Potentiometry was employed to investigate the formation of complexes between EDTA and Cu²+ ions in aqueous solution. To do so, the potential of a Cu electrode was measured in a series of solutions containing 1 mM Cu(NO3)2, 100 mM KNO3, and varying concentrations of EDTA (added as the tetrasodium salt). Using the data provided below, calculate the formation constant (K) of the Cu²+-EDTA complex.

Potentiometry was employed to investigate the formation of complexes between EDTA and Cu²+ ions in aqueous solution. To do so, the potential of a Cu electrode was measured in a series of solutions containing 1 mM Cu(NO3)2, 100 mM KNO3, and varying concentrations of EDTA (added as the tetrasodium salt). Using the data provided below, calculate the formation constant (K) of the Cu²+-EDTA complex.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 103QAP: An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from...

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An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
At what pH does Ecell = 0.00 V for the reduction of dichromate by iodide ion in acid solution, assuming standard-state concentrations of all species except H+ ion?
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 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)?
How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
The electrochemistry of metal complexes reflects the underlying chemical equilibria involved in their formation. A chemist can use the measured electrochemistry to determine the solubility product of a metal-ion complex, or vice versa. Calculate the electrode potential of the following half-cell involving the reduction of the Cu(I)-thiocyanate complex to copper metal, Cu(0). CuSCN (sat’d), SCN– (0.0300M) | Cu The solubility product, KSP, of CuSCN is 1.77 x 10-11 = [Cu+][SCN–]
To study the effects of a weakly acidic medium on the rate of corrosion of a metal alloy, a student prepared a buffer solution containing both 0.123 M NaC2H3O2 and 0.087 M HC₂H3O2. Calculate the pH of the buffer using the K₁ for C₂H3O₂. Be sure to write the chemical equation for the equilibrium as the reaction of C₂H3O₂ with water. Then use the chemical equation as a guide in setting up the equilibrium expression for Kb. For acetic acid, HC₂H3O2, K₂ = 1.8 x 10-5. pH =
A solution prepared by mixing 60.0 mL of 0.360 M AGNO, and 60.0 mL of 0.360 M TINO, was titrated with 0.720 M NaBr in a cell containing a silver indicator electrode and a reference electrode with a constant potential of 0.175 V. The reference electrode is attached to the positive terminal of the potentiometer, and the silver electrode is attached to the negative terminal. The solubility constant of TIBr is Kp = 3.6 × 10-6 and the solubility constant of AgBr is = 5.0 x 10-13. Ksp Which precipitate forms first? O TIBI O AgBr Which of the expressions shows how the cell potential, E, depends on [Ag*]? E = 0.175 V – [0.799 V – 0.05916log ([Ag+])] 1 E = |0.799 V – 0.05916log - 0.175 V [Ag*) E = [0.799 V – 0.05916log ([Ag*]D] – 0.175 V E = 0.175 V - |0.799 V – 0.05916log [Ag* * (ল) Calculate the first and second equivalence points of the titration. first equivalence point: mL second equivalence point: mL What is the cell potential after each of the given volumes of 0.720 M NaBr have been…
ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous solution containing M2X2 (where X is the anion) with a supplied current of 6.82 A for 10 h, consuming 0.179 kWh of electrical energy. Assume that the current efficiency is 91%.