Consider an Electrochemical Cell with a Zinc Electrode Immersed in a Solution

Consider an electrochemical cell with a zinc electrode immersed in a solution of Zn²⁺ and a silver electrode immersed in a solution of Ag⁺. Zn²⁺ + 2e^- $\to$ Zn
$\varepsilon$ ° = -0.76 V
Ag⁺ + e^- $\to$ Ag
$\varepsilon$ ° = 0.80 V
If is 0.050 M and is 11.26 M,calculate $\varepsilon$ .

A) 1.46 V
B) 1.76 V
C) 1.36 V
D) 1.66 V
E) 1.63 V