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With the help of an appropriate equation explain why the pH of the 0.2M CH3COOH rose...
Calculate the pH of 1.0L of the buffer 2.00M CH3COONa/2.00M CH3COOH before and after the addition of 0.090 mol NaOH. The Ka of CH3COOH is 1.8x10^-5
Calculate the pH of 2.00 L of the buffer 2.50 M CH3COOH/1.50 M CH3COONa after the addition of 0.25 mol NaOH. For CH3COOH/CH3COONa, Ka = 1.8 ´ 10-5 and pKa = 4.74. Assume no volume changes after addition of 0.25 mol NaOH. You can assume that [H+] at equilibrium is very small. Select one: a. 6.21 b. 6.09 c. 5.96 d. 5.12 e. 4.58
Calculate the pH of 1.00 L of the buffer 1.04 M CH3COONa/1.10 M CH3COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: (b) pH after addition of 0.045 mol NaOH: (c) pH after further addition of 0.145 mol HCl:
Calculate the pH of 1.00 L of the buffer 1.03 M CH3COONa/0.97 M CH3COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: (b) pH after addition of 0.080 mol NaOH: (c) pH after further addition of 0.144 mol HCl:
Calculate the pH of 1.00 L of the buffer 1.05 M CH3COONa/0.96 M CH3COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: 4.786 (b) pH after addition of 0.065 mol NaOH: (c) pH after further addition of 0.144 mol HCI:
What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 x 10-5 So the answer is 4.64. However, I was under the impression that it is Ka * (base/acid). So wouldn't that be 1.8 x 10^-5 * (.35/.45)? Isn't the CH3COONa the base? Someone please explain. Thank you.
When is using the Henderson-Hasselbalch equation not appropriate for solving for pH? Why?
5. A solution is made up of 0.2m naocl and .01m hocl,
please explain all
5. A solution is made up of 0.2M NaOCl and 0.1 M HOCl. a) Write the net ionic equation that represents the reaction of this solution with a strong acid. b) Write the net ionic equation that represents the reaction of this solution with a strong base. c) Calculate the pH of this solution.
Explain how dissolving the Group IV carbonate precipitate with 6M CH3COOH, followed by the addition of extra acetic acid, establishes a buffer with a pH of approximately 5.
please help
Calculate the pH of the solution at every stage of titration. The Ka of CH3COOH is 2.4 x10-5. 2 decimal places for all three answers in this question. a. After the addition of 20.0 ml of 0.10 M NaOH to 20.0 ml of 0.15 M CH3COOH. b. After the addition of 30.0 ml of 0.10 M NaOH to 20.0 ml of 0.15 M CH3COOH. c. After the addition of 40.0 ml of 0.10 M NaOH to 20.0 ml...