A solution is prepared by mixing 88.0 mL of 5.00 M HCl and 26.0 mL of 8.00 M HNO3. Water is then added until the final volume is 1.00 L. How would you calculate [H+], [OH -], and the pH for this solution? please explain?
This is a typical acid/base equilibrium problem, that involves the use of logarithms.
We assume that both nitric acid and hydrochloric acid dissociate to give stoichiometric
Moles of nitric acid:
And, moles of hydrochloric acid:
This molar quantity is diluted to
Now we know that water undergoes autoprotolysis:
Alternatively, we know further that