The conjugate base of [Al(H₂O)₃(OH)₃] is:

1. [Al(H₂O)₃(OH)₂]⁺                           

2. [Al(H₂O)₃(OH)₂O]^-

3. [Al(H₂O)₃(OH)₃]^-                           

4.  [Al(H₂O)₂(OH)₄]^-

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 solubility product of Hg₂I₂ is equal to:

1. $\left[{\mathrm{Hg}}_2^{2+}\right]\left[{\mathrm{I}}^{-}\right]$

2. $\left[{\mathrm{Hg}}_{}^{2+}\right]\left[{\mathrm{I}}^{-}\right]$

3. $\left[{\mathrm{Hg}}_2^{2+}\right][{\mathrm{I}}^{-}{]}^2$

4. $\left[{\mathrm{Hg}}_2^{2+}{]}^2\right[{\mathrm{I}}^{-}{]}^2$

Which oxide of nitrogen is the most stable?

1. 2NO₂(g) $\rightleftharpoons$N₂(g) + 2O₂(g);         K=6.7x10¹⁶ mol litre^-1

2. 2NO(g) $\rightleftharpoons$N₂(g) + O₂(g);            K=2.2x10³⁰ mol litre^-1

3. 2N₂O₅(g) $\rightleftharpoons$2N₂(g) + 5O₂(g);      K=1.2x10³⁴ mol^-5 litre^-5

4. 2N₂O(g) $\rightleftharpoons$2N₂(g) + O₂(g);         K=3.5x10³³ mol litre^-1

On adding A to the reaction at equilibrium,  AB(s) $\rightleftharpoons$ A(g) + B(g), the new equilibrium concentration of A becomes double, the equilibrium concentration of B would become:

1. 1/2 of its original value

2. 1/4 of it s original value

3. 1/8 of its original value

4. twice of its original value

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

Given, HF + H₂O$\stackrel{K_{\mathit{a}}}{\to }$H₃O⁺ + F^-

          F^- + H₂O $\stackrel{K_b}{\to }$HF + OH^-

which relation is correct?

1. K_b =K_w                       

2. K_b =1/K_w 

3. K_a x K_b =K_w                 

4.  K_a/K_b = K_w 

The value sf K_p1 and K_p2 for the reactions

              X$\rightleftharpoons$Y+Z                                          ....(1)

   and      A$\rightleftharpoons$2B                                          ......(2)

are in the ratio 9:1. If the degree of dissociation of X and A be equal, then total pressure at equilibrium (1) and (2) are in the ratio:

1. 1:9                                     

2. 36:1

3. 1:1                                     

4. 3:1

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 constants for the reaction,

A₂ $\rightleftharpoons$2A at 500 K and 700 K are 1x10^-10 and 1x10^-5. The given reaction is                  

(a) exothermic                    (b) slow

(c) endothermic                  (d) fast

1. a,b

2.c,b

3.a,d

4 c,d