A voltaic cell is set up with copper and hydrogen half-cells. Standard conditions are used in the copper half-cell, Cu2+ (aq, 1.00 M) | Cu (s). The hydrogen gas pressure is 1.00 bar. A value of 0.490 V is recorded for E Cell at 298 K. Determine the concentration of H+ and the pH of the solution.

the concentration of H+ = 3 ×     M and the pH = 2.6 of the solution

Explanation:

Based on reduction potentials, hydrogen is a better reducing agent than copper, therefore copper() is the cathode and hydrogen () is the anode.

Cathode reaction (reduction):  ⇒   Cu(s)

Anode reaction (oxidation) :       ⇒    

net reaction:         ⇒  

E cathode = 0.337 v

Q(reaction quotient) =

for 2 electrons but is unknown. we solve this using hernst equation.

pH = 2.6

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explanation:

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