Question

Calculate the pH of a solution formed by mixing equal volumes of two solutions A and B of a strong acid having pH = 6 and pH = 4 respectively.

Answer 1

The pH of a solution can be determined with the concentration of H+, mixing two solutions the pH is not added, rather the moles of H+ is additive, for equal volumes in the given question we need to find the moles of H+ and solution and solution b and add them and then calculate the final PH .

$Concentration [H^+] =\frac{10^{-6}(v)+10^{-4}(v)}{v+v}$

$\frac{10^{-6}+10^{-4} }{2}=[tex]\frac{1.01}{2} \times 10^{-4}$

$pH=-log(\frac{1.01}{2} \times 10^{-4})=4.29$