The pH of a solution of H₂O₂ is 6.0. Some chlorine gas is bubbled into this solution. Which of the following is correct?

• The pH of resultant solution becomes 8.0

• Hydrogen gas is liberated from resultant solution

• The pH of resultant solunon becomes less than 6.0 and oxygen gas is liberated

• Cl₂O is formed in the resultant solution

Which of the following is not a characteristic property of chemical equilibrium ?

• Rate of forward reaction is equal to rate of backward reaction at equilibrium.

• After reaching the chemical equilibrium, the concentrations of reactants and products remain unchanged with time.

• For A (g) $\rightleftharpoons$ B (g), K_c is 10^-2. If this reaction is carried out in the presence of catalyst, the value of K_c decreases.

• After reaching the equilibrium, both forward and backward reactions continue to take place.

50 mL of H₂O is added to 50 mL of 1 × 10^-3 M barium hydroxide solution. What is the pH of the resulting solution ?

• 3.0

• 3.3

• 11.0

• 11.7

In a 500 mL flask, the degree of dissociation of PCl₅ at equilibrium is 40% and the initial amount is 5 moles. The value of equilibrium constant in mol L^-1 for the decomposition of PCl₅ is

• 2.33

• 2.66

• 5.32

• 4.66

Boron halides behave as Lewis acids because of their  .......... nature.

• proton donor

• covalent

• electron deficient

• ionising

Which of the following is not a conjugate acid-base pair?

• ${\mathrm{HPO}}_3^{2-}, {\mathrm{PO}}_3^{3-}$

• ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}, {\mathrm{HPO}}_4^{2-}$

• ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}, {\mathrm{H}}_3{\mathrm{PO}}_4$

• ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}, {\mathrm{PO}}_3^{3-}$

Which one of the following salts give an acidic solution in water?

• CH₃COONa

• NH₄Cl

• NaCl

• CH₃COONH₄

The equilibrium constant for the reaction 

${\mathrm{SO}}_2\left(\mathrm{g}\right)\hspace{0.17em}+ \frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right) \rightleftharpoons {\mathrm{SO}}_3\left(\mathrm{g}\right) \mathrm{is}\hspace{0.17em}5\times {10}^{-2} \mathrm{atm}.$ The equilibnum constant of the reaction $2{\mathrm{SO}}_3\left(\mathrm{g}\right)\hspace{0.17em}\rightleftharpoons 2{\mathrm{SO}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \mathrm{would}\hspace{0.17em}\mathrm{be}.$

• 100 atm

• 200 atm

• 4 × 10² atm

• 6.25 × 10⁴ atm

If the equilibrium constant for the reaction,

${\mathrm{H}}_2\left(\mathrm{g}\right)\hspace{0.17em}+ {\mathrm{I}}_2\left(\mathrm{g}\right) \rightleftharpoons 2\mathrm{HI} \left(\mathrm{g}\right) \mathrm{is} \mathrm{K}$. what is the equilibrium constant of $\mathrm{HI}\left(\mathrm{g}\right) \rightleftharpoons \frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right) +\hspace{0.17em}\frac{1}{2}{\mathrm{I}}_2\left(\mathrm{g}\right) ?$

• 1/K

• √K

• K

• 1/√K

540.

The pH of 0.01 M solution of acetic acid is 5.0. What are the values of [H⁺] and K_a respectively?

• 1 × 10^-5M, 1× 10^-8

• 1 × 10^-5M, 1× 10^-9

• 1 × 10^-4M, 1 × 10^-8

• 1 × 10^-3M, 1 × 10^-8