The pKa for acid A is greater than pKa for acid B. The strong acid is:

1. Acid A                                           

2. Acid B

3. Are equally strong                         

4. None of the above

Subtopic:  Acids & Bases - Definitions & Classification |
 84%
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At a certain temperature, 2HI H2 +I2 only 50% HI is dissociated at equilibrium. The equilibrium constant is:

1. 1.0                     

2. 3.0                 

3. 0.5               

4. 0.25

Subtopic:  Kp, Kc & Factors Affecting them |
 64%
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A solution of FeCl3 in water acts as acidic due to:

1. Acidic impurities                         

2. Ionization

3. Hydrolysis of Fe3+                       

4. Dissociation

Subtopic:  Salt Hydrolysis & Titration |
 72%
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Which of the following solution does not act as buffer?

1. H3PO4 + NaH2PO4

2. Na2CO3 + H2CO3

3. HCl + NH4Cl

4. CH3COOH + CH3COONa

Subtopic:  Buffer |
 71%
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Which equilibrium can be described as Lewis acid-base reaction but not Bronsted acid-base reaction?

1. H2O + CH3COOHH3O+ + CH3COO-

2. 2NH3 + H2SO4 2NH4+ + SO42-

3. NH3 + CH3COOH NH4+ + CH3COO-

4. [Cu(H2O)4]2+ + 4NH3  [Cu(NH3)4]2+ + 4H2O

Subtopic:  Acids & Bases - Definitions & Classification |
 73%
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In the reaction, PCl⇌ PCl3 + Cl2, the amounts of PCl5, PCl3, and Cl2 at equilibrium are 2 moles each and the total pressure is 3 atm. The equilibrium constant Kp is: 

1. 1.0 atm                                       

2. 2.0 atm

3. 3.0 atm                                       

4. 6.0 atm

Subtopic:  Kp, Kc & Factors Affecting them |
 66%
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An aqueous solution of hydrogen sulphide shows the equilibrium,

           H2H+ + 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
Subtopic:  Ionisation Constant of Acid, Base & Salt |
 70%
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When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because:

1. the impurities dissolve in HCl

2. HCl is highly soluble in H2O

3. the product of [Na+] and [Cl-] exceeds the solubility product of NaCl

4. the solubility product of NaCl is lowered by the chloride ion from aqueous HCl

Subtopic:  Solubility Product |
 63%
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The aqueous solution of a salt is alkaline. This shows that salt is made from:

1. a strong acid and strong base

2. a strong acid and weak base

3. a weak acid and weak base

4. a weak acid and strong base

Subtopic:  Acids & Bases - Definitions & Classification |
 83%
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40% of a racemic mixture of 0.2 moles of N2 and 0.6 moles of H2 react to give NH3 according to the equation, N2 (g) + H2(g)2NH3 (g) at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases is:

1. 4:5                       

2. 5:4

3. 7:10                     

4. 8:5

Subtopic:  Kp, Kc & Factors Affecting them |
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