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

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LeChatNoir LeChatNoir · Answer 1 · 2017-06-08T20:20:00+02:00

[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

:)

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BarrettArcher BarrettArcher · Answer 2 · 2019-04-09T08:45:29+02:00

Answer : The pOH of the solution is, 5.24

Solution : Given,

Concentration of [tex]H^[/tex] = [tex]1.7\times 10^{-9}M[/tex]

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.

[tex]pH=-\log [H^+][/tex]

[tex]pH=-\log (1.7\times 10^{-9})=8.76[/tex]

Now we have to calculate the pOH.

[tex]pH+pOH=14[/tex]

[tex]8.76+pOH=14[/tex]

[tex]pOH=5.24[/tex]

Therefore, the pOH of the solution is, 5.24