The values of K_p1 and K_p2 for the reactions

$\mathrm{X}\rightleftharpoons \mathrm{Y} + \mathrm{Z} ........\left(\mathrm{i}\right)$
$\mathrm{and} \mathrm{A}\rightleftharpoons 2\mathrm{B} .........\left(\mathrm{ii}\right)$

are in ratio of 9:1, if degree of dissociation of X and A be equal, then total pressure at equilibrium (i) and (ii) are in the ratio 

1. 3:1

2. 1:9

3. 36:1

4. 1:1

For a sparingly soluble salt A^pB^q, the relationship of its solubility product (L_s) with its solubility (s) is:

1. L_s =s^p+q.p^p.q^q                           

2.  L_s =s^p+q.p^q.q^p  

3. L_s =s^pq.p^p.q^q                            

4.  L_s = s^pq.(pq)^p+q

For NH₄HS(s) $\rightleftharpoons$NH₃ (g) + H₂S(g), the observed pressure for reaction mixture in equilibrium is 1.12 atm at 106$°$C. The value of K_p for the reaction is:

1. 3.136 atm²                           

2. 0.3136 atm²

3. 31.36 atm²                           

4. 6.98 atm²

The hydrogen ion concentration of a 10^-8 M HCl aqueous solution at 298 K (K_w =10-14) is       

1. 1.0 x10^-6 M                     

2. 1.0525 x 10^-7 M

3. 9.525 x 10^-8 M               

4. 1.0 x10^-8 M

2 mole of PCl₅ were heated in a closed vessel of 2 litre capacity. At equilibrium 40% of PCl₅ dissociated into PCl₃ and Cl₂. The value of the equilibrium constant is :

1. 0.267

2. 0.53

3. 2.63

4. 5.3

The relation for calculating pH of a solution containing weak acid and its salt is:

1. pH = pK_a + log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Acid}\right]}$

2. pH = pK_a - log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Acid}\right]}$

3. pH = pK_a + log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Salt}\right]}$

4. pOH = pK_a - log$\frac{\left[\mathrm{Acid}\right]}{[\mathrm{Conjugate} \mathrm{Base}]}$

The equilibrium constant Br₂ $\rightleftharpoons$2Br at 500 K and 700 K are 10^-10 and 10^-5 respectively. The reaction is:

(a) endothermic                                  (b) exothermic

(c) fast                                               (d) slow

1. a,b

2.c,b

3.a,d

4 c,d

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

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

1. CO         

2. \(F^{-}\)         

3. AlCl₃      

4. PF₃

Solubility of MX₂ type electrolytes is 0.5x10^-4 mol/L, then the K_sp of electrolytes is :         

1. 5 x 10^-12

2. 25 x 10^-10

3. 1 x 10^-13

4. 5 x 10^-13