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A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu 2+ ] = 1.00 M , and the vanadium compartment contains a vanadium electrode and V 2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H 2 EDTA 2− , resulting in the reaction H 2 EDTA 2 − ( a q ) + V 2 + ( a q ) ⇌ VEDTA 2 − ( a q ) + 2H + ( a q ) K = ? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H 2 EDTA 2− solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K , for the titration reaction. c. Calculate at the halfway point in the titration.

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 17, Problem 159MP
Textbook Problem
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A galvanic cell is based on the following half-reactions:

Chapter 17, Problem 159MP, A galvanic cell is based on the following half-reactions: In this cell, the copper compartment , example  1

In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2−, resulting in the reaction

H 2 EDTA 2 ( a q ) + V 2 + ( a q ) VEDTA 2 ( a q ) + 2H + ( a q ) K = ?

The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2− solution added. At the stoichiometric point, Chapter 17, Problem 159MP, A galvanic cell is based on the following half-reactions: In this cell, the copper compartment , example  2 was observed to be 1 .98 V. The solution was buffered at a pH of 10.00.

a. Calculate Chapter 17, Problem 159MP, A galvanic cell is based on the following half-reactions: In this cell, the copper compartment , example  3 before the titration was carried out.

b. Calculate the value of the equilibrium constant, K, for the titration reaction.

c. Calculate Chapter 17, Problem 159MP, A galvanic cell is based on the following half-reactions: In this cell, the copper compartment , example  4 at the halfway point in the titration.

(a)

Interpretation Introduction

Interpretation: The Ecell  before the titration was carried out is to be calculated. The value of the equilibrium constant (K).for the titration reaction and the value of Ecell at the halfway point in the titration are to be calculated.

Concept introduction: Electrochemical cell is a combination of two half cells in which the two electrodes are joined by a wire and a salt bridge. Electrons flow from anode where oxidation occurs to cathode where reduction takes place. Cell potential is defined as the measure of energy per unit charge available from the redox reaction to carry out the reaction. Equilibrium constant is defined as the ratio of the concentration of products and the concentration of the reactants.

To determine: The Ecell before the titration was carried out.

Explanation of Solution

Explanation

The concentration of [Cu2+] is 1.00 M.

The volume of vanadium solution is 1.00 L.

The concentration of H2EDTA2 is 0.0800 M.

The volume of H2EDTA2 solution added is 500.0 mL.

The Ecell is 1.98 V.

The value of pH is 10.00.

The titration reaction of 1.00 L vanadium with 0.0800 M H2EDTA2 is shown as follows,

H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)

When 500.0 mL H2EDTA2 is added, the initial moles of V2+ present in the solution is same as that of added moles of H2EDTA2. So, the initial moles of V2+ are determined as follows,

Initial moles of V2+=moles of H2EDTA2 added=(Molarity)H2EDTA2×VH2EDTA2

Substitute the values of molarity and volume of H2EDTA2 in the above expression to calculate the moles of V2+.

Initial moles of V2+=moles of H2EDTA2 added=(Molarity)H2EDTA2×VH2EDTA2=(0.0800 M)(500 mL)(1 L1000 mL)=0.0400 mol

Thus, the initial moles of V2+ are 0.0400 mol.

The concentration of V2+ in 1.00 L solution is calculated by using the expression,

Molarity of V2+=Moles of V2+Liters Solution

Substitute the value of moles of V2+ and volume of solution in the above expression to calculate the molarity (concentration) of V2+.

Molarity of V2+=Moles of V2+Liters Solution=0.0400 mol1.00 L=0

(b)

Interpretation Introduction

Interpretation: The Ecell before the titration was carried out is to be calculated. The value of the equilibrium constant (K) for the titration reaction and the value of Ecell at the halfway point in the titration are to be calculated.

Concept introduction: Electrochemical cell is a combination of two half cells in which the two electrodes are joined by a wire and a salt bridge. Electrons flow from anode where oxidation occurs to cathode where reduction takes place. Cell potential is defined as the measure of energy per unit charge available from the redox reaction to carry out the reaction. Equilibrium constant is defined as the ratio of the concentration of products and the concentration of the reactants.

To determine: The value of the equilibrium constant (K) for the titration reaction.

(c)

Interpretation Introduction

Interpretation: The Ecell before the titration was carried out is to be calculated. The value of the equilibrium constant (K) for the titration reaction and the value of Ecell at the halfway point in the titration are to be calculated.

Concept introduction: Electrochemical cell is a combination of two half cells in which the two electrodes are joined by a wire and a salt bridge. Electrons flow from anode where oxidation occurs to cathode where reduction takes place. Cell potential is defined as the measure of energy per unit charge available from the redox reaction to carry out the reaction. Equilibrium constant is defined as the ratio of the concentration of products and the concentration of the reactants.

To determine: The value of Ecell at the halfway point in the titration.

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Chapter 17 Solutions

Chemistry: An Atoms First Approach
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