A chemistry graduate student is given 500. mL of a 0.40 M benzoic acid HC 6 H 5 CO 2 solution. Benzoic acid is a weak acid with = K a × 6.3 10 ? 5 . What mass of NaC 6 H 5 CO 2 should the student dissolve in the HC 6 H 5 CO 2 solution to turn it into a buffer with pH = 4.45 ? You may assume that the volume of the solution doesn\'t change when the NaC 6 H 5 CO 2 is dissolved in it. Solution According to Henderson-Hasselbalch equation pH = pKa + log { (salt) /( acid)} pH = pKa + log (C6H5COONa/C6H5COOH) pKa = -log(Ka) pKa = - log ( 6.3×10^-5) pKa = 4.20 Number of moles of C6H5COOH: 500 mL × ( 1L /1000 mL ) × ( 0.40 mol / L) = 0.20 mol Substitute all the values in above equation. 4.45 = 4.20 + log (C6H5COONa / 0.20 mol) 0.25 = log ( C6H5COONa / 0.20 mol) C6H5COONa = 1.7783 × 0.2 mol C6H5COONa = 0.35565 mol Mass of C6H5COONa = 0.35565 mol × ( 144.11 g / 1 mol) = 51.25 g .