Hello!
datos:
Molarity = [tex] 2.0*10^{-4}\:M\:(mol/L) [/tex]
ps: The ionization constant of the nitric acid is strong (100% ionized in water) or completely dissociates in water, so the pH will be:
[tex] pH = - log\:[H_3O^+] [/tex]
[tex] pH = - log\:[2*10^{-4}] [/tex]
[tex] pH = 4 - log\:2 [/tex]
[tex] pH = 4 - 0.30 [/tex]
[tex] \boxed{\boxed{pH = 3.70}}\end{array}}\qquad\checkmark [/tex]
Note:. The pH <7, then we have an acidic solution.
I Hope this helps, greetings ... DexteR!
Answer:
The pH of the nitric acid solution is 3.70.
Explanation:
The pH is negative logarithm of hydrogen ion concentration.
[tex]pH=-\log[H^+][/tex]
Concentration of nitric acid = [tex]2\times 10^{-4} M[/tex]
[tex]HNO_3(aq)\rightarrow H^+(aq)+NO_{3}^{-}(aq)[/tex]
1 mole of nitric acid gives 1 mole of hydrogen ions.
Then[tex]2\times 10^{-4} M[/tex] of nitric acid will give .
[tex][H^+]=1\times 2\times 10^{-4} M=2\times 10^{-4} M[/tex]
The pH of the solution :
[tex]pH=-\log[2\times 10^{-4} M]=3.70[/tex]
