If Kc is ranging in the range of 10 3 to 10-3; i. e. reactants and products are just in equilibrium.
G 0 = – RT lnK or G 0 = – 2.303RT log K
Factors affecting equilibrium constant:- temperature, pressure, catalyst and molar concentration of reactants and products.
Le Chatelier’ s principle:-
It states that a change in any of the factors that determine the equilibrium conditions of a system will cause the system to change in such a manner so as to reduce or to counteract the effect of the change.
Arrhenius acids are the substances that ionize in water to form H +. Arrhenius bases are the substances that ionize in water to form OH-.
Lewis acids are lone pair( of e-) accepters while Lewis bases are lone pair donators.
Proton donor are acids while proton accepters are bases( Bronsted-Lowry concept).
The acid-base pair that differs only by one proton is called a conjugate acid-base pair. If Brönsted acid is a strong acid then its conjugate base is a weak base and vice versa.
Ionic product of water. Kw = [ H + ][ OH – ] pH =-log [ H + ]; here [ H + ] is molar concentration of hydrogen ion. pH + pOH = 14 pKa + pKb = 14 Ka x Kb = Kw = ionic product of water = 1 x 10-14
Buffer solution: The solutions which resist change in pH on dilution or with the addition of small amounts of acid or alkali are called Buffer Solutions.
Common ion effect: It can be defined as a shift in equilibrium on adding a substance that provides more of an ionic species already present in the dissociation equilibrium.