Question

How can you tell the difference between an acid and a base given that chemical equation:
${C_5}{H_5}N + {H_2}O \to {C_6}{H_5}NH + O{H^ - }?$

Answer 1

Hint: An acid is a molecule or ion capable of donating protons (hydrogen ion ${H^ + }$) or capable of forming covalent bonds with one electron pair. Base is a substance which dissociates in aqueous solution to form hydroxide ion $O{H^ - }$.

Complete step by step answer:
An acid base reaction is a chemical reaction that occurs between an acid and a base. An acid base reaction is the removal of a hydrogen ion from the acid and its addition to the base. An acid and a base reacts not to produce a salt and solvent, but to form a new acid and a new base.
In the given chemical equation ${C_5}{H_5}N + {H_2}O \to {\left[ {{C_5}{H_5}NH} \right]^ + } + O{H^ - }$ here water splits into ${H^ + }\& O{H^ - }$ ions. A hydrogen atom is devoted to ${C_5}{H_5}NH$ which makes it acidic.

Additional Information:
The first category of acids is the proton donors. In the special case of aqueous solution, proton donors form the hydronium ion ${H_3}{O^ + }$ and are known as Arrhenius acids. Acid form aqueous solution with a sour taste can turn blue litmus red. An aqueous solution of an acid has a $pH$ less then $7$ and is colloquially also referred to as acid. Bases and acids are seen as chemical opposite because the effect of an acid is to increase the hydronium $\left( {{H_3}{O^ + }} \right)$ concentration in water, whereas bases reduce this concentration. A reaction between aqueous solution of an acid and base is called neutralization, producing a solution of water and a salt in which the salt separates into its component ions. If the aqueous solution is saturated with a given salt, solute any addition such salt precipitate out of the solution. The $pH$ of a solution that is based on standard condition is greater than seven. Bases are litter.
The concept of an acid base reaction was first proposed by Roule, who introduced the word “base” into chemistry to mean a substance which reacts with an acid to give it solid form (as a salt). Bronsted Lowry definition does not refer to the formation of conjugate acids and conjugate bases, produced by the transfer of a proton from the acid to base.
The Brosted-Lowry model calls hydrogen containing substance acids. Thus some substances, which many chemists considered to be acids, such as $S{O_3}$ or $BC{l_3}$ are excluded from the classification due to lack of hydrogen. An acid alkali reaction is a special case of an acid base-reaction. Where the base is also an alkali. Acid alkali reactions are also neutralization reactions.

Note: Arrhenius acid is a substance that when added to water, increases the concentration of ${H^ + }$ ions in water. An Arrhenius base is a substance which increases the concentration of hydroxide $\left( {O{H^ - }} \right)$ ions when dissolved in water. An Arrhenius acid upon the introduction to water, the chemical must either cause directly otherwise.
An increase in the aqueous hydronium concentration or
A decrease in the aqueous hydroxide concentration.
An Arrhenius base, upon the introduction to water, the chemical must either cause, directly or otherwise.
A decrease in the aqueous hydronium concentration or
An increase in the aqueous hydroxide concentration.
Water is amphoteric, that is it can act as both an acid and a base.