Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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1-8 would be great.
1. Fill in the following table. [H₂O) (M) 5.9x10² [OH] (M) POH 6.5 3.6x10-5 2. Perform the following calculations. a. Calculate the pH of a 0.06 M HBr solution. b. Calculate the pH of a 0.025 M Ba(OH)2 solution. 3. In the lab you make a 0.65 M solution of an unknown acid. a. If the measured pH of the solution is 4.56, what is the K, of the acid? b. Based on your answer in a, if you were to make a 0.36 M solution of the unknown acid, what would the expected pH be? 4. In the lab you make a 0.26 M solution of methyl amine, which has a K₁= 4.4x104. a. Find the [OH] in this solution. b. What is the pH of this solution? 5. Determine the K, or K, for each of the provided K, or K... a. k, = 3.0x108 b. K₁= 1.8x10 c. Kb = 4.4x104 d. k, = 1.7x10 6. Consider a solution of 0.70 M NaF (K, of HF = 6.6x10¹¹). a. Will this solution be acidic, basic or neutral? b. What is the pH of this solution? 7. Calculate the pH of a benzoic acid/benzoate buffer containing 0.999 M benzoic acid and 0.995 M benzoate. The K, of benzoic acid is 6.3x10¹5. 8. Consider the titration of 0.2 M nitrous acid (K. = 4.5x104) by 0.1 M NaOH. Calculate the pH when the following volume of NaOH have been added to 250 mL of nitrous acid. a. 0.00 ml b. 200.00 mL c. 500.00 mL d. 700.00 mL PH 3.9
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Transcribed Image Text:1. Fill in the following table. [H₂O) (M) 5.9x10² [OH] (M) POH 6.5 3.6x10-5 2. Perform the following calculations. a. Calculate the pH of a 0.06 M HBr solution. b. Calculate the pH of a 0.025 M Ba(OH)2 solution. 3. In the lab you make a 0.65 M solution of an unknown acid. a. If the measured pH of the solution is 4.56, what is the K, of the acid? b. Based on your answer in a, if you were to make a 0.36 M solution of the unknown acid, what would the expected pH be? 4. In the lab you make a 0.26 M solution of methyl amine, which has a K₁= 4.4x104. a. Find the [OH] in this solution. b. What is the pH of this solution? 5. Determine the K, or K, for each of the provided K, or K... a. k, = 3.0x108 b. K₁= 1.8x10 c. Kb = 4.4x104 d. k, = 1.7x10 6. Consider a solution of 0.70 M NaF (K, of HF = 6.6x10¹¹). a. Will this solution be acidic, basic or neutral? b. What is the pH of this solution? 7. Calculate the pH of a benzoic acid/benzoate buffer containing 0.999 M benzoic acid and 0.995 M benzoate. The K, of benzoic acid is 6.3x10¹5. 8. Consider the titration of 0.2 M nitrous acid (K. = 4.5x104) by 0.1 M NaOH. Calculate the pH when the following volume of NaOH have been added to 250 mL of nitrous acid. a. 0.00 ml b. 200.00 mL c. 500.00 mL d. 700.00 mL PH 3.9
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