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* 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* 10^(-5)M`

Therefore, the
`OH^-` concentration is,
`6.0* 10^(-5)M`