# The value of the equilibrium constant for a particular reaction is 1.6 × 1012. When the system is in equilibrium, it will include: 1. All reactants 2. Mostly reactants 3. Mostly products 4. Similar amounts of reactants and products

Subtopic:  Kp, Kc & Factors Affecting them |
71%
From NCERT
NEET - 2015
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The Ksp of Ag2CrO4, AgCl, AgBr, and Agl are respectively, 1.1 × 10–12, 1.8 × 10–10, 5.0 × 10–13, 8.3 × 10–17. Which one of the following salts will precipitate last if ${\mathrm{AgNO}}_{3}$ solution is added to the solution containing equal moles of NaCl, NaBr, Nal, and Na2CrO4?

1. Agl

2. AgCl

3. AgBr

4. Ag2CrO4

Subtopic:  Solubility Product |
52%
From NCERT
NEET - 2015
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Which of the following salts will give the highest pH in water?
1. KCl
2. NaCl
3. Na2CO3
4. CuSO4

Subtopic:  pH calculation |
75%
From NCERT
AIPMT - 2014
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For the reversible reaction:
N2(g) + 3H2(g) $$\rightleftharpoons$$ 2NH3(g) + heat

The equilibrium shifts in a forward direction:

1. by increasing the concentration of $N{H}_{3}\left(g\right)$
2. by decreasing the pressure.
3. by decreasing the concentration of ${N}_{2}\left(g\right)$ $and$ ${H}_{2}\left(g\right)$
4. by increasing pressure and decreasing temperature.

Subtopic:  Le Chatelier's principle |
84%
From NCERT
AIPMT - 2014
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For a given exothermic reaction, Kp and Kp are the equilibrium constants at temperatures T1 and Trespectively. Assuming that the heat of reaction is constant in temperatures range between T1 and T2, it is a readily observation that:
1. ${K}_{p}>{K}_{p}^{\text{'}}$
2. ${K}_{p}<{K}_{p}^{\text{'}}$
3. ${K}_{p}={K}_{p}^{\text{'}}$
4. ${K}_{p}=\frac{1}{{K}_{p}^{\text{'}}}$

Subtopic:  Kp, Kc & Factors Affecting them |
55%
AIPMT - 2014
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Which of these is least likely to act as Lewis base?
1. F
2. BF3
3. PF3
4. CO

Subtopic:  Acids & Bases - Definitions & Classification |
74%
From NCERT
AIPMT - 2013
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The strongest acid among the following compounds is:

 1 HClO3 2 HClO4 3 H2SO3 4 H2SO4
Subtopic:  Ionisation Constant of Acid, Base & Salt |
74%
From NCERT
AIPMT - 2013
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pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product Ksp of Ba (OH)2 is:
1. $3.3×{10}^{-7}$
2. $5.0×{10}^{-7}$
3. $4.0×{10}^{-6}$
4. $5.0×{10}^{-6}$

Subtopic:  Solubility Product |
68%
From NCERT
AIPMT - 2012
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Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?

1. $$\mathrm{B a C l_{2}}$$
2. $$\mathrm{A l C l_{3}}$$
3. $$\mathrm{L i C l}$$
4. $$\mathrm{B e C l_{2}}$$${}_{}$

Subtopic:  pH calculation |
55%
From NCERT
AIPMT - 2012
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Buffer solutions have constant acidity and alkalinity because:

 1 these give unionized acid or base on reaction with added acid or alkali. 2 acid and alkali in these solutions are shielded from attack by other ions 3 they have large excess of H+ or OH- ions 4 they have fixed  value of pH

Subtopic:  Buffer |
57%
From NCERT
AIPMT - 2012
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