In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Agand Pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl concentration is 0.10 M. What will the concentration of Agand Pb2+ at equilibrium?

(Ksp for AgCl  = 1.8 × 10-10)
(Ksp for PbCl2 = 1.7 × 10-5

1.

Ag+=1.8×10-11 M;

Pb2+=1.7×10-4M

2.

Ag+=1.8×10-7 M;

Pb2+=1.7×10-6M

3.

Ag+=1.8×10-11 M;

Pb2+=8.5×10-5M

4.

Ag+=1.8×10-9 M;

Pb2+=1.7×10-3M

Subtopic:  Solubility Product |
 62%
From NCERT
AIPMT - 2011
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The reaction-

2A+B(g)  3C(g)+D(g)

begins with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

1. [(0.75)3(0.25)]÷[(0.50)2(0.75)]

2. [(0.75)3(0.25)]÷[(0.50)2(0.25)]

3. [(0.75)3(0.25)]÷[(0.75)2(0.25)]

4. [(0.75)3(0.25)]÷[(1.00)2(1.00)]

Subtopic:  Kp, Kc & Factors Affecting them |
 65%
From NCERT
AIPMT - 2010
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Given reaction:  A2(g) + B2(g)  ⇋ 2AB(g)  

At equilibrium, the concentrations of  A2 = 3.0×10-3 M;  B2 = 4.2×10-3 M and AB=2.8×10-3M. If the reaction takes place in a sealed vessel at  527 °C, then the value of  KC will be: 

1. 3.9  2. 0.6 
3. 4.5 4. 2.0 
Subtopic:  Kp, Kc & Factors Affecting them |
 82%
From NCERT
AIPMT - 2012
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Given that the equilibrium constant for the reaction 

2SO2(g) + O2(g)  2SO3(g) 

has a value of 278 at a particular temperature, the value of the equilibrium constant for the following reaction at the same temperature will be:

SO3(g)   SO2(g) + 1/2 O2(g) 

1.  3.6 × 10-3 

2.  6.0 × 10-2 

3.  1.3 × 10-5 

4.  1.8 × 10-3 

Subtopic:  Kp, Kc & Factors Affecting them |
 72%
From NCERT
AIPMT - 2012
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The equilibrium constant Kp for the following reaction is:

MgCO3(s)MgO(s)+CO2(g)

1. Kp PCO2

2. Kp=PCO2×PCO2×PMgOPMgCO3

3. Kp=PCO2+PMgOPMgCO3

4. Kp=PMgCO3PCO2×PMgO

Subtopic:  Kp, Kc & Factors Affecting them |
 88%
From NCERT
AIPMT - 2000
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The correct relation between dissociation constants of a di-basic acid is:

1. Ka1=Ka2

2. Ka1>Ka2

3. Ka1<Ka2

4. Ka1=1Ka2

Subtopic:  Kp, Kc & Factors Affecting them |
 68%
From NCERT
AIPMT - 2000
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For any reversible reaction, if we increase the concentration of the reactants, the effect on equilibrium constant will:
1. Depend on the amount of concentration
2. Remain unchanged
3. Decrease
4. Increase

Subtopic:  Kp, Kc & Factors Affecting them |
 80%
From NCERT
AIPMT - 2000
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Equilibrium constants K1 and K2 for the following equilibria

NO(g)+12O2K1NO2( g) and 2NO2( g)K22NO(g)+O2( g)

are related as:

1. K2=1 K1

2. K2=K12

3. K2=1 K12

4. K2=K12

Subtopic:  Introduction To Equilibrium |
 87%
From NCERT
AIPMT - 2005
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Conjugate acid of NH2 is:

1. NH4OH

2. NH4+

3. \(NH_{2}^{-}\)

4. NH3

Subtopic:  Acids & Bases - Definitions & Classification |
 88%
From NCERT
AIPMT - 2000
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Incorrect statement about pH and H+ is: 
 

1. pH of neutral water is not zero.
2. Adding 1M solution of CH3COOH and 1M solution of NaOH, the pH will be 7.
3. H+ of dilute and hot H2SO4 is more than concentrate and cold H2SO4
4. Mixing solution of CH3COOH and HCl, pH will be less than 7

Subtopic:  pH calculation |
 73%
From NCERT
AIPMT - 2000
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