The pH value of decinormal solution of NH₄OH which is 20% ionised is

• 12.95

• 12.30

• 14.70

• 13.30

For the reaction,
2SO₂ (g) + O₂ (g) $\rightleftharpoons$ 2SO₃ (g) at 300 K, the value of $∆$G° is -690.9 R. The equilibrium constant value for the reaction at that temperature is (R is gas constant)

• 10 atm^-1

• 10 atm

• 10

• 1

In which of the following reaction K_p> K_c ?

• ${\mathrm{PCl}}_3 + {\mathrm{Cl}}_3 \to {\mathrm{PCl}}_5$

• ${\mathrm{H}}_2+{\mathrm{I}}_2 \to 2\mathrm{HI}$

• $2{\mathrm{SO}}_3 \to {\mathrm{O}}_2 + 2{\mathrm{SO}}_2$

• ${\mathrm{N}}_2+ 3{\mathrm{H}}_2 \to 2{\mathrm{NH}}_3$

The ratio of volumes of CH₃COOH 0.1 (N) to CH₃COONa 0.1 (N) required to prepare a buffer solution of pH 5.74 is (Given pK_a of CH₃COOH is 4.74)

• 10 : 1

• 5 : 1

• 1 : 5

• 1 : 10

Which of the following is a characteristic of a reversible reaction?

• It never proceeds to completion

• It can be influenced by a catalyst

• It proceeds only in forward direction

• Number of moles of reactants and products are equal.

The equilibrium constant of a reaction is 300. If the volume of a reaction flask is trippled, the equilibrium constant will be

• 300

• 100

• 600

• 150

1007.

A solution with pH = 2 is more acidic than one with a pH =6, by a factor of

• 4000

• 5000

• 8000

• 10,000

Within the list shown below, the correct pair of structures of alanine in pH ranges 2-4 and 9-11 is

I. H₃N⁺-CH(CH₃)CO₂H
II. H₂N-CH(CH₃)CO${}_2^{-}$
III. H₃N⁺-CH(CH₃)CO${}_2^{-}$
IV.H₂N-CH(CH₃)CO₂H

• I and II

• I and III

• II and III

• III and IV

Assertion: Relative strength of acids can be known by knowing the value of dissociation constant.

Reason : It gives the value of H dissolved in solution.

• If both Assertion and Reason are true and Reason is the correct explanation of Assertion.

• If both Assertion and Reason are true but Reason is not the correct explanation of Assertion.

• If Assertion is true but Reason is false.

• If Assertion is false but Reason is true.

A 100 mL 0.1 = (M) solution of ammonium acetate is diluted by adding 100 mL of water. The pH of the resulting solution will be (pK_a of acetic acid is nearly equal to pK_b of NH₄OH).

• 4.9

• 5.0

• 7.0

• 10.0