I have a 10.00mL solution of 0.2000M CH3COONa is titrated with 0.1000M HCl to the equivalence point.

Write out the equation, calculate the volume HCl required and calculate the pH of the solution at its equivalence point.

Ok, I'm still learning this whole titration thing so bear with me guys, and let me know if I'm doing this right.

I'm not too sure about my Equation...

CH3COONa + H20 + HCl <-> H30+ + CH3COO- + NaCl

but what do i do with my NaCl? do i simply disregard it like I would with the water in my ICE table?

so i used M1V1=M2V2

so, (0.2M)(0.01L)=(0.1M)V2

V2 = 0.02L HCl

and to get my pH, I need my concentration of H+, so I can use pH=-log[H+], however I don't know my Ka value, nor do I know how much [H+] I have because I'm not sure about my equation so I cannot form my ice table either. I'm stuck.

Hopefully there's someone out there who understands titration equations.