Refer to Appendix 6 which shows the calculations involved in determining the volumes of 0.20 M acetic acid and 0.20 M sodium acetate needed to make 20.00 mL of a buffer with pH = 5.00. Study the method used: set up two equations with two unknowns; the first is the Henderson-Hasselbalch equation, the second is the fact that the volumes of HA and A− solutions should sum to 20 mL. In the Henderson-Hasselbalch equation, use the same volumes for the ratio, since the concentrations of the HA and A− solutions are the same, and the change in the ratio is due to the different volumes. Once you understand the method, use it to calculate the volumes of 0.20 M acetic acid and 0.20 M sodium acetate needed to make 20.00 mL of a buffer having pH = 4.00 and again to make 20.00 mL of a buffer with pH = 6.00. Your TA will check the accuracy of your calculations before you mix your buffer solutions.Our experiment uses a special case where both the acetic acid and sodium acetate are available in 0.20 M concentrations, but in general, the molarities of the weak acid and its sodium salt are not equal. If the molarity of the acid was twice that of the salt, explain how this would change the calculation.