Question

the pH of a solution is 3.602.its H+ ion concentration isfrom Ionic equilibrium ​

Answer 1

pH = 3.602

pH = -log[H+]

:. [H+] = antilog(-pH

= antilog(-3.602)

= antilog(—4.398)

[H+] = 2.5 × 10-⁴ M

Answer 2

Answer : The $H^-$ concentration is, $2.5\times 10^{-4}M$

Explanation :

pH : It is defined as the negative logarithm of hydrogen ion concentration.

Formula used :

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

Now we have to calculate the $H^+$ concentration.

Given : pH = 3.602

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

$3.602=-\log [H^+]$

$[H^+]=2.5\times 10^{-4}M$

Therefore, the $H^-$ concentration is, $2.5\times 10^{-4}M$