summary:
For calculating pH of weak acid , we simply used following formula
Ka = c × (degree of dissociation)^2
[H+] = c × degree of dissociation
pH = -log [H+]
Where
Ka = dissociation constant of weak acid
For calculating pH of weak base , we used following formula
Kb= c × (degree of dissociation)^2
[OH-] = c × degree of dissociation
pOH = -log [OH-]
pH + pOH= 14
Where
Kb = dissociation constant of weak base
c = concentration of base
Determine the pH of each of the following solutions. (a) 0.571 M carbonic acid (weak acid...
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).
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).
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). = ________
please ansee all parts part 1 part 2 part 3 Calculate the pH of each of the following strong acid solutions. (a) 0.00859 M HBO pH = 2.066 (b) 0.333 g of HI in 34.0 L of solution pH = (c) 21.0 mL of 6.90 M HBr diluted to 3.90 L pH = (d) a mixture formed by adding 33.0 mL of 0.00391 M HBr to 83.0 ml of 0.000280 M HI pH = Calculate [OH ") and pH for...
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).
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) 0.213 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) 0.416 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 = ___________
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).
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).