The pH of a buffer solution containing equal molal concentration of a weak base and its chloride (K_b for weak base = 2 x 10^-5) is 

• 5

• 9

• 4.7

• 9.3

Consider the following equilibrium in a closed container

        ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$

At a fixed temperature, the volume of the reaction container is halved. For this change which of the following statement holds true regarding the equilibrium constant (K_p) and degree of dissociation ($\mathrm{\alpha }$)?

• Neither K_P nor $\mathrm{\alpha }$ changes

• Both K_p and $\mathrm{\alpha }$ changes

• K_p changes but $\mathrm{\alpha }$ does not

• K_p does not change but $\mathrm{\alpha }$ changes

Conjugate acid ${\mathrm{S}}_2{\mathrm{O}}_8^{2-}$

• H₂S₂O₈

• H₂SO₄

• HS₂${\mathrm{O}}_8^{-}$

• HS${\mathrm{O}}_4^{-}$

The equilibrium constant of a reaction is 300. If the volume of reaction flask is tripled, the equilibrium constant is

• 300

• 600

• 900

• 100

A 0.01 M ammonia solution is 5% ionised, its pH will be

• 11.80

• 10.69

• 7.22

• 12.24

The pH of a 10^-8 molar solution of HCl in water is

• 8

• between 7 and 8

• between 6 and 7

• None of these 

The solubility of AgCl is 1 x 10^-5 mol/L. Its solubility in 0.1 molar sodium chloride solution is

• $1 \times {10}^{-10}$

• $1 \times {10}^{-5}$

• $1 \times {10}^{-9}$

• $1 \times {10}^{-4}$

When ammonium chloride is added to ammonia solution, the pH of the resulting solution will be

• increased

• seven

• decreased

• unchanged

Calculate pH of a buffer prepared by adding 10 mL of 0.10 M acetic acid to 20 mL of 0.1 M sodium acetate [ pK_a (CH₃COOH) = 4.74 ]

• 3.00

• 4.44

• 4.74

• 5.04

The degree of dissociation of a 0.01 M weak acid is 10^-3. Its pOH is

• 5

• 3

• 9

• 11