just the two questions with red around them

Calculate the pH of a solution prepared by mixing 0.0860mol of chloroacetic acid plus 0.0170mol of sodium chloroacetate 1.00L of water. First do the calculation by assuming that the concentrations of HA and Aequal their formal concentrations. The pKa of chloroacetic acid is 2.865. Then do the calculation with [HA] and [A]from Equations 9.21 and 9.22. [HA]=FHA[H+]+[OH](921)[A]=FA+[H+][OH](922) Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of 1.00I:0.210molClCH2CO2H,0.050molClCH2CO2Na, 0.080molHNO3, and 0.080molCa(OH)2. Ca(OH)2 provides 2OH [HA]=FHA[H+]+[OH][A]=FA+[H+][OH] Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of 1.00L:0.210molClCH2CO2H,0.050molClCHCO2Na, 0.080molHNO3, and 0.080molCa(OH)2. Ca(OH)2 provides 2OH