The pOH of a solution of 0.15 M HCl (aq) would be what?

13.18

Explanation:

We'll begin by calculating the hydrogen ion concentration, [H⁺] in the solution. This can be obtained as follow:

HCl (aq) —> H⁺(aq) + Cl¯(aq)

From the balanced equation above,

1 mole of HCl dissociate to produce 1 mole of H⁺.

Therefore, 0.15 M HCl will also dissociate to produce 0.15 M H⁺.

Thus, the concentration of the hydrogen ion, [H⁺] in the solution is 0.15 M.

Next, we shall determine the pH of the solution. This can be obtained as follow:

Concentration of the hydrogen ion, [H⁺] = 0.15 M.

pH =?

pH = – Log[H⁺]

pH = – Log 0.15

pH = 0.82

Finally, we shall determine the pOH of the solution. This can be obtained as follow:

pH = 0.82

pOH =?

pH + pOH = 14

0.82 + pOH = 14

Collect like terms

pOH = 14 – 0.82

pOH = 13.18

Therefore, the pOH of the solution is 13.18

6.4 cm (max) - 25 cm (min)