Introduction to Acid
An acid is a substance which reacts to a base. Generally, acids can be recognized as tasting sour, reacting with metals for example- calcium and bases for example- sodium carbonate. Aqueous acids have pH below 7, as the acidity increases, pH decreases. Chemicals having characteristics of an acid are found to be acidic.
General examples of acids comprises of acetic acid (in vinegar), sulphuric acid (used in car batteries) and tartaric acid (used in baking). As these 3 examples exhibit, acids can be liquids, solutions, or solids. Gases such as hydrogen chloride can be acids too. Some strong acids and concentrated weak acids are corrosive, but there are exceptions such as carbonates and boric acid.
Introduction to Base
A base is a substance that can take hydrogen ions (protons) or usually, donate a pair of valence electrons. Soluble base is known as an alkali if it takes and releases hydroxide ions (OH-) quantitatively. The Bronsted-Lowry theory explains bases as proton (hydrogen ion) acceptors whereas the more general Lewis theory defines bases as electron pair donors, permitting other Lewis acids than the protons to be taken. Oldest Arrhenius theory explains bases as hydroxide anions that are strictly applied only to alkali.
In water by changing the autoionization equilibrium bases provide solutions with a hydrogen ion activity lower as that of pure water, that is, a pH more than 7.0 at standard conditions. Examples of common bases are ammonia and sodium hydroxide. Metal hydroxides, oxides, and particularly alkoxides are basic and counter anions of weak acids are basically weak bases.
Strength of Acids and Bases:
Acids
1. Strong Acids:
Fully dissociate in water, developing H+ and an anion.
There are simply 6 strong acids: The left over acids thus are considered weak acids.
HCl, H2SO4, HNO3, HClO4, HBr, HI
2. Weak acids:
A weak acid only partially dissociates into water to produce H+ and the anion
For instance, HF dissociates in water to provide H+ and F-. It is weak acid. With a dissociation equation
HF(aq) ↔ H+(aq) + F-(aq)
Note: Double arrow is used for the weak acid.
Bases
1. Strong Bases:
They dissociate 100% into the OH- (hydroxide ion) and cation.
Example: NaOH(aq) → Na+(aq) + OH-(aq)
Q. Which are found to be strong bases?
A. The hydroxides of Groups I and II.
2. Weak Bases:
What compounds are taken as weak bases?
Usually weak bases are anions of weak acids.
Weak bases do not provide OH- ions through dissociation. They react with water to provide the OH- ions.
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