The relation for calculating pH of a solution containing weak acid and its salt is:

1. pH = pK_a + log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Acid}\right]}$

2. pH = pK_a - log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Acid}\right]}$

3. pH = pK_a + log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Salt}\right]}$

4. pOH = pK_a - log$\frac{\left[\mathrm{Acid}\right]}{[\mathrm{Conjugate} \mathrm{Base}]}$

The equilibrium constants for the reaction,

A₂ $\rightleftharpoons$2A at 500 K and 700 K are 1x10^-10 and 1x10^-5. The given reaction is                  

(a) exothermic                    (b) slow

(c) endothermic                  (d) fast

1. a,b

2.c,b

3.a,d

4 c,d

For the chemical reaction, $3\mathrm{X}\left(\mathrm{g}\right) + \mathrm{Y}\left(\mathrm{g}\right) \rightleftharpoons {\mathrm{X}}_3\mathrm{Y}\left(\mathrm{g}\right)$;

the amount of X₃Y at equilibrium is affected by :

1. Temperature and pressure

2. Temperature only

3. Pressure only

4. Temperature, pressure and catalyst

H₂S gas when passed through a solution of cations containing HCl precipitates the cations of the second group in qualitative analysis but not those belonging to the fourth group. It is because: 
 

The equilibrium constant Br₂ $\rightleftharpoons$2Br at 500 K and 700 K are 10^-10 and 10^-5 respectively. The reaction is:

(a) endothermic                                  (b) exothermic

(c) fast                                               (d) slow

1. a,b

2.c,b

3.a,d

4 c,d

Solubility of a gas in liquid increases on:

1. Addition of a catalyst

2. Increasing the pressure

3. Decreasing the pressure

4. Increasing the temperature

A solution is called saturated if:

1. ionic concentration product < solubility product

2. ionic concentration product > solubility product

3. ionic concentration product $\ge$ solubility product

4. none of the above

The concentration of [H⁺] and concentration of [OH^-] of a 0.1M aqueous solution of 2% ionised weak monobasic acid is                                                                    

[ionic product of water = 1x 10^-14]

1. 0.02x10^-3 M and 5x10^-11 M

2. 1x10^-3 M and 3x10^-11 M

3. 2x10^-3 M and 5x10^-12 M

4. 3x10^-2 M and 4x10^-13 M

The relation for calculating pH of a weak base is:

1. pH =pK_w -1/2 pK_b + 1/2 logc

2. pH =pK_w +1/2 pK_b - 1/2 logc

3. pH =pK_w -1/2 pK_a + 1/2 logc

4. none of the above

In a closed container of 1 dm³, 8 moles of \(AB_3\)​ gas reach equilibrium following the reaction:
\(2 \mathrm{AB}_3(g) \rightleftharpoons \mathrm{~A}_2(g)+3 \mathrm{~B}_2(g)\)
What is the equilibrium constant when 2 moles of \(A_2\) are observed at equilibrium?

1. 72 mol²L^-2                     

2. 36 mol²L^-2 

3. 3 mol²L^-2                       

4. 27 mol²L^-2