Consider the titration of 60.0 mL of 0.10 M HBr with 0.15 M KOH. Calculate the pH after 40.0 mL...

Question:

Titration and pH of a Solution:

Strong base releases hydroxide ions and strong acid releases protons. Hydroxide ions and protons react to form a molecule of water. If an equal number of moles of an acid and base react, the final solution will be a neutral solution. The following formulas are generally utilized to find the pH value of a solution.

{eq}\begin{align} ~\text{ Molar concentration of a solution} &=\dfrac{~\text{ Number of moles of solute present in a solution} ~}{~\text{Volume of the solution} } \\[0.3cm] \hspace{1cm} p\rm{H} &= -\log_{10}{[ \rm H^+]} \\[0.3cm] \hspace{1cm} p\rm{OH} &= -\log_{10}{[ \rm OH^-]} \\[0.3cm] \hspace{1cm} p\rm{H} + p\rm{OH}&= 14\\[0.3cm] \end{align} {/eq}.

Answer and Explanation: 1