Solubility of a gas in liquid increases on:

1. Addition of a catalyst

2. Increasing the pressure

3. Decreasing the pressure

4. Increasing the temperature

A solution is called saturated if:

1. ionic concentration product < solubility product

2. ionic concentration product > solubility product

3. ionic concentration product $\ge$ solubility product

4. none of the above

The concentration of [H⁺] and concentration of [OH^-] of a 0.1M aqueous solution of 2% ionised weak monobasic acid is                                                                    

[ionic product of water = 1x 10^-14]

1. 0.02x10^-3 M and 5x10^-11 M

2. 1x10^-3 M and 3x10^-11 M

3. 2x10^-3 M and 5x10^-12 M

4. 3x10^-2 M and 4x10^-13 M

The relation for calculating pH of a weak base is:

1. pH =pK_w -1/2 pK_b + 1/2 logc

2. pH =pK_w +1/2 pK_b - 1/2 logc

3. pH =pK_w -1/2 pK_a + 1/2 logc

4. none of the above

Eight mole of a gas AB₃ attain equilibrium in a closed container of volume 1 dm³ as,

2 AB₃ $\rightleftharpoons$ A₂(g) + 3B₂(g). If at equilibrium 2 mole of A₂ are present then, equilibrium constant is:

1. 72 mol²L^-2                     

2. 36 mol²L^-2 

3. 3 mol²L^-2                       

4. 27 mol²L^-2  

Which is Lewis base?

1. HCl               

2. HNO₃

3. HF               

4. NH₃

For a reversible reaction, if the concentrations of the reactants are doubled, the equilibrium constant will be                                                                                       

1. one-fourth                         

2. halved

3. doubled                             

4. the same

The molecule that is least likely to act as a Lewis base is:     

1. CO         

2. \(F^{-}\)         

3. AlCl₃      

4. PF₃

For a hypothetical equilibrium:

$4\mathrm{A} + 5\mathrm{B} \stackrel{ }{\rightleftharpoons } 4\mathrm{x} + 6\mathrm{y}$;
the equilibrium constant K_c has the unit:

1. mol² litre^-2

2. litre mol^-1

3. litre² mol^-2

4. mol litre^-1

Calculate the pOH of a solution at 25$°$C that contains 1x10^-10 M of hydronium ion.        

1. 7.00                         

2. 4.00

3. 9.00                         

4. 1.00