Which is the strongest acid in the following?          

(a) H₂SO₄            (b) HClO₃        (c) HClO₄         (d) H₂SO₃ 

The conjugate acid of NH₂^- is                           

(a) N₂H₄      (b) N${\mathrm{H}}_4^{+}$       (c) NH₄OH        (d) NH₃

A 50 ml solution of strong acid of pH = 1 is mixed with a 50 ml solution of strong acid of pH=2. The pH of the mixture will be nearly:                                                     

(log 5.5 = 0.74)

1. 0.74                   2. 1.26

3. 1.76                   4.  1.5

The pH of a solution obtained by mixing 50ml of 0.4N HCl and 50ml of 0.2M NaOH is:

(1) 13

(2) 12

(3) 1.0

(4) 2.0

In which of the following reaction the value of K_p will be equal to K_c ?

$1. {\mathrm{N}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)$

$2. {\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right) + {\mathrm{Cl}}_2\left(\mathrm{g}\right)$

$3. 2{\mathrm{NH}}_3\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2\left(\mathrm{g}\right) +3{\mathrm{H}}_2\left(\mathrm{g}\right)$

$4. 2{\mathrm{SO}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right)$

$\frac{{\mathrm{K}}_{\mathrm{p}}}{{\mathrm{K}}_{\mathrm{c}}}$ for the gaseous reaction:

$$\begin{gathered} \mathrm{I}. 2\mathrm{A} + 3\mathrm{B} \rightleftharpoons 2\mathrm{C} \\ \mathrm{II}. 2\mathrm{A}\rightleftharpoons 4\mathrm{B} \\ \mathrm{III}. \mathrm{A}+\mathrm{B}+2\mathrm{C} \rightleftharpoons 4\mathrm{D} \end{gathered}$$

Would be respectively:

(1) (RT)^-3, (RT)², (RT)⁰ 

(2) (RT)^-3, (RT)-², (RT)^-1 

(3) (RT)^-3, (RT)², (RT) 

(4) None of the above

How many grams of CaC₂O₄ (molecular weight =128) on dissolving in distilled water will give a saturated solution

[K_sp (CaC₂O₄) = 2.5x10^-9 mol²l^-2

1. 0.0064 g             2. 0.1280 g

3. 0.0128 g             4. 1.2800 g

Ostwald dilution law for weak electrolyte HA can be given as

$\left(1\right) {\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\alpha }}^2}{(1-\mathrm{\alpha })}$
$\left(2\right) \mathrm{Ka} = {\mathrm{C\alpha }}^2 \mathrm{if} \mathrm{\alpha }\to 0$
$\left(3\right) {\mathrm{K}}_{\mathrm{a}} = \frac{{\mathrm{C\lambda }}^2}{{\mathrm{\lambda }}^2({\mathrm{\lambda }}^2-\mathrm{\lambda })}$
$\left(4\right) \mathrm{All} \mathrm{of} \mathrm{the} \mathrm{above}$

If carbon dioxide is 2% dissociated at equilibrium 2CO₂ (g)$\rightleftharpoons$2CO(g) + O₂(g). The mole fraction of CO₂ at equuilibrium is

(1) 1.01/0.98            (2) 0.98/1.01

(3) 0.01/0.98            (4) 0.098/1.01

Which of the following is least likely to behave as Lewis base?
(1) NH₃

(2) BF₃

(3) OH^-

(4) H₂O