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11 Nov 2019
3. Determine the pH at 25C of a solution prepared by dissolving 0.25 mole of ammonium chloride in 1.0 L of 0.28 M aqueous ammonia.
7.The pH of a bicarbonate-carbonic acid buffer is 7.28. Calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3â).(Ka1 of carbonic acid is 4.2 Ã10â7)
18. Calculate the pH of the following two buffer solutions:
(a) 1.1 M CH3COONa/2.9 M CH3COOH.
(b) 0.1 M CH3COONa/0.3 M CH3COOH.
Which is the more effective buffer?
A. 1.1 M CH3COONa/2.9 M CH3COOH
B. 0.1 M CH3COONa/0.3 M CH3COOH
32. The pH of a sodium acetate-acetic acid buffer is 4.60. Calculate the ratio [CH3COOâ] / [CH3COOH].
3. Determine the pH at 25C of a solution prepared by dissolving 0.25 mole of ammonium chloride in 1.0 L of 0.28 M aqueous ammonia.
7.The pH of a bicarbonate-carbonic acid buffer is 7.28. Calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3â).(Ka1 of carbonic acid is 4.2 Ã10â7)
18. Calculate the pH of the following two buffer solutions:
(a) 1.1 M CH3COONa/2.9 M CH3COOH.
(b) 0.1 M CH3COONa/0.3 M CH3COOH.
Which is the more effective buffer?
A. | 1.1 M CH3COONa/2.9 M CH3COOH |
B. | 0.1 M CH3COONa/0.3 M CH3COOH |
32. The pH of a sodium acetate-acetic acid buffer is 4.60. Calculate the ratio [CH3COOâ] / [CH3COOH].
Jean KeelingLv2
12 Sep 2019