What is [NH$$_{4}^+$$] in a solution that is 0.02 M NH₃ 0.01 M KOH ? [K_b(NH₃) = 1.8 $$\times$$ 10^$$-$$5]

For an isomerisation reaction A $$\rightleftharpoons$$ B, the temperature dependence of equilibrium constant is given by

log_e K = 4.0 $$-$$ $$\frac{2000}{T}$$

The value of $$\Delta$$S$$^\circ$$ at Hook is, therefore

1.1 mole of A mixed with 2.2 moles of B and the mixture is kept in a 1 L flask and the equilibrium, A + 2B $$\rightleftharpoons$$ 2C + D is reached. If at equilibrium 0.2 mole of C is formed then the value of K_c will be

Sulphuric acid is a dibasic acid. It ionises in two stages and hence has two dissociation constants K_a1 and K_a2. Which of the following is the correct observation regarding K_a1 and K_a2 ?