Nickel is immersed in 0.1M NaCl at pH = 1 and H2 pressure of 1 atm.  Calculate the potential of the cathodic 1/2 reaction.

For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?

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.