An antacid tablet, with magnesium hydroxide as the active ingredient, was dissolved in 20.00 mL of 1.0686 M hydrochloric solution. After the tablet completely reacted, the excess hydrochloric acid was titrated with 10.65 mL of 1.0825 M sodium hydroxide. At the completion of the titration, the solution was dark pink. Phenolphthalein was used as the indicator in this experiment. The labeled mass of the magnesium hydroxide is 311 mg per tablet. Show all work. a) Write the molecular, ionic and net ionic equations for the reactions in this experiment. b) Calculate the mass of magnesium hydroxide in the antacid tablet using the experimental datac) Calculate the % recovery [(experimental value/label value) x 100]d) Is the percent recovery consistent with the experimental error, as indicated by the final solution being dark pink? (In other words, what does it mean experimentally when the final solution in this titration with phenolphthalein as the indicator is dark pink? What impact does this titration error have on the final results, in this case, the calculated mass of the magnesium hydroxide in the antacid tablet?)e) 10.00 mL of the sodium hydroxide solution used in this experiment diluted to 100.00 mL and this new solution was used to determine the molar mass of a monoprotic acid, HX (where X is some anion). 0.402 g of the monoprotic acid (HX) was dissolved in 100.0 mL of DI water and the solution was titrated with 18.20 mL of the dilute sodium hydroxide solution to a phenolphthalein endpoint. What is the molar mass of the acid?f) Are any of the reactions in this problem redox reactions? Why or why not?