The standard addition method is used to determine the concentration of vitamin C in apple juice by polarography, a method that produces a current that is proportional to concentration. A 2.00 mL sample of apple juice is diluted to a total volume of 25.0 mL, which gives a current reading of 1.01 µA. This solution is then spiked with a 5.00 mL aliquot of a 262 mg/L solution of vitamin C, producing a reading of 2.27 HA. What is the concentration of vitamin C in the apple juice? Concentration of vitamin C (mg/L):

The standard addition method is used to determine the concentration of vitamin C in apple juice by polarography, a method that produces a current that is proportional to concentration. A 2.00 mL sample of apple juice is diluted to a total volume of 25.0 mL, which gives a current reading of 1.01 µA. This solution is then spiked with a 5.00 mL aliquot of a 262 mg/L solution of vitamin C, producing a reading of 2.27 HA. What is the concentration of vitamin C in the apple juice? Concentration of vitamin C (mg/L):

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

Chapter18: Electrochemistry

Section: Chapter Questions

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

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An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
A current is passed through a solution of copper(II) sulfate long enough to deposit 14.5 g of copper. What volume of oxygen is also produced if the gas is measured at 24 °C and 0.958 atm of pressure?
Calculate the electrode potentials for the following systems: (a) Cr2O72-(5.00 10-3 M),Cr3+(2.50 10-2 M),H+ (0.100 M)|Pt (b) UO22+(0.100 M),U4+ (0.200 M),H+ (0.600 M)|Pt
Answer the following questions by referring to standard electrode potentials at 25C. a Will oxygen, O2, oxidize iron(II) ion in solution under standard conditions? b Will copper metal reduce 1.0 M Ni2(aq) to metallic nickel?
Electrolysis of a solution of CuSO4(aq) to give copper metal is carried out using a current of 0.66 A. How long should electrolysis continue to produce 0.50 g of copper?
A galvanic cell is based on the following half-reactions: 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 H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)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, 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.
An electrochemical cell is made by placing a zinc electrode in 1.00 L of 0.200 M ZnSO4 solution and a copper electrode in 1.00 L of 0.0100 M CuCl2 solution. a What is the initial voltage of this cell when it is properly constructed? b Calculate the final concentration of Cu2+ in this cell if it is allowed to produce an average current of 1.0 amp for 225 s.

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