Among the following, the correct order of acidity is

1. HClO < HClO₂ < HClO₃ < HClO₄

2. HClO₂ < HClO < HClO₃ < HCLO₄

3. HClO₄ < HClO2 < HClO < HClO₃

4. HClO₃ < HClO₄ < HClO₂ < HClO

MY and NY₃ , two nearly insoluble salts, have the same Ksp values of 6.2 x 10^-13 at room

temperature. Which statement would be true in regard to MY and NY₃?

1. The molar solubility of MY in water is less than that of NY₃

2. The salts MY and NY₃ are more soluble in 0.5 M KY than in pure water

3. The addition of the salt of KY to solution of MY and NY₃ will have no effect on their

solubilities

4. The molar solubilities of MY and NY₃ in water are identical

The Ksp of Ag₂CrO₄, AgCl, AgBr and Agl are, respectively, 1.1x10^-12, 1.8x10^-10, 5.0x10^-13, and 8.3x10^-17. The salt precipitates that last if the AgNO₃ solution is added to the solution containing equal moles of NaCl, NaBr, Nal and Na₂CrO₄ is -

Which of the following statements is correct for a reversible process in a state of

equilibrium?

1. ΔG = -2.30 RT logK

2. ΔG = 2.30 RT log K

3. ΔG° = -2.30 RT logK

4. ΔG° = 2.30 RT logK

The pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed is:

1. 12.65

2. 2.04

3. 7.01

4. 1.35

Among the following pairs of solution the one which is not an acidic buffer is:

1. HClO₄ and NaClO₄

2. CH₃COOH and CH₃COONa

3. H₂CO₃ and Na₂CO₃

4. H₃PO₄ and Na₃PO₄

For the reversible reaction, N₂(g) + 3H₂(g) — 2NH₃(g) + Heat the equilibrium shifts in

forward direction

1. By increasing the concentration of NH₃(g)

2. By decreasing the pressure

3. By decreasing the concentrations of N₂(g) and H₂(g)

4. By increasing pressure and decreasing temperature

For a given exothermic reaction, K_p and K'_p are the equilibrium constants at temperatures

T₁ and T₂ respectively. Assuming that heat of reaction is constant in a temperature range

between T₁ and T₂, it is readily observed that

1. K_p>K'_p                       

2. K_p<K'_p

3. K_p = K'_p                     

4. K_p = 1/K'_p

Buffer solutions have constant acidity and alkalinity because
1. these give unionised acid or base or base on reaction with added acid or alkali
2. acids and alkalies in these solutions are shielded from attack by other ions
3. they have large excess of H⁺ or OH^- ions
4. they have fixed value of pH

The molecule that is least likely to behave as Lewis base is: 

1. NH₃

2. BF₃

3. OH^-

4. H₂O