Rate of a Reaction
Rate of a reaction is defined as the speed at which the reactants are converted into products.
Slow Reaction
Slow reactions are reactions that can be measured in the laboratories. e.g., hydrolysis of ester
Fast Reactions
Fast reactions are generally ionic reactions. It is difficult to measure their rates.
Reversible Reactions
The reactions in which the products can react with one another under suitable conditions to give back the reactants are called reversible reactions.
Irreversible Reactions
The chemical reactions where the products do not combine to give the reactants are called irreversible reactions.
Arrhenius Acid
A substance which dissociates in aqueous solution to give hydrogen ions is an Arrhenius acid.
Arrhenius Base
A substance which dissociates in aqueous solution to give hydroxyl ions is called an Arrhenius base.
Lewis Acid
A substance which can accept a pair of electrons is termed Lewis acid.
Lewis Base
A substance which can donate a pair of electrons is called Lewis base.
Bronsted-Lowry Acid
A substance which can donate a proton is a Bronsted-Lowry acid.
Bronsted-Lowry Base
A substance that can accept a proton is a Bronsted-Lowry base.
pH
pH is the negative logarithm of H3O+ ion concentration in moles/litre
pH of water = 7 at 298 KpH of acids = less than 7
pH of bases = greater than 7Exothermic Reactions
The chemical reactions which proceed with the evolution of heat energy DH = -ve.
Endothermic Reactions
The chemical reactions which proceed with the absorption of heat energy, DH = +ve.
