1
answer
0
watching
150
views
18 Nov 2019
The water autoionization constant is temperature dependent, and at 50 degree C K_w = 5.495 times 10^-14. The pH of neutral water at this temperature is The H_3 O^+ (or H^+) concentration at pH 5.70 (at 25 degree C with the K_2 = 1.0 times 10^-14 is (2 sig figs) times 10 (integer). The OH^- concentration at pH 4.18 (at 25 degree with the K_2 = 1.0 times 10^-14 is (2 sig figs) times 10 The K_a of acetic acid at 25 degree C is 1.8 times 10^-5. The K_b of acetic acid at this temperature is (integer). Use the information in question 3 (above) to calculate the pH of a 0.20 M solution of acetic acid at a temperature of 25 degree C. The pH of the solution is Use the information in question 3 (above) to calculate the pH of a solution obtained by combining 20.0 ml of 0.20 M acetic acid and 10.0 ml of 0.20 M sodium hydroxide. The calculated pH of the solution is
The water autoionization constant is temperature dependent, and at 50 degree C K_w = 5.495 times 10^-14. The pH of neutral water at this temperature is The H_3 O^+ (or H^+) concentration at pH 5.70 (at 25 degree C with the K_2 = 1.0 times 10^-14 is (2 sig figs) times 10 (integer). The OH^- concentration at pH 4.18 (at 25 degree with the K_2 = 1.0 times 10^-14 is (2 sig figs) times 10 The K_a of acetic acid at 25 degree C is 1.8 times 10^-5. The K_b of acetic acid at this temperature is (integer). Use the information in question 3 (above) to calculate the pH of a 0.20 M solution of acetic acid at a temperature of 25 degree C. The pH of the solution is Use the information in question 3 (above) to calculate the pH of a solution obtained by combining 20.0 ml of 0.20 M acetic acid and 10.0 ml of 0.20 M sodium hydroxide. The calculated pH of the solution is
Jarrod RobelLv2
7 Jan 2019