a)
HClO dissociates as:
HClO -----> H+ + ClO-
0.592 0 0
0.592-x x x
Ka = [H+][ClO-]/[HClO]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((3*10^-8)*0.592) = 1.333*10^-4
since c is much greater than x, our assumption is correct
so, x = 1.333*10^-4 M
So, [H+] = x = 1.333*10^-4 M
use:
pH = -log [H+]
= -log (1.333*10^-4)
= 3.8753
Answer: 3.88
b)
H3AsO3 dissociates as:
H3AsO3 -----> H+ + H2AsO3-
0.646 0 0
0.646-x x x
Ka = [H+][H2AsO3-]/[H3AsO3]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((5.1*10^-10)*0.646) = 1.815*10^-5
since c is much greater than x, our assumption is correct
so, x = 1.815*10^-5 M
So, [H+] = x = 1.815*10^-5 M
use:
pH = -log [H+]
= -log (1.815*10^-5)
= 4.7411
Answer: 4.74
c)
C5H5N dissociates as:
C5H5N +H2O -----> C5H5NH+ + OH-
0.731 0 0
0.731-x x x
Kb = [C5H5NH+][OH-]/[C5H5N]
Kb = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Kb = x*x/(c)
so, x = sqrt (Kb*c)
x = sqrt ((1.7*10^-9)*0.731) = 3.525*10^-5
since c is much greater than x, our assumption is correct
so, x = 3.525*10^-5 M
So, [OH-] = x = 3.525*10^-5 M
use:
pOH = -log [OH-]
= -log (3.525*10^-5)
= 4.4528
use:
PH = 14 - pOH
= 14 - 4.4528
= 9.5472
Answer: 9.55
0/4 Submissions Used -/0.1 points 22 Determine the pH of each of the following solutions. (a)...
22. + -/0.1 points 0/4 Submissions Used Determine the pH of each of the following solutions. (a) 0.555 M hydrogen peroxide (weak acid with Ka = 2.4e-12). (b) 0.665 M acetic acid (weak acid with Ka = 1.8e-05). (c) 0.207 M pyridine (weak base with Kb = 1.7e-09).
22. + -10.1 points 0/4 Submissions Used Determine the pH of each of the following solutions. (a) 0.360 M phenol (weak acid with Ka = 1.3e-10). (b) 0.458 M hydrogen peroxide (weak acid with Ka = 2.4e-12). (c) 0.238 M pyridine (weak base with Kb = 1.7e-09).
3. -/0.1 points 0/4 Submissions Used Calculate the percent ionization of arsenous acid (H3ASO3) in solutions of each of the following concentrations (Kg = 5.1e-10.) (a) 0.135 M (b) 0.357 M (c) 0.805 M
27. + -/0.1 points 0/4 Submissions Used Determine the pH of each of the following solutions. (a) 0.120 M hydrazoic acid (weak acid with Ka = 1.98-05). (b) 0.146 M phenol (weak acid with Ka = 1.3e-10). (c) 0.534 M pyridine (weak base with Kb = 1.72-09).
Determine the pH of each of the following solutions. (a) 0.807 M hypochlorous acid (weak acid with Ka = 3e-08). (b) 0.672 M hypoiodous acid (weak acid with Ka = 2.3e-11). (c) 0.807 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions. Determine the pH of each of the following solutions. (a) 0.211 M hypobromous acid (weak acid with Ka = 2.5e-09) Ка 3 Зе-08). (b) 0.235 M hypochlorous acid (weak acid with Ka (c) 0.586 M pyridine (weak base with K 1.7e-09)
Determine the pH of each of the following solutions. (a) 0.607 M hydrosulfuric acid (weak acid with Ka = 9.5e-08). (b) 0.155 M hypoiodous acid (weak acid with Ka = 2.3e-11). (C) 0.549 M pyridine (weak base with Kb = 1.7e-09).
-/0.1 points 23. 0/4 Submissions Used Calculate the percent ionization of carbonic acid (H2CO3) in solutions of each of the following concentrations (Ka = 4.3e-07.) (a) 0.148 M % (b) 0.436 M % (c) 0.718 M %
Determine the pH of each of the following solutions. (a) 0.532 M phenol (weak acid with Ka = 1.3e-10). (b) 0.277 M hypobromous acid (weak acid with Ka = 2.5e-09). (c) 0.713 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions. (a) 0.416 M hypobromous acid (weak acid with Ka = 2.5e-09). pH = ___________ (b) 0.644 M ascorbic acid (weak acid with Ka = 8e-05). pH = ___________ (c) 0.703 M pyridine (weak base with Kb = 1.7e-09). pH = ___________