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The conjugate base of H₃BO₃ is:
1. $\mathrm{B}(\mathrm{OH}{)}_4^{-}$                                     
2. ${\mathrm{H}}_2{\mathrm{BO}}_3^{-}$
3. ${\mathrm{HBO}}_3^{2-}$                                       
4. ${\mathrm{H}}_4{\mathrm{BO}}_3^{+}$

Given a system: $A\left(\mathrm{s}\right)\stackrel{ }{\rightleftharpoons }2B\left(\mathrm{g}\right) + 3C\left(\mathrm{g}\right).$ 
If the concentration of C at eqilibrium is increased by a factor 2, it will cause the eqilibrium concentration of B to change to:
1. two times of its original value
2. one half of its original value
3. 2$\sqrt{2}$ times of its original value
4. $\frac{1}{2\sqrt{2}}$ times of its original value

Ionisation constant of CH₃COOH is 1.7 X 10^-5 and concentration of H⁺ ions is 3.4 X 10^-4.Then, find out initial concentration of CH₃COOH molecules.            
1. 3.4 X 10^-4 
2. 3.4 X 10^-3
3. 6.8 X 10^-4
4. 6.8 X 10^-3
 

The formation of phosgene is represented as,
            CO + Cl₂ $\rightleftharpoons$COCl₂
The reaction is carried out in 500 mL flask. At equilibrium o.3 mole of phosgene, 0.1 mole of CO and 0.1 mole of Cl₂ are present. The equilibrium constant of the reaction is:
1. 30                     
2. 15
3. 5                       
4. 3

The reaction quotient (Q) for the reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right) + 3{\mathrm{H}}_2\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons }2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ is given by 
$\mathrm{Q}=\frac{{\left[{\mathrm{NH}}_3\right]}^2}{\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\right]}^3}$ The reaction will proceed towards the right side, if    
1. Q>K_c
2. Q=0
3. Q=K_c
4. Q<K_c

The value of equilibrium constant of the reaction,$\mathrm{HI}\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons }\frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right) + \frac{1}{2}{\mathrm{I}}_2\left(\mathrm{g}\right) \mathrm{is} 8.0.$
The equilibrium constant of the reaction, ${\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{I}}_2\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons 2\mathrm{HI}\left(\mathrm{g}\right)}$ wiill be [2008]
1. $\frac{1}{16}$ 
2. $\frac{1}{64}$
3. 16
4. $\frac{1}{8}$

Which salt undergoes hydrolysis?
1. CH₃COONa                                     
2. KNO₃
3. NaCl                                               
4. K₂SO₄

The hydrolysis of the salt of a strong acid and a weak base is called:
1. Anionic hydrolysis
2. Cationic hydrolysis
3. Amphoteric hydrolysis
4. None of the above

For the reaction, A+B $\rightleftharpoons$3C at 25$°$ C, a 3 litre vessel contains 1, 2, and 4 mole of A, B and C respectively. If K_c for the reaction is 10, then the reaction will proceed in:
1. forward direction                           
2. backward direction
3. in either direction                           
4. in equilibrium

Which of the following is most soluble in water?
1. MnS (K_sp = 8x10^-37)         
2. ZnS (K_sp = 7x10^-16)
3. Bi₂S₃ (K_sp = 1x10^-70)       
4. Ag₂S (K_sp = 6x10^-51)

The compound that does not act as Lewis acid is:
1. AlCl₃                                           
2. BF₃
3. NH₃                                             
4. FeCl₃

The values of K_p1 and K_p2 for the reactions
$\mathrm{X}\rightleftharpoons \mathrm{Y} + \mathrm{Z} ........\left(\mathrm{i}\right)$
$\mathrm{and} \mathrm{A}\rightleftharpoons 2\mathrm{B} .........\left(\mathrm{ii}\right)$
are in ratio of 9:1, if degree of dissociation of X and A be equal, then total pressure at equilibrium (i) and (ii) are in the ratio 
1. 3:1
2. 1:9
3. 36:1
4. 1:1

For NH₄HS(s) $\rightleftharpoons$NH₃ (g) + H₂S(g), the observed pressure for reaction mixture in equilibrium is 1.12 atm at 106$°$C. The value of K_p for the reaction is:
1. 3.136 atm²                           
2. 0.3136 atm²
3. 31.36 atm²                           
4. 6.98 atm²

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$\frac{\left[\mathrm{Acid}\right]}{[\mathrm{Conjugate} \mathrm{Base}]}$

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

The molecule that is least likely to act as a Lewis base is:     
1. CO         
2. \(F^{-}\)         
3. AlCl₃      
4. PF₃

The ionisation constant of ammonium hydroxide is 1.77 x 10^-5 at 298 K. Hydrolysis constant of ammonium chloride is
1. 5.65 x 10^-10                     
2. 6.50 x 10^-12
3. 5.65 x 10^-13                     
4. 5.65 x 10^-12

For a given solution pH = 6.9 at 60$°$C, where K_w=10^-12. The solution is:
1. acidic                                         
2. basic
3. neutral                                         
4. unpredictable

The stronger Bronsted based is:
1. ClO^-               
2. Cl${\mathrm{O}}_2^{-}$   
3. Cl${\mathrm{O}}_3^{-}$               
4.  Cl${\mathrm{O}}_4^{-}$ 

The equilibrium, 2SO₂ (g) + O₂ (g) $\rightleftharpoons$2SO₃ (g)
shifts forward if:
1. a catalyst is used
2. an absorbent is used to remove SO₃ as soon as it is formed
3. small amounts of reactants are used
4. none of the above

The pH of blood is maintained by CO₂ by and H₂CO₃ in the body and chemical constituents of blood. This phenomenon is called:
1. colloidal                           
2. buffer action
3. acidic                               
4. salt balance

At temperature T, a compound AB₂ (g) dissociates according to the reaction 2AB₂$\rightleftharpoons$2AB(g) +B₂(g) with a degree of  dissociation x, which is small compared with unity. The expression for K_p, in terms of x and the total pressure P , is:
1. Px³/2                                 
2. Px²/3
3. Px³/3                                 
4. Px²/2

For the reactions,
A $\rightleftharpoons$ B;                                  K_c = 2
B $\rightleftharpoons$ C;                                  K_c = 4
C $\rightleftharpoons$ D;                                  K_c = 6
K_c for the reaction, A $\rightleftharpoons$ D is:
1. (2+4+6)                       
2. (2x4)/6
3. (4x6)/2                         
4. 2x4x6

For the reaction equilibrium,
2NOBr(g) $\rightleftharpoons$2NO(g) + Br₂, if $P_{\mathit{B}{\mathit{r}}_{\mathit{2}}}$ = P/9 at equilibrium and P is total pressure. The ratio of K_p/P is equal to:
1. 1/9               
2. 1/81
3. 1/27               
4. 1/3

Which of the following salts will give the highest pH in the water?                   
1. KCl           
2. NaCl         
3. Na₂CO₃     
4. CuSO₄

An aqueous solution of which salt has the lowest pH?
1. NaOH                 
2. NH₄Cl
3. Na₂CO₃             
4. NaCl

 The following equilibria are given
 N₂ + 3H₂ $\rightleftharpoons$ 2NH₃,      K₁
N₂ + O₂ $\rightleftharpoons$ 2NO,          K₂
H₂ + $\frac{1}{2}$O₂ $\rightleftharpoons$ H₂O,       K₃
The equilibrium constant of the reaction, 2NH₃ + $\frac{5}{2}$O₂ $\rightleftharpoons$ 2NO + 3H₂O in terms of  K₁, K₂ and K₃ is  
1. $K_{\mathit{1}}{K}_{\mathit{3}}^{\mathit{3}}\mathit{/}{K}_{\mathit{2}}$                       
2. $K_2{K}_{\mathit{3}}^{\mathit{3}}\mathit{/}{K}_1$
3. K₁K₂K₃                            
4. K₁K₂/K₃ 

At a certain temperature, 2HI $\rightleftharpoons$H₂ +I₂ only 50% HI is dissociated at equilibrium. The equilibrium constant is:
1. 1.0                     
2. 3.0                 
3. 0.5               
4. 0.25

In the reaction, PCl₅ $\rightleftharpoons$PCl₃ + Cl₂, the amounts of PCl₅, PCl_3, and Cl₂ at equilibrium are 2 moles each and the total pressure is 3 atm. The equilibrium constant K_p is: 
1. 1.0 atm                                       
2. 2.0 atm
3. 3.0 atm                                       
4. 6.0 atm

On addition of inert gas at constant volume to the reaction, N₂ + 3H₂$\rightleftharpoons$2NH₃ at  equilibrium:
1. the reaction halts
2. forward reaction is favored
3. the reaction remains unaffected
4. backward reaction is favored

In which of the following case reaction goes farthest to completion?
1. K=10³                                         
2. K=10^-2
3. K=10                                           
4. K=10⁰

For the reversible reaction,
N₂ (g) + 3H₂(g) $\rightleftharpoons$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 decreassing temperature
 

The strongest acid among the following is:          
1. H₂SO_{4           
2.} HClO₃       
3. HClO₄         
4. H₂SO₃ 

The conjugate acid of NH₂^- is                           
1. N₂H₄   
2. N${\mathrm{H}}_4^{+}$   
3. NH₄OH   
4. NH₃

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

The amount of CaC₂O₄ (molecular weight =128) will dissolve in distilled water to make 1 liter of a saturated solution is: 
[K_sp (CaC₂O₄) = 2.5 x 10^-9 ]
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
$\left(1\right) {\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\alpha }}^2}{(1-\mathrm{\alpha })}$
$\left(2\right) \mathrm{Ka} = {\mathrm{C\alpha }}^2 \mathrm{if} \mathrm{\alpha }\to 0$
$\left(3\right) {\mathrm{K}}_{\mathrm{a}} = \frac{{\mathrm{C\lambda }}^2}{{\mathrm{\lambda }}^2({\mathrm{\lambda }}^2-\mathrm{\lambda })}$
$\left(4\right) \mathrm{All} \mathrm{of} \mathrm{the} \mathrm{above}$

The molecule that is least likely to behave as Lewis base is: 
1. NH₃
2. BF₃
3. OH^-
4. H₂O

K_c and K_p are not equal for a reaction given below:
1. 2NO(g) $\rightleftharpoons$N₂(g) + O₂(g)
2. SO₂(g) + NO₂(g) $\rightleftharpoons$SO₃(g) + NO(g)
3. H₂(g) + I₂(g) $\rightleftharpoons$2HI(g)
4. 2C(s) + O₂(g) $\rightleftharpoons$2CO₂(g)

Which one of the following molecular hydrides acts as a Lewis acid?
1. NH₃         
2. H₂O         
3. B₂H₆           
4. CH₄

If the concentration of OH^- ions in the reaction
Fe(OH)³ (s) $\rightleftharpoons$Fe³⁺ (aq) + 3OH^-(aq) is decreased to 1/4 times, then equilibrium concentration of Fe³⁺ will increase by
(a) 8 times                            (b) 16 times
(c) 64 times                          (d) 4 times

The pOH of a solution at 25$°$C that contains 1 x 10^-10 M of hydronium ions is:  
1. 7.00                               
2. 4.00
3. 9.00                                 
4. 1.00

At a certain temperature the following equilibrium is established, CO(g) + N0₂(g) $\stackrel{}{\rightleftharpoons }$ CO₂(g)+ NO(g)One mole of each of the four gas is mixed in one litre container and the reaction is allowed to reach equilibrium state. When excess of baryta water (Ba(OH)₂) is added to the equilibrium mixture, the weight of white ppt (BaCO₃) obtained is 236.4 gm. The equilibrium constant K_c of the reaction is (Ba = 137)
(1) 1.2
(2) 2.25
(3) 2.1
(4) 3.6