Question

question 2- all 4 parts. please type orwritr clearly thank you!

2. Buffer capacity refers to the amount of acid or base a buffer can "absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can "absorb" five times as much acid or base as a 0.1 M buffer for a given pH change. In this problem you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity of acid or base is added. You are given 60 mL of 0.50 M phosphate buffer, pH = 6.83, to test. The starting composition of the buffer, both in terms of the concentration and the molar quantity of the two major phosphate species is: Concentration of HPO,0.304 M Concentration of H,PO,0.196 M Molar quantity of HPO: 18.2 mmol Molar quantity of H,PO,: 11.8 mmol a. You add 1.7 mL of 1.00 M HCl to the buffer. Calculate the molar quantity of H,O added as HCI, and the final molar quantity of HPO, and HAPO, at equilibrium? b. What is the new HPO,/H,PO, ratio, and the new pH of the solution? The pK, of H,PO, is 6.64. Use the Henderson-Hasselbach equation to calculate the new pH. (Note: You can use the molar ratio rather than the concentration ratio because both species are in the same volume.) c. Now take a fresh 60 mL of the 0.50 M pH 6.83 buffer and add 3.7 mL of 1.00 M NaOH. Using steps similar to those above, calculate the new pH of the solution.