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 

Calculate the pOH of a solution at 25$°$C that contains 1x10^-10 M of hydronium ion.        

1. 7.00                         

2. 4.00

3. 9.00                         

4. 1.00

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

What happens to pH of a solution when NH₄Cl crystal is added to a dilute solution of NH₄OH?

1. Decreases                                   

2. Increases

3. Remains unaffected                       

4. All of the above

The phenomenon of interaction of anions and cations furnished by an electrolyte with the H⁺ and  OH^- ions of water to produce acidic nature or alkalinity is known as hydrolysis. In hydrolysis:

1. the pH may either increase or decrease

2. all the salts (except those made up with strong acid and base) undergo hydrolysis

3. the variation of pH depends upon the nature of salts as well as on the temperature

4. all of the above