Question

What is the pH of a 2.0 x 10^-4 M solution of nitric acid (HNO3)

Answer 1

Answer:

The pH of the nitric acid solution is 3.70.

Explanation:

The pH is negative logarithm of hydrogen ion concentration.

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

Concentration of nitric acid = $2\times 10^{-4} M$

$HNO_3(aq)\rightarrow H^+(aq)+NO_{3}^{-}(aq)$

1 mole of nitric acid gives 1 mole of hydrogen ions.

Then$2\times 10^{-4} M$ of nitric acid will give .

$[H^+]=1\times 2\times 10^{-4} M=2\times 10^{-4} M$

The pH of the solution :

$pH=-\log[2\times 10^{-4} M]=3.70$

Answer 2

Hello!

datos:

Molarity = $2.0*10^{-4}\:M\:(mol/L)$

ps: The ionization constant of the nitric acid is strong (100% ionized in water) or completely dissociates in water, so the pH will be:

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

$pH = - log\:[2*10^{-4}]$

$pH = 4 - log\:2$

$pH = 4 - 0.30$

$\boxed{\boxed{pH = 3.70}}\end{array}}\qquad\checkmark$

Note:. The pH <7, then we have an acidic solution.

I Hope this helps, greetings ... DexteR!