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Chapter 12: Q8P-b (page 283)

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

Short Answer

Expert verified

(b) For 20 mL the value ofpMn2+is 2.175.

Step by step solution

01

Introduction

Equations and data obtained in order to proceed for calculation are as follows

Titration  Reaction: Mn2++EDTA⇌MnY2−Kf=1013.89At   pH   8  αY4−=4.2×10−3 Table 12−1

02

Determine equilibrium constant

Kf'=αY4−×Kf=4.2×10−3×1013.89=3.3×1011

Equivalence point=50 mL

03

Determine the value of pMn2+

The concentration of the remaining productcan be calculated using the following equation

=Fraction remaining × Initial concentration × Dilution factor

If 20 mL solution is added then the reaction will be 20/50 completed as the equivalence point is at 50 mL. Then the metal (Mn) concentration will be

Mn2+=50−20500.02 M2525+20=6.67×10−3 M

Therefore, the value of pMn2+

pMn2+=−logMn2+=−log6.67×10−3=2.175

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Most popular questions from this chapter

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

Calcium ion was titrated with EDTA at pH 11, using Calmagite as indicator (Table 12-3). Which is the principal species of Calmagite at pH 11? What color was observed before the equivalence point? After the equivalence point?

Pyrocatechol violet(Table 12-3) is to be used as a metal ion indicator in an EDTA titration. The procedure is as follows:

1. Add a known excess of EDTA to the unknown metal ion.

2. Adjust the pH with a suitable buffer.

3. Back-titrate the excess chelate with standard Al3+.

From the following available buffers, select the best buffer, and then state what color change will be observed at the end point. Explain your answer.

  1. pH 6–7 (ii) pH 7–8 (iii) pH 8–9 (iv) pH 9–10

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−⇌Cu(CH3CO2)+       β1(=K1)Cu2++2CH3CO2−⇌Cu(CH3CO2)2       β2

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

Cu(CH3CO2)++CH3CO2−⇌Cu(CH3CO2)2(aq)   K2

(b) Consider 1.00 L of solution prepared by mixing 1.00 × 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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