Can someone show me how to figure this tough chem problem out?

Calculate the pH of a solution which is made by adding 2.50 g of sodium acetate to 200.0 mL of .150 M acetic acid. Assume that the added sodium acetate does not change the volume of the solution. The pKa of acetic acid is 4.76.Can someone show me how to figure this tough chem problem out?
calculate the number of moles by dividing the 2.50g by the molar mass of sodium acetate


2.5g/82.03 g/mol=.030moles


calculate the number of moles of the acetic acid by multiplying .15M*.2L=.0300moles


use the following equation


pH=Pka+log(#moles of sodium acetate/#moles acetic acid)


pH=4.76+log(.030/.0300)


pH=4.76Can someone show me how to figure this tough chem problem out?
DYOHW!!





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