A weak acid, HA has a Ka of 1.00 x 10-5. If 0.100 mole of this acid is dissolved in one litre of water, the percentage of acid dissociated at equibrium is closest to
1. 99.9%
2. 1.00%
3. 99.9%
4. 0.100%
Ionisation constant of CH3COOH is 1.7 X 10-5 and concentration of H+ ions is 3.4 X 10-4.Then, find out initial concentration of CH3COOH molecules.
1. 3.4 X 10-4
2. 3.4 X 10-3
3. 6.8 X 10-4
4. 6.8 X 10-3
Given, HF + H2OH3O+ + F-
F- + H2O HF + OH-
which relation is correct?
1. Kb =Kw
2. Kb =1/Kw
3. Ka x Kb =Kw
4. Ka/Kb = Kw
The concentration of [H+] and concentration of [OH-] of a 0.1M aqueous solution of 2% ionised weak monobasic acid is
[ionic product of water = 1x 10-14]
1. 0.02x10-3 M and 5x10-11 M
2. 1x10-3 M and 3x10-11 M
3. 2x10-3 M and 5x10-12 M
4. 3x10-2 M and 4x10-13 M
Aqueous solution of acetic acid contains
1. CH3COO- and H+
2. CH3COO-, H3O+ and CH3COOH
3. CH3COO-, H3O+ and H+
4. CH3COOH, CH3COO- and H+
An aqueous solution of hydrogen sulphide shows the equilibrium,
H2S H+ + HS-
If dilute hydrochloric acid is added to an aqueous solution of hydrogen sulphide without any temperature change, then:
1. | The equilibrium constant will change |
2. | The concentration of HS- will increase |
3. | The concentration of undissociated hydrogen sulphide will decrease |
4. | The concentration of HS- will decrease |
The following equilibrium exists in an aqueous solution
CH3COOH H+ + CH3COO- . If dilute HCl is added to this solution:
1. the equilibrium constant will increase
2. the equilibrium constant will decrease
3. acetate ion concentration will increase
4. acetate ion concentration will decrease
In the following reaction
Which are the two Bronsted bases ?
1.
2.
3.
4.
Ostwald dilution law for weak electrolyte HA can be given as
The molecule that is least likely to behave as Lewis base is:
1. NH3
2. BF3
3. OH-
4. H2O