Electrochemistry

Step 1: Write the reaction and information given
The reaction is: H+(aq)+e−⟶‌

1

2

H2(1bar) The pH of the solution is 10.0 .
Step 2: Find the concentration of H+
We know that pH=−log[H+]
This means [H+]=10−pH=10−10M
Step 3: Note important values
Standard electrode potential for the hydrogen electrode is E∘=0V and the number of electrons (n) is 1.
Step 4: Write and use the Nernst Equation
The Nernst equation is: E=E∘−‌

0.0591

n

‌log[H+]Now plug in the values:
E=0−‌

0.0591

1

‌log(10−10)
Step 5: Calculate the answer
‌log(10−10)=−10,‌ so ‌E=0−(0.0591×−10)
‌E=0+0.591V
Step 6: Final value and sign
The calculated value is E=0.591V. However, since the concentration is smaller than the standard value, the potential is actually negative. So, E=−0.591V or approximately -0.6 V .