pH of 0.01 M KOH solution at 25°C will be

To find the pH of a 0.01 M KOH solution at 25°C, we first need to understand that KOH is a strong base, which means it will dissociate completely in water to form K+ and OH- ions.

The concentration of OH- ions will therefore be equal to the concentration of the KOH solution, which is 0.01 M.

We can then use the formula for pOH, which is -log[OH-]. Substituting the given concentration into this formula gives us:

pOH = -log[0.01] = 2

Since pH and pOH are related by the equation pH + pOH = 14 at 25°C, we can find the pH by subtracting the pOH from 14:

pH = 14 - pOH = 14 - 2 = 12

So, the pH of the 0.01 M KOH solution at 25°C is 12.