# $\mathrm{If A}$ $+$ $B$ $⇋$ $C$ $+$ $D$ $Cons\mathrm{tan}t$ $=$ ${K}_{1}$$E$ $+$ $F$ $⇌$ $G$ $+$ $H$ $Cons\mathrm{tan}t$ $=$ ${K}_{2}$ then C + D + E + F ⇒ product. The constant of reaction will be: 1.  $\frac{{K}_{1}}{{K}_{2}}$ 2.  $\frac{{K}_{2}}{K1}$ 3. ${K}_{1}{K}_{2}$ 4. None of these

Subtopic:  Kp, Kc & Factors Affecting them |
77%
From NCERT
AIPMT - 1998
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The fertilizer which makes the soil acidic is:

1. ${\left(N{H}_{4}\right)}_{2}S{O}_{4}$

2.  Super phosphate of lime .

3. $C{H}_{3}COONa$

4. $Ca{\left(N{O}_{3}\right)}_{2}$

Subtopic:  Salt Hydrolysis & Titration |
73%
From NCERT
AIPMT - 1998
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What is the correct relationship between the pHs of isomolar solutions of sodium oxide (pH1), sodium sulphide (pH2), sodium selenide (pH3), and sodium telluride (pH4)?

1. ${\mathrm{pH}}_{1}<{\mathrm{pH}}_{2}<{\mathrm{pH}}_{3}<{\mathrm{pH}}_{4}$

2. ${\mathrm{pH}}_{1}>{\mathrm{pH}}_{2}>{\mathrm{pH}}_{3}>{\mathrm{pH}}_{4}$

3. ${\mathrm{pH}}_{1}<{\mathrm{pH}}_{2}<{\mathrm{pH}}_{3}\approx {\mathrm{pH}}_{4}$

4. ${\mathrm{pH}}_{1}>{\mathrm{pH}}_{2}\approx {\mathrm{pH}}_{3}>{\mathrm{pH}}_{4}$

Subtopic:  pH calculation |
58%
AIPMT - 2005
Hints

H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because:

 1 Presence of HCl decreases the sulphide ion concentration 2 Sulphides of group IV cations are unstable in HCl 3 Solubility product of group II sulphides is more than that of group IV sulphides 4 Presence of HCl increases the sulphides ion concentration
Subtopic:  Common Ion Effect |
AIPMT - 2005
Hints

Among the following examples, the species that behave(s) as a Lewis acid is/are:
$B{F}_{3},SnC{l}_{2},SnC{l}_{4}$
1. Stannous chloride, stannic chloride
2. $B{F}_{3}$stannous chloride
3. Only $B{F}_{3}$
4. $B{F}_{3}$, stannous chloride , stannic chloride

Subtopic:  Acids & Bases - Definitions & Classification |
From NCERT
AIPMT - 1999
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4 gm of NaOH is dissolved in 1000 ml of water. The ${\mathrm{H}}^{+}$ ion concentration will be:

 1 10-1 M 2 10-13 M 3 10-4 M 4 10-10 M
Subtopic:  pH calculation |
70%
From NCERT
AIPMT - 1999
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The solubility product of a sparingly soluble salt AX2 is 3.2 ×10–11. Its solubility (in moles/litre) is:

1. 3.1×10–4

2. 2 × 10–4

3. 4 × 10–4

4. 5.6 × 10–6

Subtopic:  Solubility Product |
85%
From NCERT
AIPMT - 2004
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A compound BA2 has $$K_{sp} = 4\times 10^{-12}$$$.$Solubility of this compound will be:

 1 10-3 2 10-4 3 10-5 4 10-6
Subtopic:  Solubility Product |
84%
From NCERT
AIPMT - 1999
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The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to the ratio of the concentrations of the conjugate acid (HIn) and base (In–) forms of the indicator by the expression:

1. $\mathrm{log}\frac{\left[\mathrm{HIn}\right]}{\left[{\mathrm{In}}^{-}\right]}={\mathrm{pK}}_{\mathrm{In}}-\mathrm{pH}$

2. $\mathrm{log}\frac{\left[\mathrm{HIn}\right]}{\left[{\mathrm{In}}^{-}\right]}=\mathrm{pH}-{\mathrm{pK}}_{\mathrm{In}}$

3.

4. All of the above.

Subtopic:  Buffer |
From NCERT
AIPMT - 2004
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For a reaction , ${\mathrm{BaO}}_{2}\left(\mathrm{s}\right)⇌\mathrm{BaO}\left(\mathrm{s}\right)+{\mathrm{O}}_{2}\left(\mathrm{g}\right)$; ∆H = + ve. At equilibrium condition, the pressure of O2 depends on the:

1. Increased mass of BaO2

2. Increased mass of BaO

3. Increased temperature on equilibrium.

4. Increased mass of BaO2 and BaO both.

Subtopic:  Kp, Kc & Factors Affecting them |
82%
From NCERT
AIPMT - 2002
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