1.
What is meant by the basicity of an acid ?
Answers
Answer:
Basicity of an acid is defined as the no. of hydroxide ions it can neutralize. This is by the definition of Arrhenius concept which says that the substance which releases Hydronium ions (H3O+) when dissolved in water.
But the thing is that the Arrhenius concept isn't used anymore. Acids are defined on the basis of Lewis concept which states that acids are those compounds or ions which have the tendency to accept an electron pair. So the basicity is counted in terms of no. of electron pairs gained by the acid.
Let us take the case of H3BO3 i.e. Boric acid. Boric acid is an acid still it does not release hydrogen ions on being ionized. Instead it accepts a hydroxide radical to form B(OH)4 anion. It accepts a lone pair of electrons from the hydroxide radical.
So, the basicity can be counted as per the need.
Explanation:
Answer:
Explanation:
The basicity of an acid is the number of hydrogen ions, which can be produced by one molecule of the acid. The table below shows some acids and their basicity.
Acid
Basicity
HCl H+ + Cl-
H2SO4 2H+ + SO42-
H3PO4 3H+ + PO42-
CH3COOH H+ + CH3COO-
1 Monobasic
2 Monobasic
3 Monobasic
1 Monobasic
Note: It isn’t in all cases that a compound furnishes all its containing hydrogen atoms as ions. Example, in ethanoic acid.
When 1 mole of hydrogen ions is furnished from 1 mole of an acid, the acid is monobasic; it is dibasic when 2 moles of hydrogen ions are furnished, and tribasic when 3 moles of hydrogen ions are furnished from 1 mole of its solution.
Related Tutorials
The Concepts of Acids and Bases
How to Determine Strength of Acids
Properties of Acids
Uses of Acids
Methods of Preparation of Acids
The BrØnsted-Lowry Concept of Acids And Bases
The Lewis Concept of Acids and Bases