The concentration of Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is $2.2\times {10}^{-4}mol L^{-1}$ . The solubility product of Ag₂C₂O₄ is
1. $2.66\times {10}^{-12}$
2. $4.5\times {10}^{-11}$
3.$5.3\times {10}^{-12}$
4. $2.42\times {10}^{-8}$

The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅N⁺H) In A 0.10 M aqueous pyridine solution (K_b for C₅H₅N = 1.7 X 10 ^-9) is

1.  0.0060%

2.  0.013%

3.  0.77%

4.  1.6%

The solubility of AgCl (s) with solubility product 1.6 x 10^-10 in 0.1 M NaCl solution would be

1.  $1.26\times {10}^{-5} \mathrm{M}$
2.  $1.6\times {10}^{-9} \mathrm{M}$
3.  $1.6\times {10}^{-11} \mathrm{M}$
4.  zero

Boric acid is an acid because its molecule
1.  contains replaceable H⁺ ion
2.  gives up a proton
3.  accepts OH^- from water releasing proton into the solution
4.  combines with proton from water molecules

A 20 litre container at 400 K contains CO₂ (g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of CO₂ attains its maximum value, will be: 

Given that : $SrC{O}_3\left(s\right) \leftrightharpoons SrO\left(s\right) + C{O}_2\left(g\right) , kp = 1.6 atm$
1. 10 litre
2. 2 litre
3. 4 litre
4. 5 litre

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.