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The electrochemical cell shown can be used to calculate the formation constant (K) for a metal (M) and EDTA. The cell has a potential of -0.257 V. The right half-cell contains a metal ion (M²) with a standard reduction potential of -0.236 V.

The electrochemical cell shown can be used to calculate the formation constant (K) for a metal (M) and EDTA. The cell has a potential of -0.257 V. The right half-cell contains a metal ion (M²) with a standard reduction potential of -0.236 V.

Chemistry
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
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The electrochemical cell shown can be used to calculate the formation constant (K) for a metal (M) and EDTA. The cell has a potential of -0.257 V. The right half-cell contains a metal ion (M²) with a standard reduction potential of -0.236 V. M²+ + 2e M(s) E = -0.236 V (g) PHz 0.40 bar Pt K₁ = 30 mL of 0.010 M citric acid 70 mL of 0.010 M NaOH Salt bridge Voltmeter + 30 mL of 0.010 MM² 70 mL of 0.010 M EDTA (av4.0.81 at pH 11) pH 11.0 (buffered) Citric acid has three pK, values: 3.128, 4.761, and 6.396. Calculate the K, for the metal-EDTA complex.
Transcribed Image Text:The electrochemical cell shown can be used to calculate the formation constant (K) for a metal (M) and EDTA. The cell has a potential of -0.257 V. The right half-cell contains a metal ion (M²) with a standard reduction potential of -0.236 V. M²+ + 2e M(s) E = -0.236 V (g) PHz 0.40 bar Pt K₁ = 30 mL of 0.010 M citric acid 70 mL of 0.010 M NaOH Salt bridge Voltmeter + 30 mL of 0.010 MM² 70 mL of 0.010 M EDTA (av4.0.81 at pH 11) pH 11.0 (buffered) Citric acid has three pK, values: 3.128, 4.761, and 6.396. Calculate the K, for the metal-EDTA complex.
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