY3-+OH-

The liberated EDTA was titrated with 28.73 (卤0.03) mL of 0.043 7 (卤0.000 1) M Zn2+. Find [K+] (and its absolute uncertainty) in the original sample.
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