The solution that has the lowest pH is:
(assuming 100% dissociation)
1. | 0.003 M HCl | 2. | 0.005 M NaOH |
3. | 0.002 M HBr | 4. | 0.002 M KOH |
The degree of ionization of a 0.1 M bromoacetic acid solution is 0.132. The pKa of bromacetic acid will be:
1. 1.98
2. 2.75
3. 4.56
4. 7.15
The species that can act as Bronsted acids as well as bases is/are:
1.
2.
3.
4. All of the above.
The solubility product of silver chromate is . The solubility of silver chromate will be:
1.
2.
3.
4.
The solubility product of mercurous iodide is . The solubility of mercurous iodide will be:
1.
2.
3.
4.
Consider the following graph:
The point that represents reaction in equilibrium is-
1. C
2. A
3. B
4. D
The concentration vs time graph for the Haber process is given below:
The curve representing hydrogen gas is
1. Y
2. Z
3. X
4. In the Haber process, hydrogen gas is not used
The pKb of dimethylamine and pka of acetic acid are 3.27 and 4.77 respectively at T (K).
The correct option for the pH of dimethylammonium acetate solution is:
1. | 7.75 | 2. | 6.25 |
3. | 8.50 | 4. | 5.50 |
The following concentrations were obtained for the formation of NH3 from N2 and H2 at equilibrium at 500K.
[N2] = 1.5 × 10–2M. [H2] = 3.0 ×10–2 M and
[NH3] = 1.2 ×10–2M.
The equilibrium constant value is:
1. | 3.55 × 102
|
2. | 20.6 × 103
|
3. | 2.06 × 104
|
4. | 10.6 × 104 |
The value of Kc = 4.24 at 800K for the reaction,
CO(g) + H2O(g) CO2 (g) + H2 (g)
If only CO and H2O are present initially at concentrations of 0.10M each.
The equilibrium concentrations of CO2, and CO are-
1. 0.067 M; 0.033 M
2. 0.76 M; 0.029 M
3. 0.65 M; 0.027 M
4. 0.061 M; 0.30 M