Question

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

Answer 1

Answer:

The pH of the final solution is 0.16 .

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 .