Ka1, Ka2 and Ka3 are the respective ionisation constants for the following reactions.
\(\mathrm{H}_2 \mathrm{~S} \rightleftharpoons \mathrm{H}^{+}+\mathrm{HS}^{-}\)
\(\mathrm{HS}^{-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{S}^{2-}\)
\(\mathrm{H}_2 \mathrm{~S} \rightleftharpoons 2 \mathrm{H}^{+}+\mathrm{S}^{2-}\)
The correct relationship between Ka1, Ka2 and Ka3 is:

1. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} \times \mathrm{K}_{\mathrm{a}_2} \) 2. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1}+\mathrm{K}_{\mathrm{a}_2} \)
3. \(K_{a_3}=K_{a_1}-K_{a_2} \) 4. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} / \mathrm{K}_{\mathrm{a}_2}\)

Subtopic:  Introduction To Equilibrium |
 80%
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Acidity of BF3 can be explained on the basis of: 

1. Arrhenius concept

2. Bronsted Lowry concept 

3. Lewis concept

4. Bronsted Lowry as well as Lewis concept

Subtopic:  Acids & Bases - Definitions & Classification |
 78%
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The mixture that will produce a buffer solution when mixed in equal volumes is:

1. 0.1 mol dm-3 NH4OH and 0.1 mol dm-3 HCl
2. 0.05 mol dm-3 NH4OH and 0.1 mol dm-3 HCl
3. 0.1 mol dm-3 NH4OH and 0.05 mol dm-3 HCl
4. 0.1 mol dm-3 CH3COONa and 0.1 mol dm-3 NaOH

Subtopic:  Buffer |
 59%
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Among the following solvents, silver chloride is most soluble in:

1. 0.1 mol dm-3 AgNO3 solution

2. 0.1 mol dm-3 HCl solution

3. H2O

4. Aqueous ammonia

Subtopic:  Common Ion Effect |
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The value of the pH of \(0.01 \) \(\text{mol dm}^{-3}   \)\(\text{CH}_3\text{COOH}\) \(\left(K_a=1.74 \times 10^{-5}\right)\)  is:

1. 3.4 2. 3.6
3. 3.9 4. 3.0
Subtopic:  pH calculation |
 62%
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Which of the following alternatives best describes the reaction A ⇌ B at its halfway point?

1. \(\Delta G^{\ominus}=0\) 2. \(\Delta G^{\ominus}>0\)
3. \(\Delta G^{\ominus}<0\) 4. \(\Delta G^{\ominus}=-RTlnK\)
Subtopic:  Kp, Kc & Factors Affecting them |
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On increasing the pressure, the direction in which the gas phase reaction proceeds to re-establish equilibrium is predicted by applying Le-Chatelier's principle. Consider the reaction,

N2(g)+3H2(g)2NH3(g)

Which of the following is correct, if the total pressure at which the equilibrium is established is increased without changing the temperature?

1. K will remain the same.
2. K will decrease.
3. K will increase.
4. K will increase initially and then decrease, when pressure is very high.

Subtopic:  Le Chatelier's principle |
 62%
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The addition of a small amount of argon at a constant volume will not affect the equilibrium of the following reaction:

1. H2(g)+I2(g)⇌2HI(g)
2. PCl5(g)⇌ PCl3(g)+Cl2(g)
3. N2(g)+3H2(g)⇌2NH3(g)
4. The equilibrium will remain unaffected in all the three cases.

Subtopic:  Le Chatelier's principle |
 73%
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 At 450 K, Kp= 2.0 × 1010 bar-1 for the given reaction at equilibrium

2SO2(g+ O2(g)  2SO3(g) 

The value of  Kc at this temperature would be :

1. 7.48 ×1012 M-1
2. 6.56 × 1011 M-1
3. 7.48 × 1011 M-1
4. 1.23 × 1010 M-1

Subtopic:  Kp, Kc & Factors Affecting them |
 68%
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For the reaction: FeO(s) + CO(g)  Fe(s) +CO2(g), Kp = 0.265  at 1050 K. If the initial partial pressures are pCO= 1.4 atm and pCO2= 0.80 atm, the partial pressure of CO2 at equilibrium at 1050 K would be:

1. 4.61 atm 2. 1.74 atm
3. 0.46 atm 4. 0.17 atm
Subtopic:  Kp, Kc & Factors Affecting them |
 52%
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