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The equilibrium constants $K_{{\mathit{P}}_{\mathit{1}}}$ and $K_{P_2}$ for the reactions X$\rightleftharpoons$2Y and Z $\rightleftharpoons$ P + Q respectively are in the ratio of 1:9. If the degree of dissociation ox X and Z be equal then the ratio of total pressure at these equilibria is:
1. 1:9                 
2. 1:36                 
3. 1:1                     
4. 1:3

Equimolar solutions of the following substances were prepared separetly. Which one of these will record the highest pH value?                                                                                             
1. BaCl₂         
2. AlCl₃         
 3. LiCl           
4. BeCl₂
 

A buffer solution is prepared in which the concentration of NH₃ is 0.3 M and the concentration of ${\mathrm{NH}}_4^{+}$ is 0.20 M. If the equilibrium constant, K_b for NH₃ equals 1.8x10^-5, what is the pH of this solution?                                                                                       
1. 9.43                             
2. 11.72
3. 8.73                               
4. 9.08

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

pH of a saturated solution of Ba(OH)₂ is 12. The value of solubility product K_sp of Ba(OH)₂ is
1. 3.3 x 10^-7                         
2. 5.0 x 10^-7
3. 4.0 x 10^-6                         
4.  5.0 x 10^-6

For the given reaction,
$2\mathrm{A}\left(\mathrm{s}\right) + \mathrm{B}\left(\mathrm{g}\right) \rightleftharpoons \mathrm{C}\left(\mathrm{g}\right) + 2\mathrm{D}\left(\mathrm{s}\right) + \mathrm{E}\left(\mathrm{s}\right)$
the degree of dissociation of B was found to be 20% at 300 K and 24% at 500K. The rate of backward reaction.
(1) Increases with increase in pressure and temperature
(2) Increases with increase in pressure and decrease in temperature
(3) Depends on temperature only and decrease with increase in temperature
(4) Increases with increase in concentration of B and increase in the temperature

In which solvent, solubility of AgCl is maximum ?
1. 0.01 M NaCl
2. Pure Water
3. 0.01 M NH₄OH
4. 0.05 M AgNO₃

$N_2+ 3H_2\rightleftharpoons 2N{H}_3$
1 mole \(N_2\) and \(3H_2\) are at 4 atm.
Equilibrium pressure is found to be 3 atm. find the \(K_p\)
1. \(\frac{1}{0.5(1.5)^3}\) 
2. \(\frac{1}{0.5(0.5)^3}\) 
3. \(\frac{3\times3}{0.5(0.5)^3}\) 
4. None of these 

For the equilibrium of the reaction, HgO(s) $\stackrel{}{\rightleftharpoons }$ Hg(g) + $\frac{1}{2}$O₂(g), K_P for the reaction at a total pressure of "P" will be:

Ionisation constant of HA (weak acid) and BOH (weak base) are 3.0 x 10^–7 each at 298K. The percent degree of hydrolysis of BA at the dilution of 10L is :
1. 25
2. 50
3. 75
4. 40

For the reaction,
${\mathrm{NH}}_2{\mathrm{COONH}}_4\left(\mathrm{s}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$, the
equilibrium pressure is 15 atmosphere. The
value of K_p is
1. 15 atm³
2. 50 atm³
3. 500 atm³
4. 100 atm³