The equilibrium constant for the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)$ is 4 X 10^-4 at 200K. In the presence of a catalyst, the equilibrium is attained 10 times faster. Therefore, the equilibrium constant in presence of the catalyst at 200K is

1. 4 X 10^-3

2. 4 X 10^-4

3. 4 X 10^-5 

4. None of these

For the given reaction, the degree of dissociation of B was found to be 20% at 300 K and 24% at 500K.
\(2 \mathrm{~A}(\mathrm{~s})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+2 \mathrm{D}(\mathrm{s})+\mathrm{E}(\mathrm{s})\)

The rate of backward reaction:

The pH of 0.1 M solution of anilium chloride is (K_a of ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_3^{+}$ = 10^-6)

(1) 3.5

(2) 3

(3) 4.5

(4) none of these

1L of an aqueous solution contains 0.15mole of CH₃COOH (pKa = 4.8) and 0.15 mole of CH₃COONa. After the addition of 0.05 mole of solid NaOH to this solution, the pH will be

(1) 4.5

(2) 4.8

(3) 5.1

(4) 5.4

In the following reaction

${\mathrm{HC}}_2{\mathrm{O}}_4^{-} + {\mathrm{PO}}_4^{3-} \rightleftharpoons {\mathrm{HPO}}_4^{2-} + {\mathrm{C}}_2{\mathrm{O}}_4^{2-}$ 

Which are the two Bronsted bases ?

1. ${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4^{-} \mathrm{and} {\mathrm{PO}}_4^{3-}$

2. ${\mathrm{HPO}}_4^{2-} \mathrm{and} {\mathrm{C}}_2{\mathrm{O}}_4^{2-}$

3. ${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4^{-} \mathrm{and} {\mathrm{HPO}}_4^{-2}$

4. ${\mathrm{PO}}_4^{3-} \mathrm{and} {\mathrm{C}}_2{\mathrm{O}}_4^{2-}$

Percentage ionisation of water at certain temperature is 3.6 X 10^-7%, Calculate K_w and pH of water.

1. 10^-14, pH = 6.7

2. 4 X 10^-14, pH=6.7

3. 2X 10^-14, pH=7

4. 10^-14, pH=7

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. 3.76                 

4. 4.50

1 litre solution of pH =4 (solution of a strong acid) is added to the 7/3 litre of water. What is the pH of resulting solution. (Log 3 = 0.48)

1. 4

2. 4.48

3. 4.52

4. 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

K_b for a monoacidic base whose 0.10 M solution has a pH of 10.48

1. 9 X 10^-6

2. 9 X 10^-9

3. 9 X 10^-7

4. 3 X 10^-7