a)
HN3 dissociates as:
HN3 -----> H+ + N3-
0.12 0 0
0.12-x x x
Ka = [H+][N3-]/[HN3]
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 ((1.9*10^-5)*0.12) = 1.51*10^-3
since x is comparable c, our assumption is not correct
we need to solve this using Quadratic equation
Ka = x*x/(c-x)
1.9*10^-5 = x^2/(0.12-x)
2.28*10^-6 - 1.9*10^-5 *x = x^2
x^2 + 1.9*10^-5 *x-2.28*10^-6 = 0
This is quadratic equation (ax^2+bx+c=0)
a = 1
b = 1.9*10^-5
c = -2.28*10^-6
Roots can be found by
x = {-b + sqrt(b^2-4*a*c)}/2a
x = {-b - sqrt(b^2-4*a*c)}/2a
b^2-4*a*c = 9.12*10^-6
roots are :
x = 1.5*10^-3 and x = -1.519*10^-3
since x can't be negative, the possible value of x is
x = 1.5*10^-3
So, [H+] = x = 1.5*10^-3 M
use:
pH = -log [H+]
= -log (1.5*10^-3)
= 2.8238
Answer: 2.82
b)
C6H5OH dissociates as:
C6H5OH -----> H+ + C6H5O-
0.146 0 0
0.146-x x x
Ka = [H+][C6H5O-]/[C6H5OH]
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 ((1.3*10^-10)*0.146) = 4.357*10^-6
since c is much greater than x, our assumption is correct
so, x = 4.357*10^-6 M
So, [H+] = x = 4.357*10^-6 M
use:
pH = -log [H+]
= -log (4.357*10^-6)
= 5.3609
Answer: 5.36
C)
C5H5N dissociates as:
C5H5N +H2O -----> C5H5NH+ + OH-
0.534 0 0
0.534-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)*0.534) = 3.013*10^-5
since c is much greater than x, our assumption is correct
so, x = 3.013*10^-5 M
So, [OH-] = x = 3.013*10^-5 M
use:
pOH = -log [OH-]
= -log (3.013*10^-5)
= 4.521
use:
PH = 14 - pOH
= 14 - 4.521
= 9.479
Answer: 9.48
27. + -/0.1 points 0/4 Submissions Used Determine the pH of each of the following solutions....
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).
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).
0/4 Submissions Used -/0.1 points 22 Determine the pH of each of the following solutions. (a) 0.592 M hypochlorous acid (weak acid with Ka 3e-08). (b) 0.646 M arsenous acid (weak acid with Ka = 5.1e-10). (c) 0.731 M pyridine (weak base with Kg 1.7e-09). 23. -/0.1 points 0/4 Submissions Used Calculate the percent ionization of arsenous acid (H3AsO3) in solutions of each of thef
Determine the pH of each of the following solutions. (a) 0.571 M carbonic acid (weak acid with Ka = 4.3e-07). (b) 0.332 M propionic acid (weak acid with Ka = 1.3e-05). (c) 0.308 M pyridine (weak base with Kb = 1.72-09).
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) 0.213 M boric acid (weak acid with Ka = 5.8e-10). (b) 0.394 M phenol (weak acid with Ka = 1.3e-10). (c) 0.869 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions. (a) 0.410 M propionic acid (weak acid with Ka = 1.3e-05). (b) 0.122 M benzoic acid (weak acid with Ka = 6.3e-05). (c) 0.867 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 = ___________
27. Determine the pH of each of the following solutions. (a) 0.354 M hypoiodous acid (weak acid with Ka = 2.3e-11). = _________ (b) 0.156 M carbonic acid (weak acid with Ka = 4.3e-07). = ________ (c) 0.476 M pyridine (weak base with Kb = 1.7e-09). = ________
Determine the pH of each of the following solutions. (a) 0.492 M carbonic acid (weak acid with Ka = 4.3e-07). (b) 0.770 M benzoic acid (weak acid with Ka = 6.3e-05). (c) 0.697 M pyridine (weak base with Kb = 1.7e-09).