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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If the solubility of MX2 – type electrolytes is 0.5 × 10–4 Mole/lit. then Ksp of electrolytes will be:

1. $5×{10}^{-12}$

2. $25×{10}^{-10}$

3. $1×{10}^{-13}$

4. $5×{10}^{-13}$

Subtopic:  Solubility Product |
76%
From NCERT
AIPMT - 2002
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The compound with the highest pH among the following is:

1. CH3COOK

2. Na2CO3

3. NH4Cl

4. NaNO3

Subtopic:  Salt Hydrolysis & Titration |
56%
From NCERT
AIPMT - 2002
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If a solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25, then pKb of NH4OH is:

1. 9.25

2. 4.75

3. 3.75

4. 8.25

Subtopic:  pH calculation |
68%
From NCERT
AIPMT - 2002
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A compound among the following that cannot be classified as a protonic acid is:

 1 B(OH)3 2 PO(OH)3 3 SO(OH)2 4 SO2(OH)2
Subtopic:  Acids & Bases - Definitions & Classification |
79%
From NCERT
AIPMT - 2003
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The reaction quotient (Q) for the reaction:

${\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)⇌2{\mathrm{NH}}_{3}\left(\mathrm{g}\right)$

is given by $\mathrm{Q}=\frac{{\left[{\mathrm{NH}}_{3}\right]}^{2}}{\left[{\mathrm{N}}_{2}\right]{\left[{\mathrm{H}}_{2}\right]}^{3}}$. The reaction will proceed from right to left if:
1. Q = KC
2. Q < KC
3. Q > KC
4. Q = 0

(where KC is the equilibrium constant)

Subtopic:  Kp, Kc & Factors Affecting them |
74%
From NCERT
AIPMT - 2003
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The solubility product of AgI at 25 ºC is 1.0 × 10–16 mol2 L–2. The solubility of AgI in 10–4 N solution of KI at 25 ºC is approximately (in mol L–1):

1. $1.0×{10}^{-16}$

2. $1.0×{10}^{-12}$

3. $1.0×{10}^{-10}$

4. $1.0×{10}^{-8}$

Subtopic:  Solubility Product |
84%
From NCERT
AIPMT - 2003
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The following equilibria are given:

 $$N_{2} \ + \ 3H_{2} \ \rightleftharpoons \ 2NH_{3}$$ K1 $$N_{2} \ + \ O_{2} \ \rightleftharpoons \ 2NO$$ K2 $$H_{2} \ + \ \frac{1}{2}O_{2} \ \rightleftharpoons \ H_{2}O$$ K3

The equilibrium constant of the reaction
$$2NH_{3} \ + \ \frac{5}{2}O_{2} \ \rightleftharpoons \ 2NO \ + \ 3H_{2}O$$ in terms of K1, K2 and K3 is:

1. K1.K2.K3
2. $$\mathrm{\frac{K_{1}K_{2}}{K_{3}}}$$
3. $$\mathrm{\frac{K_{1}K_{3}^{2}}{K_{3}}}$$
4. $$\mathrm{\frac{K_{2}K_{3}^{3}}{K_{1}}}$$

Subtopic:  Introduction To Equilibrium |
83%
From NCERT
AIPMT - 2003
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