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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, the degree of dissociation of B was found to be 20% at 300 K and 24% at 500K.
\(2 \mathrm{~A}(\mathrm{~s})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+2 \mathrm{D}(\mathrm{s})+\mathrm{E}(\mathrm{s})\)
The rate of backward reaction:

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