Question

What is the pH of a solution of KOH with a hydroxide concentration of [OH⁻] = 1.10 x 10⁻⁴

Answer 1

`p[H+] = 10.042`

Step-by-step explanation:

As we know that

`pKw = pH + pOH`......eq (1)

we will calculate the pH of OH- and then we will calculate the pH of H+

So p[OH-]
`= - log [1.10 * 10^(-4)]`

Solving the right side of the equation, we get

p[OH-]

`= - [-3.958]\\= 3.958`

Now we know that

`pKw = 14.0`

Substituting the value of pOH in the above equation, we get -

`14.0 = p[H+] + 3.958\\p[H+] = 14 - 3.958\\p[H+] = 10.042`