A 40.00 ml aliquot of 0.0500 M HNO2 is diluted to 80.0 ml in water and titrated with 0.0800 M Ce4+ to form NO3- and Ce3+. Assume the hydrogen ion concentration is at 1.00 M throughout the titrtion. Use 1.44 Volts as the standard potential for the Ce4+/Ce3+ system and 0.94 Volts for the NO3-/NO2 system.Write and balance the two half-cell reactionsCalculate the potential of the indicator electrode with respect to an Ag/AgCl saturated reference electrode after the titration of the HNO2 solution with 5.00, 50.00, 60.00 and 100.00 ml of Ce4+.

A 40.00 mL aliquot of 0.0500 M HNO2 is diluted to 80.00 mL in water and was titrated with 0.0800 M…

Answered: A 40.00 ml aliquot of 0.0500 M HNO2 is…

Chemistry

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

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A 40.00 ml aliquot of 0.0500 M HNO2 is diluted to 80.0 ml in water and titrated with 0.0800 M Ce⁴⁺ to form NO₃^- and Ce³⁺. Assume the hydrogen ion concentration is at 1.00 M throughout the titrtion. Use 1.44 Volts as the standard potential for the Ce⁴⁺/Ce³⁺ system and 0.94 Volts for the NO₃^-/NO₂ system.

Write and balance the two half-cell reactions
Calculate the potential of the indicator electrode with respect to an Ag/AgCl saturated reference electrode after the titration of the HNO₂ solution with 5.00, 50.00, 60.00 and 100.00 ml of Ce⁴⁺.

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