Amongst the given option which of the following molecules/ion acts as a Lewis acid? 
1. \(\text{OH}^- \) 2. \(\text{NH}_3 \)
3. \(\text H_2 \text O \) 4. \(\text{BF}_3 \)
Subtopic:  Acids & Bases - Definitions & Classification |
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The equilibrium concentration of the species in the reaction \(A+B \rightleftharpoons C+D\) are 2, 3, 10 and 6 mol L–1, respectively at 300 K. \(\Delta G^o\) for the reaction is: (R = 2 cal/mol K) 
1. –13.73 cal  2. 1372.60 cal 
3. –137.26 cal  4. –1381.80 cal
Subtopic:  Introduction To Equilibrium |
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Which combination of the following substances will result in the formation of an acidic buffer when mixed?
1. Weak acid and it's salt with a strong base.
2. Equal volumes of equimolar solutions of weak acid and weak base.
3. Strong acid and its salt with a strong base.
4. Strong acid and its salt with a weak base.
(The pKa of acid = pKb of the base)
Subtopic:  Buffer |
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For a weak acid HA, the percentage of dissociation is nearly 1% at equilibrium. If the concentration of acid is 0.1 mol L-1, then the correct option for its Ka at the same temperature will be:
1. \(1 \times 10^{-4}\)    
2. \(1 \times 10^{-6} \)
3. \(1 \times 10^{-5} \)
4. \(1 \times 10^{-3} \)
Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is: 
[Given pKa of CH3COOH = 4.57]
1. 2.57 2. 5.57
3. 3.57 4. 4.57
Subtopic:  pH calculation |
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\(3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{g}) \) 
For the above reaction at 298 K, \(\text K_c\) is found to be \(3.0 \times 10^{-59} \). If the concentration of \(\text O_2\) at equilibrium is 0.040 M, then the concentration of \(\text O_3 \) in M is: 
1. \(1.2 \times 10^{21} \)
2. \(4.38 \times 10^{-32} \)
3. \(1.9 \times 10^{-63} \)
4. \(2.4 \times 10^{31} \)

Subtopic:  Introduction To Equilibrium |
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The solubility product of \(\mathrm{BaSO_4}\) in water is \(1.5 \times 10^{-9} \). The molar solubility of \(\mathrm{BaSO_4}\) in 0.1 M solution of Ba(NO3)2 in- 
1. \(2.0 \times 10^{-8} M\)
2. \(0.5 \times 10^{-8} M\)
3. \(1.5 \times 10^{-8} M\)
4. \(1.0 \times 10^{-8} M\)

Subtopic:  Solubility Product |
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Consider the following reaction taking place in 1L capacity container at 300 K.
\(\mathrm{A +B \rightleftharpoons C+D }\)
If one mole each of A and B are present initially and at equilibrium 0.7 mol of C is formed, then the equilibrium constant \((K_c) \) for the reaction is

1. 9.7  2. 1.2 
3. 6.2  4. 5.4 
Subtopic:  Introduction To Equilibrium |
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If 0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is :
1. 3 2. 2
3. 4 4. 1
Subtopic:  pH calculation |
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Kp for the following reaction is 3.0 at 1000 K.
\(\mathrm{CO_{2}(g)\,+\,C(s)\rightarrow \,2CO(g)}\)
The value of Kfor the reaction at the same temperature is: 
(Given - R = 0.083 L bar K–1 mol–1)
1. 0.36 2. 3.6 × 10–2
3. 3.6 × 10–3 4. 3.6
Subtopic:  Introduction To Equilibrium |
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