Question

What is the [H+] in a solution with pOH of 0.253?

Answer 1

Answer: pOH of the solution is 13.41.

Explanation:-

pH is the measure of acidity or alkalinity. It is also defined as negative logarithm of hydrogen ion concentration.

$pH=-log[H^+]$

$pOH=-log[OH^-]$

$pH+pOH=14$

Given: $[H^+]$ = 0.253

Thus $pH=-log[0.253]$

$pH=0.59$

$0.59+pOH=14$

$pOH=14-0.59=13.41$

Answer 2

PH + pOH = 14

pH + 0.253 = 14

pH = 14 - 0.253

pH = 13.747

[ H+] = 10 ^ -pH

[ H+ ] = 10 ^- 13.747

[ H+ ] = 1.790x10⁻¹⁴ M

hope this helps!