To calculate the pH of the resulting solution, we need to first find out the moles of KCl electrolysed.

Using the formula, Moles = Concentration x Volume, we get:

Moles of KCl = 0.5 x (1/1000) = 0.0005 moles


Next, we need to calculate the charge passed during electrolysis.

Using the formula, Charge = Current x Time, we get:

Charge passed = 16.08 x (1/60) = 0.268 C


During electrolysis, KCl is converted into K+ and Cl-. The water molecules are also electrolysed to form H+ and OH-.

The reactions are:

2H2O → O2 + 4H+ + 4e-
2H2O + 2e- → H2 + 2OH-

We can see that for every 2 electrons that pass through the solution, one molecule of H2O is converted into H+ and OH-.

Therefore, the total number of electrons passed through the solution can be calculated as:

Number of electrons = Charge / (Faraday constant x 1000)

Where Faraday constant = 96485 C/mol

Number of electrons = 0.268 / (96485 x 1000) = 2.77 x 10^-6 mol

Since each electron produces one H+ ion and one OH- ion, the number of moles of H+ and OH- produced can be calculated as:

Moles of H+ and OH- = Number of electrons / 2 = 1.385 x 10^-6 mol


The resulting solution will be basic since the number of moles of OH- is higher than the number of moles of H+.

The concentration of OH- can be calculated as:

[OH-] = Moles of OH- / Volume of solution

Since the volume of the solution is 1 litre, we get:

[OH-] = 1.385 x 10^-6 M

Using the formula, pOH = -log[OH-], we get:

pOH = -log(1.385 x 10^-6) = 5.86

The pH can be calculated as:

pH = 14 - pOH = 8.14

Therefore, the pH of the resulting solution will be 8.14.