Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations :
A)  $60 mL \frac{M}{10}HCI + 40 mL \frac{M}{10}NaOH$
B)   $55 mL \frac{M}{10}HCI + 45 mL \frac{M}{10}NaOH$
C)  $75 mL \frac{M}{5}HCI + 25 mL \frac{M}{5}NaOH$
D)  $100 mL \frac{M}{10}HCI + 100 mL \frac{M}{10}NaOH$
pH of which one of them will be equal to 1?
1. B
2. A
3. D
4. C

The solubility of BaSO₄ in water is $2.42 \times {10}^{-3}$ g/ litre at 298 K. The value of the solubility product will be:

(Molar mass of BaSO₄ = 233 gmol^–1)

1.  $1.08 \times {10}^{-10} {\mathrm{mol}}^2 {\mathrm{L}}^{-2}$
2.  $1.08 \times {10}^{-12} {\mathrm{mol}}^2 {\mathrm{L}}^{-2}$
3.  $1.08 \times {10}^{-14} {\mathrm{mol}}^2 {\mathrm{L}}^{-2}$
4.  $1.08 \times {10}^{-8} {\mathrm{mol}}^2 {\mathrm{L}}^{-2}$

Which of the following conditions will favour maximum formation of the product in the reaction, 
 $A_2 \left(g\right) + B_2 \left(g\right) \leftrightharpoons X_2 \left(g\right) {∆}_{r}H = -X k J$ ?

1. Low temperature and high pressure
2. Low temperature and low pressure
3. High temperature and high pressure
4. High temperature and low pressure

Among the following the correct order of acidity is

1. HClO < HClO₂< HClO₃< HClO₄
2. HClO₂< HClO < HClO₃< HClO₄
3. HClO₄< HClO₂< HClO < HClO₃
4. HClO₃< HClO₄< HClO₂< HClO

At room temperature, MY and NY3, two nearly insoluble salts, have the same K_sp values of 6.2 x 10^-13 . The true statement regarding MY and NY₃ is:

1. The molar solubility of MY in water is less than that of NY₃.

2. The salts MY and NY₃ are more soluble in 0.5 M KY than in pure water

3. The addition of the salt of KY to a solution of MY and NY₃ will have no effect on their solubilities

4. The molar solubilities of MY and NY₃ in water are identical.

When equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed, then the pH of the resulting solution will be:
1. 12.65
2. 2.0
3. 7.0
4. 1.04

An acidic buffer cannot be formed by which of the following combinations?
1. ${\mathrm{HClO}}_4 \mathrm{and} {\mathrm{NaClO}}_4$
2. ${\mathrm{CH}}_3\mathrm{COOH} \mathrm{and} {\mathrm{CH}}_3\mathrm{COONa}$
3. ${\mathrm{H}}_2{\mathrm{CO}}_3 \mathrm{and} {\mathrm{Na}}_2{\mathrm{CO}}_3$
4. ${\mathrm{H}}_3{\mathrm{PO}}_{4 }\mathrm{and} {\mathrm{Na}}_3{\mathrm{PO}}_4$

If the equilibrium constant for ${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right) \rightleftarrows 2\mathrm{NO}\left(\mathrm{g}\right)$ is K, the equilibrium constant for 
$\frac{1}{2}{\mathrm{N}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right) \rightleftarrows \mathrm{NO}\left(\mathrm{g}\right)$will be?

1. $K^{\frac{1}{2}}$

2. $\frac{1}{2}K$

3. K

4. $K^2$

Aqueous solution of which of the following compounds is the best conductor of electric current?
1. Acetic acid, $C_2{H}_4{O}_2$
2. Hydrochloric acid, HCl
3. Ammonia, $N{H}_3$
4. Fructose, $C_6{H}_{12}{O}_6$

The value of the equilibrium constant for a particular reaction is 1.6 x 10¹². When the system is in equilibrium, it will include:
1. All reactants
2. Mostly reactants
3. Mostly products
4. Similar amounts of reactants and products