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%
From NCERT
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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 |
 72%
From NCERT
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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%
From NCERT
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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 |
 68%
From NCERT
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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 |
 62%
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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%
From NCERT
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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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On addition of inert gas at constant volume to the reaction, N2 + 3H22NH3 at  equilibrium:

1. the reaction halts

2. forward reaction is favored

3. the reaction remains unaffected

4. backward reaction is favored

Subtopic:  Le Chatelier's principle |
 82%
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In which of the following case reaction goes farthest to completion?

1. K=103                                         

2. K=10-2

3. K=10                                           

4. K=100

Subtopic:  Introduction To Equilibrium | Kp, Kc & Factors Affecting them |
 75%
From NCERT
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For the reversible reaction,

N2 (g) + 3H2(g) 2NH3 (g) + heat

 the equilibrium shifts in forward direction                                   

1. by increasing the concentration of NH3 (g) 

2. by decreasing the pressure

3. by decreasing the concentrations of N2 (g)and H2(g)

4. by increasing pressure and decreassing temperature

 

Subtopic:  Le Chatelier's principle |
 83%
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