Question

The pH of an aqueous solution is 4.32. What is the [OH–]?

Answer 1

Answer;

C. 2.1 x 10–10 M

Explanation;

pKw=pH + pOH = 14  

pOH = 14-4.32

        =9.68  

But; pOH = -log[OH]

[OH-]=10^(-9.68)

         =2.089x10^-10M

         ≈ 2.1 x 10–10 M

Answer 2

Answer: The concentration of hydroxide ion concentration is $2.08\times 10^{-10}$

Explanation:

pH is defined as negative logarithm of hydrogen ion concentration. It is basically defined as the power of hydrogen ions in a solution.

To calculate the hydroxide ion concentration of the solution, we need to determine the pOH of the solution first and to do so, we calculate the pOH by the following equation:

$pH+pOH=14\\pOH=14-4.32=9.68$

pOH is defined as negative logarithm of hydroxide ion concentration. It is basically defined as the power of hydroxide ions in a solution.

The equation used to calculate pOH of the solution is given as:

$pOH=-\log[OH^-]$

pOH of the solution = 9.68

Putting values in above equation, we get:

$9.4=-\log[OH^-]$

$[OH^-]=antilog(-9.68)$

$[OH^-]=2.08\times 10^{-10}$

Hence, the concentration of hydroxide ion concentration is $2.08\times 10^{-10}$