Question
1. At the freezing point of water(0?C), K w=1.210?15. Calculate [H+] and [OH?] fora neutral solution at thistemperature. [H+], [OH?] = ?? 2. Which solution
1. At the freezing point of water(0?C), Kw=1.2×10?15. Calculate [H+] and [OH?] fora neutral solution at thistemperature. [H+], [OH?] = ??
2. Which solution below has the highest concentration ofhydroxide ions?
pH = 6.0 | |
pH = 7.6 | |
pH = 4.5 | |
pH = 9.2 | |
pH = 12.4 |
3. Which solution below has the highest concentration ofhydronium ions?
pH = 6.5 | |
pH = 13.5 | |
pH = 9.9 | |
pH = 3.1 | |
pH = 7.7 |
4. An aqueous solution at 25.0°C contains [H+] = 0.085 M. Whatis the pH of the solution?
1.20 ? 10?13 | |||||||||||
1.07 | |||||||||||
13.0 | |||||||||||
-1.0 | |||||||||||
0.0850 5. The pH of an aqueous solution at 25.0 °C is 10.40. What isthe molarity of H+ in this solution?
|
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Get StartedRecommended Textbook for
Chemistry The Central Science
Authors: Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward
12th edition
321696727, 978-0132175081, 978-0321696724
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