Question

Calculate the p o h of a solution at 25 c that contains 1 10 10 m of hydronium ions, i.E., h 3 o + ;

Answer 1

Answer:

pOH=−log10[−OH]=5.60

Explanation:

We know or should know that under standard conditions (the which operate here): pH+pOH=14.

pH=−log10[H3O+] = −log10[3.98×10−9]=8.40.

And thus pOH=14−8.60=5.60

Answer 2

Answer:

The pOH of the solution is 4.

Explanation:

The pH of the solution is define as negative logarithm of $H_3O^+$ concentration in a solution.

$pH=-\log[H_3O^+]$

$pH=-\log[1\times 10^{-10} M]=10$

$pH+pOH=14$

$pOH = 14-pOH = 14 -10 = 4$

The pOH of the solution is 4.