Question

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

Answer 1

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!

Answer 2

The pH of the nitric acid solution is 3.70.

Step-by-step explanation:

The pH is negative logarithm of hydrogen ion concentration.

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

Concentration of nitric acid =
`2* 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* 10^(-4) M` of nitric acid will give .

`[H^+]=1* 2* 10^(-4) M=2* 10^(-4) M`

The pH of the solution :

`pH=-\log[2* 10^(-4) M]=3.70`