Two buffers are prepared by adding an equal number of moles of formic acid (HCOOH) and sodium formate (HCOONa) to enough water to make 1.00 L of solution. Buffer A is prepared using 1.00 mol each of formic acid and sodium formate. Buffer B is prepared by using 0.010 mol of each. 

(a) Calculate the pH of each buffer, and explain why they are equal.

(b) Which buffer will have the greater buffer capacity? Explain.

(c) Calculate the change in pH for each buffer upon the addition of 1.0 mL of 1.00 M HCl.

(d) Calculate the change in pH for each buffer upon the addition of 10 mL of 1.00 M HCl.

(e) Discuss your answers for parts (c) and (d) in light of your response to part (b).