K_a1 , K_a2 and K_a3 are the respective ionisation constants for the following reactions.

H₂S $\mathit{}\to$   H⁺ + HS

HS^–  $\mathit{}\to$ H⁺ + S²

 H₂S $\mathit{}\to$ 2H⁺ + S²

The correct relationship between is K_a1 , K_a2 and K_a3

1. K_a3= K_a1 * K_a2
2. K_a3= K_a1 + K_a2
3. K_a3= K_a1 – K_a2
4. K_a3= K_a1 / K_a2

pH for 0.01 M NaOH solution is

K_p for the given reaction is (36 × 10^–2atm^–1) Find out K_c (M^–1) (nearest integer).

(2NO₂ N₂O₄)

(R=0.0821 atm. L/mol. K)

(T = 300K)

A(g) ->B(g) + $\frac{1}{2}$ <!-- [if gte mso 9]><xml> </xml><![endif]-->C(g)

In the about reaction, the correct relation between K_p, a and equilibrium pressure (p) is

Which of the following equilibrium will shift in forward direction on applying pressure?

The ionization constant of HCN is 4.5 × 10^–10 at 298 K. Hydrolysis constant of sodium cyanide is