The electrochemical cell shown can be used to calculate the formation constant (Kf) for a metal (M) and EDTA. The cell has apotential of -0.265 V. The right half-cell contains a metal ion (M2+) with a standard reduction potential of -0.236 V.M2+ + 2 e- = M(s)E° = -0.236 VVoltmeter(g) PH2=0.40 barSalt bridgePt30 mL of 0.010 M citric acid70 mL of 0.010 M NaOH30 mL of 0.010 M M2+70 mL of 0.010 M EDTA (ay4-=0.81 at pH 11)pH 11.0 (buffered)Citric acid has three pKa values: 3.128, 4.761, and 6.396. Calculate the Kf for the metal-EDTA complex.

Given: Cell potential (Ecell) = -0.265V PH2 = 0.40 bar pka values of citric acid = 3.128, 4.761 and…

The electrochemical cell shown can be used to calculate the formation constant (Kf) for a metal (M) and EDTA. The cell has a potential of -0.265 V. The right half-cell contains a metal ion (M2+) with a standard reduction potential of –0.236 V. M2+ +2 e¯ = M(s) E° = -0.236 V V Voltmeter + H, (g) PH2=0.40 bar Salt bridge Pt

The electrochemical cell shown can be used to calculate the formation constant (Kf) for a metal (M) and EDTA. The cell has a potential of -0.265 V. The right half-cell contains a metal ion (M2+) with a standard reduction potential of –0.236 V. M2+ +2 e¯ = M(s) E° = -0.236 V V Voltmeter + H, (g) PH2=0.40 bar Salt bridge Pt

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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