Question

When the [H+] in a solution is 1.7 × 10−9 M, what is the pOH ?

Answer 1

[H⁺] = 1,7×10⁻⁹ mol/dm³

pH = -log[H⁺]
pH = -log[1,7×10⁻⁹]
pH = 8,77

pH + pOH = 14
pOH = 14-8,77
pOH = 5,23

:)

Answer 2

Answer : The pOH of the solution is, 5.24

Solution : Given,

Concentration of
`H^` =
`1.7* 10^(-9)M`

As we know that the pH is the negative logarithm of the hydrogen ion concentration.

First we have to calculate the pH of the solution.

`pH=-\log [H^+]`

`pH=-\log (1.7* 10^(-9))=8.76`

Now we have to calculate the pOH.

`pH+pOH=14`

`8.76+pOH=14`

`pOH=5.24`

Therefore, the pOH of the solution is, 5.24