The solubility of AgCl (s) with solubility product 1.6 x 10^-10 in 0.1 M NaCl solution would be

(1) 1.26 x 10^-5 M               

(2) 1.6 x 10^-9 M

(3) 1.6 x 10^-11 M               

(4) zero

Boric acid is an  acid because its molecule

(1) contains replaceable H⁺ ion

(2) gives up a proton

(3) accepts OH^- from water releasing proton

(4) combines with proton from water molecule

Which of the following fluoro-compounds is most likely to behave as a Lewis base?
(1) BF₃

(2) PF₃

(3) CF₄

(4) SiF₄

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