Calcular el poh y el ph de una solucion 0.00016M de KOH

The pOH of the solution is 3.796 while the pH is 10.2

Explanation:

We are required to calculate the pOH and pH of a 0.00016M solution of KOH.

The first step is to calculate the pOH of the solution. Remember that pOH is defined as the negative logarithm of the hydroxide ion concentration.

Thus;

pOH= -log[OH^-]

pOH= -log [0.00016]

pOH= 3.796

We also know that pH+pOH= 14

Therefore, pH= 14-pOH

Thus;

pH= 14-3.796

pH= 10.2

Hence the pOH of the solution is 3.796 while the pH is 10.2

your answer would be “dry”

12 is it do you think so