Answer the fоllоwing questiоn. A 25.00 mL аliquot of the weаk (HA) аcid was titrated with 0.1185 M NaOH(aq) using both an indicator and a pH meter. Ka (HA), is 6.50 x10-4. A total of 29.38 mL of 0.1185 M NaOH(aq) was required to reach the equivalence point. 1. Calculate the molarity of the acid solution. (4 pts) 2. Calculate the pH of the acid solution before titration (Hint: use the RICE table). (4 pts) 3. Calculate the pH and [A-] at the half-equivalence point. (4 pts) 4. Calculate the pH at the equivalence point of the titration. (Hint: use Kb for hydrolysis of A- anion and RICE table). (4 pts) 5. Calculate the pH of the solution after 20.00 mL of 0.1185 M NaOH(aq) was added. (Hint: ignore the spectator sodium ion and find moles of acid and A- and use Henderson-Hasselbalch equation). (2EC) Submit your final answers here. After submitting the exam, upload the matching calculations to the Exam 3 Solutions, Extra Credit, and Partial Credit assignment. GL