$K_{a_1},K_{a_2}and{K}_{a_3}$ are the respective ionization constants for the following reaction (a), (b) and (c).

(A) $H_2{C}_2{O}_4?H^{+}+H{C}_2{O}_4^{-}$

(B) $H{C}_2{O}_4^{+}?H^{-}+C_2{O}_4^{2-}$

(C) $H_2{C}_2{O}_4?2H^{+}+C_2{d}_4^{2-}$

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