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3. For the following questions, consider the table given below. Indicator pH range of color change Color of undissociated indicator Color of conjugate base Appropriate indicator for titration of 0.1000 M reagents of acid and base SA-SB WA-SB WB-SA Bromocresol 3.8 5.4 Yellow Blue green Phenolphthalein 8.2 10.0 Colorless Pink Methyl red 4.8-6.0 Red Yellow Methyl orange 3.2 4.4 Red Yellow SA strong acid, SB = strong base, WA = weak acid, WB = weak base a. Calculate [H] and pH for each of the following solutions and list the color that would be imparted to the solution by one drop of (i) bromocresol green, (ii) phenolphthalein. (1) 0.05 M HC1 (2) 1.2×10 M HC1 (3) 250 ppm HC1 b. Calculate [H] and pH for each of the following solutions and list the color that would be imparted to the solution by one drop of (i) methyl orange, (ii) phenolphthalein. (1) 0.05 M NaOH (2) 1.3 M NaOH (3) Freshly boiled water at 25°C C. Acid base indicators are usually weak acids, which can exist in solution as either the undissociated acid or the dissociated conjugate base. The two species have different colors. As the pH of the titration changes, the predominant form of the indicator changes from one form to the other. In the table above, check off which indicator(s) would be appropriate for each type of titration. d. A graph of the titration curve for a weak acid titrated with NaOH is given on the next page. The volume of NaOH is reported in mL. Determine what volume of base must be added in order to get a change in the color of the indicator if the indicator used is (i) Bromocresol green (ii) Methyl red (iii) Phenolphthalein (iv) Methyl orange