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General Chemistry Principles & Modern Applications 9 th Edition Petrucci/Harwood/Herring/Madura Chapter 17 Additional Aspects of Acid-Base Equilibria Dr.

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Presentation on theme: "General Chemistry Principles & Modern Applications 9 th Edition Petrucci/Harwood/Herring/Madura Chapter 17 Additional Aspects of Acid-Base Equilibria Dr."— Presentation transcript:

1 General Chemistry Principles & Modern Applications 9 th Edition Petrucci/Harwood/Herring/Madura Chapter 17 Additional Aspects of Acid-Base Equilibria Dr. Travis D. Fridgen Memorial University of Newfoundland © 2007 Pearson Education

2 The acid dissociation constant for hexanoic acid is 1.41x A buffer solution is prepared by mixing hexanoic acid and sodium hexanoate and is found to have a pH of 4.9. What is the ratio of the salt to acid concentration in this buffer solution?

3 The acid dissociation constant for hexanoic acid is 1.41x A buffer solution is prepared by mixing hexanoic acid and sodium hexanoate and is found to have a pH of 4.9. What is the ratio of the salt to acid concentration in this buffer solution?

4 10.0 ml of molar NaOH is required to fully titrate a 30.0 mL sample of propanoic acid. What was the concentration of the acid sample? (no need to use a calculator) M M M M M

5 M M M M M 10.0 ml of molar NaOH is required to fully titrate a 30.0 mL sample of propanoic acid. What was the concentration of the acid sample? (no need to use a calculator).

6 15.0 ml of an NaOH solution is required titrate a 30.0 mL sample of oxalic which is known to be M. What was the concentration of the sodium hydroxide solution? (no need to use a calculator) M M M M M

7 15.0 ml of an NaOH solution is required titrate a 30.0 mL sample of oxalic which is known to be M. What was the concentration of the sodium hydroxide solution? (no need to use a calculator) M M M M M

8 What is the pH of a buffer solution composed of equimolar amounts of dimethylamine and dimethylammonium chloride? dimethylamine, K b = 5.4x

9 What is the pH of a buffer solution composed of equimolar amounts of dimethylamine and dimethylammonium chloride? dimethylamine, K b = 5.4x10 -4

10 A buffer solution containing equimolar amounts of the base, aniline, and the salt of its conjugate acid, aniline hydrochloride, will result in an acidic buffer solution. aniline K b = 4.3x True 2. False

11 A buffer solution containing equimolar amounts of the base, aniline, and the salt of its conjugate acid, aniline hydrochloride, will result in an acidic buffer solution. aniline K b = 4.3x True 2. False

12 Which of the following statements is incorrect? 1.A buffer solution contains a weak acid or base and the salt of its conjugate base or acid, respectfully. 2. A buffer solution resists changes in pH upon addition of small amounts of acid or base. 3. The more concentrated the buffer solution is, the better its buffer capacity. 4. Water is a buffer solution with a pH of A buffer solution containing 0.10 M acid and conjugate base has the same pH as a solution containing 1.0 M of the same acid and conjugate base. alt of its conjugate small amounts of

13 Which of the following statements is incorrect? 1.A buffer solution contains a weak acid or base and the salt of its conjugate base or acid, respectfully. 2. A buffer solution resists changes in pH upon addition of small amounts of acid or base. 3. The more concentrated the buffer solution is, the better its buffer capacity. 4. Water is a buffer solution with a pH of A buffer solution containing 0.10 M acid and conjugate base has the same pH as a solution containing 1.0 M of the same acid and conjugate base. alt of its conjugate small amounts of

14 malonic acid K a,1 = 1.5x10 -3 K a,2 = 2.0x10 -6 Malonic acid is a diprotic acid with the acid dissociation constants given to the right. A solution which contains sodium malonate NaC 3 H 3 O 4 1. is basic 2. is acidic 3. is neutral 4. will contain undissolved sodium malonate 5. None of the above answers is correct.

15 malonic acid K a,1 = 1.5x10 -3 K a,2 = 2.0x10 -6 Malonic acid is a diprotic acid with the acid dissociation constants given to the right. A solution which contains sodium malonate NaC 3 H 3 O 4 1. is basic 2. is acidic 3. is neutral 4. will contain undissolved sodium malonate 5. None of the above answers is correct.

16 ascorbic acid K a,1 = 8.0x10 -5 K a,2 = 1.6x Ascorbic acid is a diprotic acid (acidic groups circled). A solution which contains the mono-sodium salt of ascorbic acid, sodium ascorbate, 1. is basic 2. is acidic 3. is neutral 4. does not register on the pH scale. 5. None of the above answers is correct.

17 ascorbic acid K a,1 = 8.0x10 -5 K a,2 = 1.6x Ascorbic acid is a diprotic acid (acidic groups circled). A solution which contains the mono-sodium salt of ascorbic acid, sodium ascorbate, 1. is basic 2. is acidic 3. is neutral 4. does not register on the pH scale. 5. None of the above answers is correct.

18 A technician collects a sample of rainwater to test the pH. Her portable pH meter is reading low battery. Litmus paper turns red indicating that the sample is acidic. As well, methyl red was found to turn red and both bromphenol blue and thymol blue were found to turn yellow. What is the best pH range of the rainwater sample as determined by these experimental results? 1. pH < < ph < < ph < < ph < < ph < 5

19 A technician collects a sample of rainwater to test the pH. Her portable pH meter is reading low battery. Litmus paper turns red indicating that the sample is acidic. As well, methyl red was found to turn red and both bromphenol blue and thymol blue were found to turn yellow. What is the best pH range of the rainwater sample as determined by these experimental results? 1. pH < < ph < < ph < < ph < < ph < 5

20 volume of titrant / ml pH equivalence point The titration curve to the right best represents the titration of : 1. a weak base with a strong acid. 2. a weak acid with a strong base. 3. a strong acid with a strong base. 4. a strong base with a strong acid.

21 volume of titrant / ml pH equivalence point The titration curve to the right best represents the titration of: 1. a weak base with a strong acid. 2. a weak acid with a strong base. 3. a strong acid with a strong base. 4. a strong base with a strong acid.

22 volume of titrant / ml pH volume of titrant / ml pH volume of titrant / ml pH Which of the following titration curves best represents the titration of 15.0 mL of M NaOH with M HCl?

23 volume of titrant / ml pH volume of titrant / ml pH volume of titrant / ml pH Which of the following titration curves best represents the titration of 15.0 mL of M NaOH with M HCl?

24 In the titration of a weak acid with a strong base methyl red was used as the indicator. Which of the points on the titration curve to the right represents the equivalence point in the titration?

25 In the titration of a weak acid with a strong base methyl red was used as the indicator. Which of the points on the titration curve to the right represents the equivalence point in the titration?

26 In the titration of a weak acid with a strong base methyl red was used as the indicator. Which of the points on the titration curve to the right represents the endpoint in the titration?

27 In the titration of a weak acid with a strong base methyl red was used as the indicator. Which of the points on the titration curve to the right represents the endpoint in the titration?

28 When titrating a solution containing a weak acid such as acetic acid, the pH at the endpoint of the titration: 1. depends on the indicator used 2. is below is above 7.0

29 When titrating a solution containing a weak acid such as acetic acid, the pH at the endpoint of the titration: 1. depends on the indicator used 2. is below is above 7.0

30 Based on the titration curve to the right, the compound being titrated is most likely: 1. H 2 Se: pK a,1 =3.89, pK a,2 = H 2 SeO 4 : strong acid, pK a,2 = H 2 SeO 3 : pK a,1 =2.65, pK a,2 = Citric acid: pK a,1 =3.75, pK a,2 = Valine: pK a,1 =2.29, pK a,2 = 9.74

31 Based on the titration curve to the right, the compound being titrated is most likely: 1. H 2 Se: pK a,1 =3.89, pK a,2 = H 2 SeO 4 : strong acid, pK a,2 = H 2 SeO 3 : pK a,1 =2.65, pK a,2 = Citric acid: pK a,1 =3.75, pK a,2 = Valine: pK a,1 =2.29, pK a,2 = 9.74


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