Consider a buffer solution made from a partially neutralizing 1.00 M hydrochlorious acid (HClO, Ka=3.5*10^-8) with 0.500M sodium hydroxide.
A) Calculate the amount of base needed to make a buffer from 50.0mL of HClO with a pH equal to the pKa of the acid.
B) What is the pH of a buffer solution made in (a) after diluting to 500mL.
C) Which solution made in (a) or (b) will have a lower capacity if equal volumes of each are compared? Why ?
D) Calculate the pH of a buffer made using 30.0mL of the acid and 10.0mL of the base.
E) Calculate the pH of a buffer using 20.0ml of acid and 30.0mL of base.
F) Which solution made in (d) or (e) can buffer more acid ? Which can buffer more base? Why?