1. Non-Vodcast Problem Eric Liu June 10, 2007 Chemistry AP

2. The Question: 1988 D Part A Part B Part C Part D This is an “essay”-type problem. Be sure to keep your words clear and concise. A 30.00 milliliter sample of a weak monoprotic acid was titrated with a standardized solution of NaOH. A pH meter was used to measure the pH after each increment of NaOH was added, and the curve above was constructed.

3. The Question: Part A Explain how this curve could be used to determine the molarity of the acid. Things to keep in mind: Keep your explanation precise and to the point! Answer the Question

4. The How-to: Part A Step 1 Sketch the curve described in the question This curve portrays a weak monoprotic acid, HA, being titrated with a strong base, NaOH. Therefore the equivalence point will be at a pH greater than 7. Volume of “x” molar NaOH added pH 7 0 Equivalence point 14 "half-way point"

5. The How-to: Part A Step 2 At the equivalence point, the there should be equal amounts (number of moles) of NaOH and monoprotic acid in solution. In other words, all the monoprotic acid will have reacted with the base. Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

6. The How-to: Part A Step 3 Since you know the molarity and volume of NaOH used at the equivalence point based on the curve, you can calculate the number of moles of base. This will correspond to the number of moles of monoprotic acid in your sample (we’ll call it “y”). Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

7. The How-to: Part A Step 4 Once you know the number of moles acid: You can do the following calculation to find the original molarity of the acid, as you know your sample of acid was 30.00mL. Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

8. The Question, cont.: Part B Things to keep in mind: Info and work from Part A Answer the question Explain how this curve could be used to determine the dissociation constant K a of the weak monoprotic acid. Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

9. The How-to: Part B Step 1 At the “half-way point” on the curve you drew from Part A, half of the weak monoprotic acid has been titrated Therefore, [HA] = [A - ] Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

10. The How-to: Part B Step 2 The equilibrium expression for the dissociation of HA is: As previously determined, at the “half-way” point:, so [H 3 O + ] = K a Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

11. The How-to: Part B Step 3 Since you are given the pH at the “half-way point”, you can calculate [H 3 O + ] Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

12. The Question, cont.: Part C Things to keep in mind: Explain your answer! If you were to repeat the titration using an indicator in the acid to signal the endpoint, which of the following indicators should you select? Give the reason for your choice. a. Methyl RedK a = 1 x 10 -5 b. Cresol RedK a = 1 x 10 -8 c. Alizarin YellowK a = 1 x 10 -11 Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

13. The How-to: Part C Step 1 Take the pK a of each: pK a Methyl Red = 5 pK a Cresol Red = 8 pK a Alizarin Yellow = 11 Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14 pK a = -log(K a )

14. The How-to: Part C Step 2 The equivalence point is closest to 8. Therefore, one would choose Cresol Red as the appropriate indicator. Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

15. The How-to: Part C Step 3 The equilibrium expression for any indicator can be: where A - is the indicator ion. An indicator changes color when the equilibrium shifts from one side to the other. When more of [A - ] than [HA] becomes present, it changes color, and vice versa. Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

16. The How-to: Part C Step 4 Just before an indicator changes color, [A - ] = [HA] Therefore, [H 3 O + ] = K a (as noted in Part B), or pH = pK a, The equivalence point of this curve is near 8, so an indicator that changes color at pH of 8 is best (Cresol Red) Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

17. The Question, cont.: Part D Things to keep in mind: Strong Acid vs. Strong Base Weak Acid vs. Strong Base Sketch the titration curve that would result if the weak monoprotic acid were replaced by a strong monoprotic acid, such as HCl of the same molarity. Identify the differences between this titration curve and the curve shown above. Volume of “x” molar NaOH added pH 7 0 Equivalence point "half-way point" 14

18. The How-to: Part D Step 1 Sketch the two graphs Differences: The blue graph starts at a higher pH The blue graph has a shorter “steep slope” near the equivalence point Volume of “x” molar NaOH added pH 7 0 Equivalence point at >7 "half-way point" 14 Volume of “x” molar NaOH added pH 7 0 14 Weak Acid vs. Strong BaseStrong Acid vs. Strong Base Equivalence point at 7 ‘y’ mL Exaggerated slope increase

19. The Conclusion You’ve just finished 1988 D of an actual Chemistry AP Test! Congrats.