Which of the following represents the correct pH of a 10^-7 M HCl in doubly distilled air-free water?

• 6.6990

• 7.0000

• 7.3010

• 6.3980

The solubihty of AgI in NaI solution is less than that in pure water because

• Agl forms complex with Nal

• of common ion effect

• solubility product of AgI less

• the temperature of the solution decreases

403.

Hydrogen ion concentration in mol/L in a solution of pH = 5.4 will be

• 3.98 × 10⁸

• 3.88 × 10⁶

• 3.68 × 10^-6

• 3.98 × 10^-6

XY₂ dissociated as XY₂(g) $\rightleftharpoons$XY(g) + Y (g) When the initial pressure of XY₂ is 600 mm Hg, the total equilibrium pressure is 800 mm Hg. Calculate K for the reaction assuming that the volume of the system remains unchanged.

• 50

• 100

• 166.6

• 400.0

For the following equilibrium, N₂O₄ $\rightleftharpoons$2NO₂ in the gaseous phase, NO₂ is 50% of the total volume when equilibrium is set up. Hence, per cent of dissociation of N₂O₄ is

• 50%

• 25%

• 66.66%

• 33.33%

Of the given anions, the strongest Bronsted base is

• ClO^-

• ClO${}_3^{-}$

• ClO${}_2^{-}$

• ClO${}_4^{-}$

At equilibrium, if K_P = 1, then

• $∆\mathrm{G}°$ > 1

• $∆\mathrm{G}°$ < 1

• $∆\mathrm{G}°$ = 0

• $∆\mathrm{G}°$ = 1

Which of the following is most acidic?

• H₂O

• H₂S

• H₂Se

• H₂Te

1 mL of 0.01 N HCl is added to 999 mL solution of 0.1 N Na₂SO₄. The pH of the resulting solution will

• 2

• 7

• 5

• 1

The equilibrium constants for the reaction,

Br₂ $\rightleftharpoons$ 2Br → 1

at 500 K and 700 K are 1 × 10^-10 and 1 × 10^-5 respectively. The reaction is

• endothermic

• exothermic

• fast

• slow