Using the Nernst equation, calculate the concentration of Cu^2+ ions given the cell potential is 0.5540 V and the standard cell potential is 0.4260 V. The equation is: 0.5540 V = 0.4260 V - (0.0592/2) log ([Cu^2+]/[1]^2). What is the concentration of Cu^2+?

A concentration cell has the same half-reactions at the anode and cathode, but a voltage results from different concentrations in the two electrode compartments.(b) A similar cell has 0.10 M Cu2+ in both compartments. When a stoichiometric amount of ethylenediamine (NH2CH2CH2NH2) is added to one compartment, the measured cell potential is 0.179 V. Calculate the formation constant Kf for the complex ion Cu(NH2CH2CH2CH2)22+. Assume there is no volume change.

Consider the redox titration of 100.0 mL of a solution of 0.010 M Fe2+ in 1.50 M H2SO4 with a 0.010 M solution of KMnO4, yielding Fe3+ and Mn2+. The titration is carried out in an electrochemical cell equipped with a platinum electrode and a calomel reference electrode consisting of an Hg2Cl2/Hg electrode in contract with a saturated KCl solution having [Cl-] = 2.9M. Using any data in Appendixes C and D, calculate the cell potential after addition of (a) 5.0 mL, (b) 10.0mL, (c) 19.0 mL, and (d) 21.0 mL of the KMnO4 solution.

A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn(s) with E° = -0.763 V. The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-2 M, respectively. What is the cell emf in volts?

At 25°C, E° = +1.88 V for a cell based on the reaction 3 AgCl(s) + Al(s) → 3 Ag(s) + Al³⁺(aq) + 3 Cl⁻(aq). Find the cell potential E if [Al³⁺] = 0.20 M and [Cl⁻] = 0.010 M using the Nernst equation.

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Cu(s) | Cu2+(aq, 3.2×10^(-3) mol L^-1) || Cu2+(aq, 4.48 mol L^-1) | Cu(s). Given E°(Cu2+/Cu) = +0.34 V, express your answer to two significant figures.

Calculate the ΔE°cell for the following concentration cell: Cu(s) | Cu2+(aq, 0.049M) || Cu2+(aq, 0.231M) | Cu(s). Cu2+(aq) + 2e- → Cu(s), E° = 0.340V.