Question

A solution is prepared by mixing equal volumes of 0.16 M HCl and 0.52 M HNO3. (Assume that volumes are additive.)

Express the pH to two decimal places.

Answer 1

The pH of the final solution is 0.16 .

Step-by-step explanation:

The pH of the solution is defined as negative logarithm of hydrogen ion concentration in a solution.

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

Concentration of HCl = 0.16 M

`HCl(aq)\rightarrow H^+(aq)+Cl^-(aq)`

HCl is a string acid .1 molar of HCl gives 1 molar of of hydrogen ions.

`[H^+]=0.16 M`

Concentration of
`HNO_3` = 0.52 M

`HNO_3(aq)\rightarrow H^+(aq)+NO_(3)^-(aq)`

Nitric is a string acid .1 molar of nitric acid gives 1 molar of of hydrogen ions.

`[H^+]'=0.52 M`

Total hydrogen ion concentration:

`[H^+]''=[H^+]+[H^+]'`

=0.16 M+0.52 M=0.68 M

The pH of the solution:

`\pH=-\log[H^+]''=-\log[0.68 M]`

pH = 0.16

The pH of the final solution is 0.16 .