The equilibrium constant of the following are

${\mathrm{N}}_2+ 3{\mathrm{H}}_2\stackrel{ }{\rightleftharpoons }2{\mathrm{NH}}_3; {\mathrm{K}}_1$
${\mathrm{N}}_2 + {\mathrm{O}}_2 \stackrel{ }{\rightleftharpoons }2\mathrm{NO}; {\mathrm{K}}_2$
${\mathrm{H}}_2 + \frac{1}{2}{\mathrm{O}}_2 \stackrel{ }{\to }{\mathrm{H}}_2\mathrm{O}; {\mathrm{K}}_3$

The equilibrium constant (K) of the reaction

$2{\mathrm{NH}}_3 + \frac{5}{2}{\mathrm{O}}_2 \stackrel{ \mathrm{K} }{\rightleftharpoons }2\mathrm{NO} + 3{\mathrm{H}}_2\mathrm{O},$ will be

(a) ${\mathrm{K}}_1\raisebox{1ex}{${\mathrm{K}}_3^3$}\!\left/ \!\raisebox{-1ex}{${\mathrm{K}}_2$}\right.$

(b) ${\mathrm{K}}_2\raisebox{1ex}{${\mathrm{K}}_3^3$}\!\left/ \!\raisebox{-1ex}{${\mathrm{K}}_1$}\right.$

(c) ${\mathrm{K}}_2\raisebox{1ex}{${\mathrm{K}}_3^{}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{K}}_1$}\right.$

(d) ${\mathrm{K}}_2^3\raisebox{1ex}{${\mathrm{K}}_3^{}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{K}}_1$}\right.$

The concentration of the Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.2 x 10^-4 M. The solubility product of Ag₂C₂O₄ is

1. 2.42 x 10^-8

2. 2.66 x 10^-12

3. 4.5 x 10^-11

4. 5.3 x 10^-12

The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅N⁺H) in a 0.10 M aqueous pyridine solution (K_b for C₅H₅N = 1.7 x 10^-9) is

(1) 0.0060 %                 

(2) 0.013 %

(3) 0.77 %                     

(4) 1.6%

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

Consider the nitration of benzene using mixed conc. H₂SO₄ and HNO₃. If a large amount

of KHSO₄ is added to the mixture, the rate of nitration will be

1. slower 

2. unchanged

3. doubled

4. faster

Consider the following liquid-vapour equilibrium

              Liquid $\rightleftharpoons$Vapour

Which of the following relations is correct?

1. 

2. 

3. 

4.