The most acidic compound among the following is:

1.		2.
3.		4.

The product 'D' in the above-mentioned reaction is: 

1.		2.
3.		4.

Calculate the hydrogen ion concentration, [\(\text{H}^+\)] (in \(\text{mol}/\text{L}\)), of a buffer solution prepared by mixing \(0.10 \text{ M}\) acetic acid (\(\text{CH}_3\text{COOH}\)) and \(0.20 \text{ M}\) sodium acetate (\(\text{CH}_3\text{COONa}\)), given that the acid dissociation constant (\(\text{K}_a\)) for acetic acid is \(1.8 \times 10^{-5}\):

1. \(3 . 5 \times 10^{- 4}\)
2. \(1 . 1 \times 10^{- 5}\)
3. \(1 . 8 \times 10^{- 5}\)
4. \(9 . 0 \times10^{- 6}\)${\mathrm{}}^{}$

For an endothermic reaction, the energy of activation is E_a, and the enthalpy of reaction is ΔH (both of these in kJ/mol). The minimum value of E_a will be:

1. Less than $∆$H

2. Equal to $∆$H

3. More than $∆$H

4. Equal to zero

The correct order of increasing C-X bond reactivity toward nucleophiles among the following is:

I		II
III	\(\left(\mathrm{CH}_3\right)_3 \mathrm{C}-\mathrm{X}\)	IV	\(\left(\mathrm{CH}_3\right)_2 \mathrm{CH}-\mathrm{X}\)

Find the standard Gibbs energy change for the reduction of Ag⁺ by copper metal if E°cell = +0.46 V at 25°C.

Given: F = 96,500 C mol⁻¹

1. -89.0 kJ

2. -89.0 J

3. -44.5 kJ

4. -98.0 kJ

The equilibrium reaction that doesn't have equal values for K_c and K_p is: 

1. \(2NO(g) \rightleftharpoons N_2(g) + O_2(g)\)
2. \(SO_2(g) + NO_2(g) \rightleftharpoons SO_3(g) + NO(g)\)
3. \(H_2(g) + I_2(g) \rightleftharpoons 2HI (g)\)
4. \(2C(s) + O_2(g) \rightleftharpoons 2CO_2(g)\)

Which of the following ions will exhibit colour in aqueous solutions?

1. La³⁺ (Z=57)

2. Ti³⁺ (Z=22)

3. Lu³⁺ (Z=71)

4. Sc³⁺ (Z=21)

Aniline gives a set of the following reactions that yielded a coloured product 'Y':
      

The structure of 'Y' is :

1.
2.
3.
4.

The reagent that is used to convert acetamide into methyl amine is:

1. NaOH-Br₂

2. Soda lime

3. Hot conc. H₂SO₄

4. PCl₅