In the equilibrium reaction 2HI (g) $\rightleftharpoons$ H₂ + I₂ which of the following expressions is true?

• K_p = K_c

• K_c = 2K_p

• K_p > K_c

• K_c = K_p (RT)²

Strongest Bronsted base among the following anions is:

• ClO^-

• ClO${}_2^{-}$

• ClO${}_3^{-}$

• ClO${}_4^{-}$

1.1 moles of A and 2.2 moles of B are mixed in a container of one litre volume to obtain the equilibrium A + 2B $\rightleftharpoons$ 2C + D.

At equilibrium 0.2 moles of C are formed. The equilibrium constant for the above reaction is

• 0.001

• 0.002

• 0.003

• 0.004

In which solution/ solvent the solubility of AgCl is minimum?

• 0.01 M NaCl

• 0.01 M CaCl₂

• Pure water

• 0.001 M AgNO₃

Which one of the following salts gives an acidic solution in water?

• CH₃COONa

• NH₄Cl

• NaCl

• CH₃COONH₄

Which of the following exhibits highest solubility in water?

• NH₃

• PH₃

• AsH₃

• SbH₃

587.

The chemical decomposition of XY₂ occurs as ${\mathrm{XY}}_2\left(\mathrm{g}\right) \rightleftharpoons \mathrm{XY} \left(\mathrm{g}\right) + \mathrm{Y}\left(\mathrm{g}\right)$. The initial vapour pressure of XY₂ is 600 mm of mercury and at equilibrium it is 800 mm of mercury. Find out the value of K for this reaction when the volume of the system remains constant.

• 50

• 100

• 166.6

• 150

The degree of ionisation of decinormal solution of CH₃COOH is 1.3%. If the log of 1.3 is 0.11, the pH of this solution is

• 2.89

• 3.89

• 4.89

• 0.89

A buffer solution is obtained by mixing 10 mL of 1.0M CH₃COOH and 20mL of 0.5M CH₃COONa and it is diluted to 100mL using distilled water. pK_a of CH₃COOH is 4.76. The pH of this buffer solution is 

• 2.76

• 3.76

• 4.76

• 0.76

1.0 L of 1.0 M solution of sodium hydroxide is neutralised by 1.0 L of 1.0 M of methanoic acid. If the heat of formation of water is X, the neutralisation energy of above reaction is

• less than X

• more than X

• equal to X

• None of the above