A chemist titrates 17.44 mL of 0.346 M NaOH into a flask containing 50.13 mL of 0.179 M HCl. When the titration is complete, the pH of the solution in the reaction flask is?

Question

A chemist titrates 17.44 mL of 0.346 M NaOH into a flask containing 50.13 mL of 0.179 M HCl. When the titration is complete, the pH of the solution in the reaction flask is?

12.64
.0919
1.36
2.22
11.78

Answer 1

moles HCl = M x L = ?

moles NaOH = M x L = ?
Write the equation. Which is there in excess. Subtract moles of the greater from moles of the lesser. The pH of the solution will be determined by the excess HCl or excess NaOH (depending upon the numbers). Then pH = -log(H^+) OR pOH = -log(OH^-)