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

564.

The strongest Bronsted base is :

• HCl${\mathrm{O}}_2^{-}$

• HClO^-

• HCl${\mathrm{O}}_3^{-}$

• HClO₄

The characteristic ion of an acid in an aqueous solution is :

• H⁺

• ${\mathrm{H}}_2^{+}$

• H₃O⁺

• H₄O⁺

Assertion : Heat of neutralisation for both H₂SO₄ and HCl with NaOH is 53.7 kJ mol^-1.

Reason : Both HCl and H₂SO₄ are strong acids.

• 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 solubility of AgCl is 1.435 g/L. What will be the solubility product ?

• 10^-4

• 0.01

• 0.001

• 0.001

2X + 2Y $\mathrm{\to }$ 2Z

The equilibrium constant for the above reaction :

• $\frac{\left[2\mathrm{X}\right]\left[2\mathrm{Y}\right]}{\left[2\mathrm{Z}\right]}$

• $\frac{\left[\mathrm{X}\right]\left[\mathrm{Y}\right]}{\left[\mathrm{Z}\right]}$

• $\frac{[\mathrm{Z}{]}^2}{\left[\mathrm{X}{]}^2\right[\mathrm{Y}{]}^2}$

• $\frac{[\mathrm{Z}{]}^2}{\left[\mathrm{X}\right]\left[\mathrm{Y}\right]}$

The solubility product for XY is :

• s²

• 2s

• 4s²

• 2s

In a reversible reaction ifthe concentration of reactants and products are doubled , the value of K_c will be :

• half of the initial value

• double of initial value

• one fourth of the initial value

• same the initial value