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Chapter 12: Q28P (page 285)

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

Short Answer

Expert verified

When an analyte replaces a metal ion and results in formation of a complex. Then it is known as Displacement titration.

Displacement of Ni2+ from NiCN42-using the analyte Ag+. Then the displaced Ni2+is titrated by EDTA in order to determine the amount of Ag+present.

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. There are several types of EDTA titration techniques like direct titration, indirect titration, back titration, displacement titration, etc.

02

Displacement Titration

When an analyte replaces a metal ion from a complex and titrates with that displaced metal ion, then it is called displacement titration.

03

Example of Displacement Titration

Displacement of Ni2+ from NiCN42-using the analyte Ag+. Then the displaced Ni2+is titrated by EDTA in order to determine the amount of Ag+present

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Most popular questions from this chapter

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

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

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?

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

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+
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