# The equilibrium constant Kp for the following reaction is: ${{\mathrm{MgCO}}_{3}}_{\left(\mathrm{s}\right)}⇌{\mathrm{MgO}}_{\left(\mathrm{s}\right)}+{{\mathrm{CO}}_{2}}_{\left(\mathrm{g}\right)}$ 1.  2. $\mathrm{Kp}={\mathrm{P}}_{{\mathrm{CO}}_{2}}×\frac{{\mathrm{P}}_{{\mathrm{CO}}_{2}}×{\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_{3}}}$ 3. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{CO}}_{2}}+{\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_{3}}}$ 4. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{MgCO}}_{3}}}{{\mathrm{P}}_{{\mathrm{CO}}_{2}}×{\mathrm{P}}_{\mathrm{MgO}}}$

Subtopic:  Kp, Kc & Factors Affecting them |
89%
From NCERT
AIPMT - 2000
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The correct relation between dissociation constants of a di-basic acid is:

1. $K{a}_{1}=K{a}_{2}$

2. $K{a}_{1}>K{a}_{2}$

3. $K{a}_{1}

4. $K{a}_{1}=\frac{1}{K{a}_{2}}$

Subtopic:  Kp, Kc & Factors Affecting them |
69%
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 |
81%
From NCERT
AIPMT - 2000
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Equilibrium constants K1 and K2 for the following equilibria

are related as:

1.

2. ${\mathrm{K}}_{2}=\frac{{\mathrm{K}}_{1}}{2}$

3.

4. ${\mathrm{K}}_{2}={\mathrm{K}}_{1}^{2}$

Subtopic:  Introduction To Equilibrium |
88%
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 |
89%
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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At 25 ºC, the dissociation constant of a base, BOH, is 1.0 × 10–12. The concentration of hydroxyl ions in 0.01M aqueous solution of the base would be:

 1 1.0 × 10–6 mole L–1 2 1.0 × 10–7 mole L–1 3 2.0 × 10–6 mole L–1 4 1.0 × 10–5 mole L–1
Subtopic:  Ionisation Constant of Acid, Base & Salt |
74%
From NCERT
AIPMT - 2005
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$\mathrm{If A}$ $+$ $B$ $⇋$ $C$ $+$ $D$ $Cons\mathrm{tan}t$ $=$ ${K}_{1}$
$E$ $+$ $F$ $⇌$ $G$ $+$ $H$ $Cons\mathrm{tan}t$ $=$ ${K}_{2}$

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