# Ionic Equilibrium

Calculate the pH of a solution which contains 100mL of 0.1M $\ce{HCl}$ and 9.9mL of 1.0M $\ce{NaOH}$.

While calculating the concentration of $\ce{H+}$ ions, why shouldn't we consider the H+ ion concentration from water?

• Check the Homework Policy for specific information regarding asking homework, or homework-type questions. Please try to narrow your question to a specific concept and show your reasoning thus far. – Jason Patterson Sep 29 '14 at 13:12

You can consider the hydrogen ion concentration from the ionization of water. However, that quantity is a million fold less than the amount of hydrogen ion coming from $\ce{HCl}$ and can be considered insignificant.