At 25$°$C, the dissociation constant of a base, BOH is 1.0 x 10^-12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be                                     

1. 2.0 x 10^-6 mol L^-1             

2. 1.0 x 10^-5 mol L^-1 

3. 1.0 x10^-6 mol  L^-1             

4. 1.0 x10^-7 mol L^-1 

The pK_a of acetylsalicylic acid (aspirin) is 3.5. The pH of gastric juice in the human stomach is about 2-3 and the pH in the small intestine is about 8. Aspirin will be:

1. Unionized in the small intestine and in the stomach

2. Completely ionized in the small intestine and in the stomach

3. Ionized in the stomach and almost unionized in the small intestine

4. Ionized in the small intestine and almost unionized in the stomach

What is [H⁺] in mol/L of a solution that is 0.20 M in CH₃COONa and 0.10 M in CH₃COOH?

(K_a for CH₃COOH = 1.8 x 10^-5)       

1. 3.5x10^-4           

2. 1.1x10^-5

3. 1.8x10^-5           

4. 9.0x10^-6

The hydrolysis of the salt of a strong acid and a weak base is called:

1. Anionic hydrolysis

2. Cationic hydrolysis

3. Amphoteric hydrolysis

4. None of the above

For the reaction, A+B $\rightleftharpoons$3C at 25$°$ C, a 3 litre vessel contains 1, 2, and 4 mole of A, B and C respectively. If K_c for the reaction is 10, then the reaction will proceed in:

1. forward direction                           

2. backward direction

3. in either direction                           

4. in equilibrium

If K₁ and K₂ are the respective equilibrium constants for the two reactions,

       XeF₆(g) + H₂O(g) $\rightleftharpoons$XeOF₄(g) + 2HF(g)

       XeO₄(g) + XeF₆(g) $\rightleftharpoons$XeOF₄(g) + XeO₃F₂ (g)

The equilibrium constant for the reaction,

       XeO₄(g) + 2HF(g) $\rightleftharpoons$  XeO₃F₂(g) + H₂O(g) is:

1. K₁K₂                                           

2.  K₁/$K_{\mathit{2}}^{\mathit{2}}$

3. K₂/K₁                                         

4. K₁/K₂

The pH of 0.1M soution of the folowing salts increases in the order:

1. NaCl < NH₄Cl < NaCN < HCl

2. HCl < NH₄Cl < NaCl < NaCN

3. NaCN < NH₄Cl < NaCl < HCl

4. HCl < NaCl < NaCN < NH₄Cl 

Three reactions involving ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ are given below:

(i) H₃PO₄ + H₂O $\to$H₃O⁺ + ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$

(ii) ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ + H₂O $\to$${\mathrm{HPO}}_4^{2-}$ + H₃O⁺

(iii) ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ + OH^- $\to$H₃PO₄ +O^2-

In which of the above does ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ act as an acid?

1. (i) only                                 

2. (ii) only

3. (i) and (ii)                           

4. (iii) only

Which of the following is most soluble in water?

1. MnS (K_sp = 8x10^-37)         

2. ZnS (K_sp = 7x10^-16)

3. Bi₂S₃ (K_sp = 1x10^-70)       

4. Ag₂S (K_sp = 6x10^-51)

The compound that does not act as Lewis acid is:

1. AlCl₃                                           

2. BF₃

3. NH₃                                             

4. FeCl₃