Ka for methanoic acid is 1.78 × 10−4 mol dm−3 at 25°C.
buffer is prepared containing 2.35 × 10−2 mol of methanoic acid and 1.84 × 10−2 mol of sodium methanoate in 1.00 dm3 of solution.
(i) Calculate the pH of this buffer solution at 25°C.
I did this correct and worked it out as 3.64
however the next part I don't understand how to approach...
A 5.00 cm3 sample of 0.100 mol dm−3 hydrochloric acid is added to the buffer solution in part (c)(i).
Calculate the pH of the buffer solution after this addition.
I did the moles of H+ added as 5x10-4 but that's all I've got so far