For a reversible reaction, if the concentrations of the reactants are doubled, the equilibrium constant will be                                                                                       

Which of these is least likely to act as a Lewis base?             

For a hypothetical equilibrium:

$4\mathrm{A} + 5\mathrm{B} \stackrel{ }{\rightleftharpoons } 4\mathrm{x} + 6\mathrm{y}$; the equilibrium constant K_c has the unit:

Calculate the pOH of a solution at 25$°$C that contains 1x10^-10 M of hydronium ion.        

Solubility of MX₂ type electrolytes is 0.5x10^-4 mol/L, then the K_sp of electrolytes is :         

For which reaction does the equilibrium constant depend on the units of concentration?

A physician wishes to prepare a buffer solution at pH=3.58 that efficiently resist changes in pH yet contains only small concetration of the buffering agents. Which one of the following weak acid together with its sodium salt would be best to use ?           [1997]

One mole of ethyl alcohol was treated with one mole of acetic acid at 25$°$C. 2/3 of the acid changes into ester at equilibrium. The equilibrium constant for the reaction will be:

For a given solution pH = 6.9 at 60$°$C, where K_w=10^-12. The solution is:

In a buffer solution containing equal concentration of B^- and H B, the K_b for B^- is 10^-10. The pH of buffer solution is 

Aqueous solution of acetic acid contains                                                   

The equilibrium, 2SO₂ (g) + O₂ (g) $\rightleftharpoons$2SO₃ (g)

shifts forward if:

The pH of blood is maintained by CO₂ by and H₂CO₃ in the body and chemical constituents of blood. This phenomenon is called:

Incorrect statement among the following is: 

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:

The rate constants for forward and backward reaction of hydrolysis is ester are 1.1 x10^-2 and 1.5x10^-3 per minute. Equilibrium constant for the reaction,                                                              

 CH₃COOC₂H₅ + H⁺ $\rightleftharpoons$ CH₃COOH + C₂H₅OH is

What happens to pH of a solution when NH₄Cl crystal is added to a dilute solution of NH₄OH?

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:

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:

In the system, CaF₂(s) $\rightleftharpoons$Ca²⁺ (aq) + 2F^-(aq), increasing the concentration of Ca²⁺ ions 4 times will cause the equilibrium concentration of F^- ions to change to:

The addition of HCl does not suppress the ionization of:

KMnO₄ can be prepared from K₂MnO₄ as per reaction,

 $3{\mathrm{MnO}}_4^{2-} + 2{\mathrm{H}}_2\mathrm{O} \rightleftharpoons 2{\mathrm{MnO}}_4^{-} + {\mathrm{MnO}}_2 + 4{\mathrm{OH}}^{-}$

The reaction can go to completion by removing OH^- ions by adding             

The rate of reaction depends upon the                    

The increasing order of basic strength of Cl^-, ${\mathrm{CO}}_3^{2-}$, CH₃COO^-, OH^-, F^- is:

If the pressure is applied to the following equilibrium, Liquid $\rightleftharpoons$ Vapour. The boiling temperature of the liquid:

Which of the following statements is not true?

In which of the following will the solubility of AgCl be the minimum?

Which of the following salts will give the highest pH in the water?                   

An aqueous solution of which salt has the lowest pH?

The value of $∆$H for the reaction,

   X₂(g) + 4Y₂(g) $\rightleftharpoons$2XY₄ (g)

is less than zero. Formulation of XY₄(g) will be favored at                           

Salting out the action of soap is based on:

Which is not an acid salt?

 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  

The pK_a for acid A is greater than pK_a for acid B. The strong acid is:

At a certain temperature, 2HI $\rightleftharpoons$H₂ +I₂ only 50% HI is dissociated at equilibrium. The equilibrium constant is:

A solution of FeCl₃ in water acts as acidic due to:

Which of the following solution does not act as buffer?

Which equilibrium can be described as Lewis acid-base reaction but not Bronsted acid-base reaction?

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: 

An aqueous solution of hydrogen sulphide shows the equilibrium,

           H₂S $\rightleftharpoons$H⁺ + HS^-

If dilute hydrochloic acid is added to an aqueous solution of hydrogen sulphide without any change in temperature, then:

When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because:

The aqueous solution of a salt is alkaline. This shows that salt is made from:

An aqueous solution of NaHSO₃ is-

40% of a racemic mixture of 0.2 moles of N₂ and 0.6 moles of H₂ react to give NH₃ according to the equation, N₂ (g) + H₂(g)$\rightleftharpoons$2NH₃ (g) at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases is:

On addition of inert gas at constant volume to the reaction, N₂ + 3H₂$\rightleftharpoons$2NH₃ at  equilibrium:

In which of the following case reaction goes farthest to completion?

For the reversible reaction,

N₂ (g) + 3H₂(g) $\rightleftharpoons$2NH₃ (g) + heat

 the equilibrium shifts in forward direction                                   

The correct representation for the solubility product constant of Ag₂CrO₄ is:

pH of a saturated solution of Ba(OH)₂ is 12. The value of solubility product K_sp of Ba(OH)₂ is

At a given temperature the K_c for the reaction,

PCl₅ (g) $\rightleftharpoons$ PCl₃ (g) + Cl₂ (g) is 2.4 x10^-3. At the same temperature, the K_c for the reaction

PCl₃ (g) + Cl₂ (g) $\rightleftharpoons$ PCl₅ (g)  is :