[Maybe]

10mL of a solution of a weak acid ( HA, Ka=4.66*10^-6) was titrated with .1500 M NaOH; the equivalence point occured at 4.67 mL of NaOH.
Calculate the pH at 0.00 mL of added HCl and at 2.00 mL of added HCL

I hope someone can help me walk through this problem. I am used to the textbook problems that have the molarity of the acid.
 
Thanks in advance.

[Borek]

Calculate the pH at 0.00 mL of added HCl and at 2.00 mL of added HCL

Strange, you were titrating with NaOH< not adding HCl.

I hope someone can help me walk through this problem. I am used to the textbook problems that have the molarity of the acid.

http://www.titrations.info/titration-curve-calculation

http://www.titrations.info/acid-base-titration-curve-calculation

[Maybe]

I apologize I forgot to change the question.
However, I found out the molarity by using the equivalence point. And I was then able to calculate the pH at different additions of NaOH.