Question

What is the [OH–] in a solution with a pOH of 4.22? 1.7 x 10–10 M 6.0 x 10–5 M 6.3 x 10–1 M 1.7 x 104 M

Answer 1

POH=4.22

pOH = -lg[OH⁻]

[OH⁻]=10^(-pOH)

[OH⁻]=10⁻⁴·²² = 6.0×10⁻⁵ mol/L

6.0×10⁻⁵ M

Answer 2

Answer : The correct option is, $6.0\times 10^{-5}M$

Explanation :  Given,

pOH = 4.22

pOH : It is defined as the negative logarithm of hydroxide ion concentration.

Now we have to calculate the $OH^-$ concentration.

Formula used :

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

Now put all the given values in this formula, we get the concentration of hydroxide ion.

$4.22=-\log [OH^-]$

$[OH^-]=6.0\times 10^{-5}M$

Therefore, the $OH^-$ concentration is, $6.0\times 10^{-5}M$