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

Subtopic:  pH calculation |
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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

Subtopic:  Ionisation Constant of Acid, Base & Salt |
 66%
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The species that can act as Bronsted acids as well as bases is/are:

1.  H2O

2.  HCO3-, HSO4- 

3.  NH3

4.  All of the above.

Subtopic:  Acids & Bases - Definitions & Classification |
 85%
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The solubility product of silver chromate is 1.1×10-12. The solubility of silver chromate will be:

1. 6.5×10-5mol L-1

2. 6.5×10-6mol L-1

3. 5.5×10-5mol L-1

4. 5.5×10-6mol L-1

Subtopic:  Solubility Product |
 55%
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The solubility product of mercurous iodide is 4.5×10-29. The solubility of mercurous iodide will be:

1. 6.5×10-7mol L-1

2. 4.09×10-8mol L-1

3. 4.09×10-7mol L-1

4. 6.5×10-8mol L-1

Subtopic:  Solubility Product |
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Consider the following graph:

The point that represents reaction in equilibrium is-

1. C

2. A

3. B

4. D

Subtopic:  Introduction To Equilibrium |
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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

Subtopic:  Introduction To Equilibrium |
 67%
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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
Subtopic:  Salt Hydrolysis & Titration |
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The following concentrations were obtained for the formation of NH3 from N2 and H2 at equilibrium at 500K.
[N
2] = 1.5 × 10–2M. [H2] = 3.0 ×10–2 M and
[NH
3] = 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
Subtopic:  Introduction To Equilibrium |
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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

Subtopic:  Introduction To Equilibrium |
 63%
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