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 $H^$ = $1.7\times 10^{-9}M$

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.

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

$pH=-\log (1.7\times 10^{-9})=8.76$

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