Among the following the strongest acid is

• CH₃COOH

• C₆H₅COOH

• m-CH₃OC₆H₄COOH

• p-CH₃OC₆H₄COOH

Among the following the weakest base is

• C₆H₅CH₂NH₂

• C₆H₅CH₂NHCH₃

• O₂NCH₂NH₂

• CH₃NHCHO

What is the pH of 0.01 M glycine solution? For glycine ${\mathrm{K}}_{\mathrm{a}1 }= 4.5 \times {10}^{-3} \mathrm{and} {\mathrm{K}}_{\mathrm{a}2 }= 1.7 \times {10}^{-10 } \mathrm{at} 298\mathrm{K}$?

• 3

• 10

• 6.1

• 7.2

In which of the following acid-base titration, pH is greater than 8 at equivalence point?

• Acetic acid versus ammonia

• Acetic acid versus sodium hydroxide

• Hydrochloric acid versus ammonia

• Hydrochloric acid versus sodium hydroxide

Which of the following is strongest Bronsted base?

• ClO-

• ClO₂^-

• ClO₃^-

• ClO₄^-

226.

When the temperature of reactions will increase then the effect on pH value will

• increase

• decrease

• first increases then decreases

• remains same.

Consider the following salts : NaCl, HgCl₂, Hg₂Cl₂, CuCl₂, CuCl and AgCl. Identify the correct set of insoluble salts in water.

• Hg₂Cl₂, CuCl, AgCl

• Hg₂Cl, CuCl, AgCl

• Hg₂Cl₂, CuCl₂, AgCl

• Hg₂Cl₂, CuCl, NaCl

The pH of aqueous solution ofammonium formate is (pK_a of HCOOH = 3.8 and pK_b of NH₃= 4.8)

• 7

• 6.0

• 6.5

• 8.9

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