Question

What is the pH of a 2.4x10^-5 M OH- solution?

Answer 1

Answer:-

9.38

Explanation:-

Given [OH-] = 2.4 x 10 ^ -5 M

We use the formula

pOH = - log [OH-]

= - log [ 2.4 x 10 ^ -5]

= 4.62

Now we use the relation

pOH +pH = 14

∴ pH = 14 - 4.62

= 9.38

Answer 2

Answer: The pH of the solution is 9.39

Explanation:

pOH is defined as the negative logarithm of hydroxide ion concentration. The formula used to calculate pOH of the solution is:

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

We are given:

$[OH^-]=2.4\times 10^{-5}M$

Putting values in above equation, we get:

$pOH=-\log(2.4\times 10^{-5})\\\\pH=4.61$

Now, to calculate pH of the solution, we use the equation:

$pH+pOH=14$

pOH = 4.61

Putting values in above equation, we get:

$pH=14-4.61=9.39$

Hence, the pH of the solution is 9.39