The molecule that cannot function as both Bronsted acid and base: 

1. ${\mathrm{HCO}}_3^{-}$

2. ${\mathrm{NH}}_3$

3. HCl

4. ${\mathrm{HSO}}_4^{-}$

The solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ in 0.1 M NaOH is:

K_sp ($\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$)= 2x ${10}^{-15}$

1. 2 x ${10}^{-8}$ M.

2. 1 x ${10}^{-13}$ M

3. 1 x ${10}^8$ M 

4. 2 x ${10}^{-13}$ 

At a certain temperature and pressure of 10⁵ Pa, iodine vapour contains 40% by volume of I atoms. The K_p for the equilibrium of the reaction would be-

 $I_2 \left(g\right) \leftrightharpoons 2I \left(g\right)$

1. 2.67 $\times$ 10⁴ Pa

2. 1.00 $\times$ 10⁵ Pa

3. 3.63 $\times$ 10⁴ Pa

4. 2.18 $\times$ 10⁵ Pa

Given the reaction 2HI _(g) $\rightleftharpoons$ H_2 (g) + I_2 (g)

A sample of HI_(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium, the partial pressure of HI_(g) is 0.04 atm.  The ${\mathrm{K}}_{\mathrm{P}}$ for the given equilibrium would be:

A mixture of 1.57 mol of N₂, 1.92 mol of H_2, and 8.13 mol of NH₃ is introduced into a 20 L vessel at 500 K. At this temperature, the equilibrium constant, K_c for the reaction N_2 (g) + 3H_2 (g) $\rightleftharpoons$ 2NH_3 (g) is 1.7 × 10².

The direction of the net reaction is:

1. Reaction is at equilibrium.

2. Reaction will proceed in forwarding direction.

3. Reaction will proceed in the backward direction.

4. Data is not sufficient.

Given the reaction:

2BrCl _(g) $\leftrightharpoons$ Br_2 (g) + Cl_2 (g); K_c= 32 at 500 K. If the initial concentration of BrCl is 3.3 × 10^-3 mol L^–1, the molar concentration of BrCl in the mixture at equilibrium would be:

1. 3.0 $\times$ 10^-2 molL^-1

2. 2.0 $\times$ 10^-4 molL^-1

3. 2.5 $\times$ 10^-6 molL^-1

4. 3.0 $\times$ $$10^-4 molL^-1

For the reaction, NO(g) + 1/2O₂ (g) ⇌ NO₂(g)

 ∆_fG° (NO₂₎ = 52.0 kJ/mol , ∆_fG° (NO) = 87.0 kJ/mol and
∆_fG° (O₂) = 0 kJ/mol. The equilibrium constant for the formation of NO₂ from
NO and O₂ at 298K would be

1. 2.36 $\times$ 10⁴ 

2. 3.10 $\times$ 10⁷

3. 1.36 $\times$ 10${}^6$

4. 2.18 $\times$ 10${}^5$

The equilibrium constant for the following reaction is 1.6 ×10⁵ at 1024K

H_2(g) + Br_2(g)  $\leftrightharpoons$2HBr_(g)

If HBr at pressure 10.0 bar is introduced into a sealed container at 1024 K, the equilibrium pressure of HBr will be :

1. 11.20 bar

2. 5.56 bar

3. 7.30 bar

4. 9.95 bar

Which of the following is/are the Lewis acids?

(i) BF₃     (ii) H₂O    (iii) H⁺       $\left(\mathrm{iv}\right)$ ${\mathrm{AlF}}_3$

1. Only (i)

2. (i) and (ii) only

3. (i) , (iii) and (iv) only

4. All of the above

A 0.02 M solution of pyridinium hydrochloride has a pH of 3.44.
The ionization constant of pyridine will be:

1. $6.6$ $\times$ ${10}^{-6}$

2. $1.51$ $\hspace{0.17em}\times$ ${10}^{-9}$

^{3. $2.36$ $\times$ ${10}^{-7}$}

4. $3.43$ $\times \hspace{0.17em}{10}^{-9}$