0.01 moles of a weak acid HA (Ka = 2.0 *10^-6) is dissolved in 1.0 L of 0.1 M HCl solution. The degree of dissociation of HA is _______ *10^-5. (Round off to the nearest integer).
[Neglect volume change on adding HA. Assume degree of dissociation <<1]

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