Chemistry : Equilibrium

If the equilibrium constant of the reaction of weak acid HA with strong base is 10⁹ then pH of 0.l M NaA is :

• 5

• 9

• 7

• 8

Which of the following compounds is the weakest Bronsted base ?

The true statement for the acids of phosphorus, H₃PO₂ H₃PO₃ and H₃PO₄ is

• the order of their acidity is H₃PO₄ > H₃PO₃ > H₃PO₂

• all of them are reducing in nature

• all of them are tribasic acids

• the geometry of phosphorus is tetrahedral in all the three.

Assertion : H₃BO₃ is a weak acid.

Reason : Water extracts the proton of H₃BO₃.

• If both assertion and reason are true and reason is the correct explanation of assertion.

• If both assertion and reason are true but reason is not the correct explanation of assertion.

• If assertion is true but reason is false

• If both assertion and reason are false.

The ionisation percentage of 0.2 M HCN the solution is 0.02%. What will be the value of ionisation constant ?

• 8 x 10^-5

• 8 x 10^-9

• 8 x 10^-7 

• 8 x 10^-3

Which one act as Bronsted acid as well as Bronsted base?

• Cl^-

• OH^-

• HCl

• H₂O

If the pH of HCl soltion is 2 then the molar concentration of this will be :

• 0.01 M

• 2 M

• 0.4 M

• 0.02 M

BF₃ molecule is :

• Lewis base

• Lewis acid

• Neutral

• None of these

NO₂ + $\frac{1}{2}$ O₂ $\rightleftharpoons$ NO₃ .......K₁

2NO₂ + O₂ $\rightleftharpoons$ 2NO₃ ........K₂

For the above reaction the relation between equilibrium constant is :

• K₂ = (K₁)²

• K₂ = $\frac{1}{{\mathrm{K}}_1}$

• K₂ = $\frac{1}{{{\mathrm{K}}_1}^2}$

• K₁ = K₂

The strongest Bronsted base is :

• HCl${\mathrm{O}}_2^{-}$

• HClO^-

• HCl${\mathrm{O}}_3^{-}$

• HClO₄