# 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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NEET - 2023
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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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NEET - 2023
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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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NEET - 2023
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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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NEET - 2023
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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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NEET - 2022
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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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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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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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$$3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{g})$$
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 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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