Given:
Current (I) = 10.0 A
Time (t) = 965 seconds
Volume (V) = 1.0 L
Concentration (C) = 1.0 M

To Find:
pH of the solution at the end of the experiment

Explanation:
To find the pH of the solution, we need to calculate the concentration of H+ ions in the solution. We can use Faraday's law of electrolysis to determine the number of moles of H+ ions produced during the electrolysis.

Step 1: Calculate the charge (Q) passed through the solution:
Using the formula Q = I × t, where
Q = charge passed (Coulombs)
I = current (Amperes)
t = time (seconds)

Substituting the given values:
Q = 10.0 A × 965 s = 9650 C

Step 2: Calculate the number of moles of H+ ions produced:
Using Faraday's law of electrolysis, the number of moles of H+ ions (n) produced is given by the formula:
n = Q / F, where
n = number of moles
Q = charge passed (Coulombs)
F = Faraday's constant = 96500 C/mol

Substituting the given values:
n = 9650 C / 96500 C/mol = 0.1 mol

Step 3: Calculate the new concentration of H+ ions:
The initial concentration of H+ ions (C1) is 1.0 M. Since the volume remains constant, the final concentration (C2) can be calculated using the formula:
C2 = (n / V) + C1, where
C2 = final concentration (M)
n = number of moles
V = volume (L)
C1 = initial concentration (M)

Substituting the given values:
C2 = (0.1 mol / 1.0 L) + 1.0 M = 0.1 M + 1.0 M = 1.1 M

Step 4: Calculate the pH of the solution:
pH is a measure of the concentration of H+ ions in a solution and is given by the formula:
pH = -log[H+], where
[H+] = concentration of H+ ions (M)

Substituting the calculated final concentration:
pH = -log(1.1) ≈ -0.041

Conclusion:
The pH of the solution at the end of the experiment is approximately -0.041. Since pH must be a positive value, the closest option is (c) 0.8.