Question

A voltaic cell contains two half-cells. One half-cell contains a nickel electrode immersed in a 1.00 M Ni(NO₃)₂ solution. The second half-cell contains a titanium electrode immersed in a 1.00 MTi(NO₃)₃ solution.

Ni2+(aq) + 2 e− → Ni(s)	E⁰red  = −0.257 V
Ti3+(aq) + 3 e− → Ti(s)	E⁰red = −1.370 V

(a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell.
____V

(b) Write the overall balanced equation for the voltaic cell. (Include states-of-matter under the given conditions in your answer.)

Answer 1

a) Given that:

Ni²⁺(aq) + 2e^- → Ni(s); E^o_red = -0.257 V    

Ti³⁺(aq) + 3e^- → Ti(s); E^o_red = -1.370 V    

Reduction half reaction is: Ni²⁺(aq) + 2e^- → Ni(s); E^o_red = -0.257 V    

Oxidation half reaction is: Ti(s) → Ti³⁺(aq) + 3e^- ; E^o_ox = - E^o_red = -( -1.370 V)    

Standard cell potential for voltaic cell is given by:

E^o_cell = E^o_red + E^o_ox

E^o_cell = (-0.257 V) + (1.370 V) = 1.113 V

b) Overall balanced equation for the voltaic cell: Ni²⁺(aq) +Ti(s) → Ni(s) + Ti³⁺(aq)