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Equilibrium · Question 58

AIPMT 2011 (Mains)MCQMedium📈 Topic in 38% papers+4−1
1

In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and 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 concentrations of Ag+ and Pb2+ be at equilibrium ? ( Ksp for AgCl = 1.8 10-10, Ksp for PbCl2 = 1.7 10-5)

  1. [Ag+] = 1.8 10-7 M, [ Pb2+] = 1.7 10-6 M
  2. [Ag+] = 1.8 10-11 M, [ Pb2+] = 8.5 10-5 M
  3. [Ag+] = 1.8 10-9 M, [ Pb2+] = 1.7 10-3 M
  4. [Ag+] = 1.8 10-11 M, [ Pb2+] = 1.7 10-4 M

Answer

(3) [Ag+] = 1.8 10-9 M, [ Pb2+] = 1.7 10-3 M

Solution

At equilibrium [Cl-] = 0.10 M and both salts precipitate (ionic products 0.1 0.1 and 0.1 (0.1)2 exceed their Ksp).

For AgCl: Ksp = [Ag+][Cl-]

⇒ [Ag+] = 1.8 10-100.10

= 1.8 10-9 M

For PbCl2: Ksp = [ Pb2+][Cl-]2

⇒ [ Pb2+] = 1.7 10-5(0.10)2

= 1.7 10-3 M

Answer: (3)

AIPMT 2011 (Mains)

Keep practising — Equilibrium

2

The value of H for the reaction X2(g) + 4Y2(g) 2XY4(g) is less than zero. Formation of XY4(g) will be favoured at

  1. high temperature and high pressure
  2. low pressure and low temperature
  3. high temperature and low pressure
  4. high pressure and low temperature
AIPMT 2011 (Prelims)
3

A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 10-5, what is the pH of this solution? ( 2.7 = 0.43)

  1. 9.08
  2. 9.43
  3. 11.72
  4. 8.73
AIPMT 2011 (Prelims)
4

Which of the following is least likely to behave as Lewis base?

  1. H2O
  2. NH3
  3. BF3
  4. OH-
AIPMT 2011 (Prelims)
5

For the reaction, N2(g) + O2(g) 2NO(g), the equilibrium constant is K1. The equilibrium constant is K2 for the reaction, 2NO(g) + O2(g) 2NO2(g) What is K for the reaction, NO2(g) 12N2(g) + O2(g)

  1. 12K1K2
  2. 14K1K2
  3. [ 1K1K2 ]1/2
  4. 1K1K2
AIPMT 2011 (Prelims)
6

The reaction, 2A(g) + B(g) 3C(g) + D(g) is begun 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)] [(1.00)2(1.00)]
  2. [(0.75)3(0.25)] [(0.50)2(0.75)]
  3. [(0.75)3(0.25)] [(0.50)2(0.25)]
  4. [(0.75)3(0.25)] [(0.75)2(0.25)]
AIPMT 2010 (Mains)
7

If pH of a saturated solution of Ba(OH)2 is 12, the value of its Ksp is

  1. 4.00 10-6 M3
  2. 4.00 10-7 M3
  3. 5.00 10-6 M3
  4. 5.00 10-7 M3
AIPMT 2010 (Prelims)
8

What is [H+] in mol/L of a solution that is 0.20 M in CH3COONa and 0.10 M in CH3COOH? Ka for CH3COOH = 1.8 10-5

  1. 3.5 10-4
  2. 1.1 10-5
  3. 1.8 10-5
  4. 9.0 10-6
AIPMT 2010 (Prelims)
9

In which of the following equilibrium Kc and Kp are not equal?

  1. 2NO(g) N2(g) + O2(g)
  2. SO2(g) + NO2(g) SO3(g) + NO(g)
  3. H2(g) + I2(g) 2HI(g)
  4. 2C(s) + O2(g) 2CO(g)
AIPMT 2010 (Prelims)
10

In a buffer solution containing equal concentration of B- and HB, the Kb for B- is 10-10. The pH of buffer solution is

  1. 10
  2. 7
  3. 6
  4. 4
AIPMT 2010 (Prelims)
11

The dissociation constants for acetic acid and HCN at 25 are 1.5 10-5 and 4.5 10-10 respectively. The equilibrium constant for the equilibrium CN- + CH3COOH HCN + CH3COO- would be

  1. 3.3 10-5
  2. 3.3 10-4
  3. 3.3 104
  4. 3.3 105
AIPMT 2009

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