For a given solution pH = 6.9 at 60$°$C, where K_w=10^-12. The solution is:

(1) acidic                                           

(2) basic

(3) neutral                                         

(4) unpredictable

The stronger Bronsted based is:

(a) ClO^-                (b) Cl${\mathrm{O}}_2^{-}$   

(c) Cl${\mathrm{O}}_3^{-}$               (d)  Cl${\mathrm{O}}_4^{-}$ 

The equilibrium, 2SO₂ (g) + O₂ (g) $\rightleftharpoons$2SO₃ (g)

shifts forward if:

(1) a catalyst is used

(2) an absorbent is used to remove SO₃ as soon as it is formed

(3) small amounts of reactants are used

(4) none of the above

The pH of blood is maintained by CO₂ by and H₂CO₃ in the body and chemical constituents of blood. This phenomenon is called:

(a) colloidal                            (b) buffer action

(c) acidic                                (d) salt balance

At temperature T, a compound AB₂ (g) dissociates according to the reaction 2AB₂$\rightleftharpoons$2AB(g) +B₂(g) with a degree of dissociation x, which is small compared with unity. The expression for K_p, in terms of x and the total pressure P , is:

(1) Px³/2

(2) Px²/3

(3) Px³/3

(4) Px²/2

For the reactions,

A $\rightleftharpoons$ B;                                  K_c = 2

B $\rightleftharpoons$ C;                                  K_c = 4

C $\rightleftharpoons$ D;                                  K_c = 6

K_c for the reaction, A $\rightleftharpoons$ D is:

(a) (2+4+6)                       (b) (2x4)/6

(c) (4x6)/2                         (d) 2x4x6

Which of the following salts will give highest pH in water?                   

1. KCl           

2. NaCl         

3. Na₂CO₃     

4. CuSO₄

Aqueous solution of which salt has the lowest pH?

(1) NaOH                 

(2) NH₄Cl

(3) Na₂CO₃               

(4) NaCl

 The following equilibria are given

 N₂ + 3H₂ $\rightleftharpoons$ 2NH₃,      K₁

N₂ + O₂ $\rightleftharpoons$ 2NO,          K₂

H₂ + $\frac{1}{2}$O₂ $\rightleftharpoons$ H₂O,       K₃

The equilibrium constant of the reaction, 2NH₃ + $\frac{5}{2}$O₂ $\rightleftharpoons$ 2NO + 3H₂O in terms of  K₁, K₂ and K₃ is  

(1) $K_{\mathit{1}}{K}_{\mathit{3}}^{\mathit{3}}\mathit{/}{K}_{\mathit{2}}$                         

(2) $K_2{K}_{\mathit{3}}^{\mathit{3}}\mathit{/}{K}_1$

(3) K₁K₂K₃                            

(4) K₁K₂/K₃ 

At a certain temperature, 2HI $\rightleftharpoons$H₂ +I₂ only 50% HI is dissociated at equilibrium. The equilibrium constant is:

(a) 1.0                     (b) 3.0                 (c) 0.5               (d)   0.25