A voltaic cell is constructed such that the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2)= 1atm) immersed...

A voltaic cell uses chemical reactions to produce electricity. This electricity is generated due to the reactions taking place at the anode and the cathode and such reactions are known as half-cell reactions. 

Nernst equation is commonly used to solve questions related to these cells. The equation is commonly written as:

`E = E^0 + (RT)/(nF) log_10 ([H^+]^2/p_H_2)`

When the hydrogen electrodes serve as both the cathode and the anode and the reaction is taking place at 298 K (or 25 degrees C) and the partial pressure of hydrogen is 1 atm, this equation reduces to:

`E = E^0 -0.059/2 log_10([H^+]^2)`

Using the given cell potential value of 0.212 V, we get

0.212 = -0.059/2 log([H^+]^2)

solving the equation, we get, [H^+] = 2.55 x 10^-4 M

since, pH = -log [H^+] = 3.59

Thus, the anode is dipped in a solution of pH = 3.59.

Hope this helps.