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 .