Neutralisation Reaction Examples: Neutralisation and heat of Neutralization

Acid and base work together to make salts and water. This reaction is called neutralization.

Example:

NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

According to ionic theory, the above reaction can also be written as follows.

Na⁺(aq) + OH^–(aq) + H⁺(aq) + Cl^–(aq) → Na⁺(aq) + Cl^–(aq) + H₂O(l)

H⁺(aq) + OH^–(aq) → H₂O(l)

According to ionic theory, the reaction in which H⁺ ion and OH^– ion form water by interacting with each other is called neutralization. According to the modern concept, the reaction of acid and base is called neutralization.

Heat absorbed in the neutral neutralization of dilute solutions of a gram-Equivalent weight acid and a gram-Equivalent weight base is called heat of neutralization.

Strong acid and strong base dissolve almost completely in their ions in solution. The neutralization heat of strong acid and strong base is actually the reaction heat of the reaction of H⁺ and OH^– to H₂O. Hence the value of heat of neutralization of strong acid and strong base is constant.

Heat is emitted in the neutralization reaction. In neutralization reaction of strong acid and strong base, 13.7 kcal of heat is emitted. Hence heat of neutralization of strong acid and strong base is 13.7 Kcal.

HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) + 13.7kcal

HNO₃(aq) + KOH(aq) → KNO₃(aq) + H₂O(l) + 13.7kcal

The numerical value of strong acid and strong base heat of neutralisation is less than 13 .7 kcal. Less than 13 kcal of heat is produced in this reaction. The reason for this is that ionization of weak acids and weak bases is not complete.

Initially, H⁺ derived from acid and OH^– ion obtained from base produce 13.7 kcal heat. Some of this heat is used to complete ionization of weak acid and weak base. Therefore, the value of free heat is less than 13.7 kcal and the numerical value of heat of neutralization is less than 13.7 kcal.

Example:

CH₃COOH(aq) + NaOH(aq) → CH₃COONa(aq) + H₂O(l) + 13.3 kcal

HCOOH(aq) + NH₄OH(aq) → HCOONH₄(aq) + H₂O(l) + 11.9kcal

Salts

Acid and base reaction together to make salt and water.

Example:

NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

According to the ionic theory of arhinius, in addition to the neutralization reaction of acid and base, other substances formed in addition to water are called salts.

According to modern ideas, an ionic solid obtained from neutralization reaction of an acid and base is called salts.

Example:

NH₃ + HCl → NH₄Cl

On dissolving the salts in water, it dissolves in its ions. Cations are called basic radicals and anions are acidic radicals.

Example:

NaCl(aq) ⇌ Na⁺(aq) + Cl^–(aq)

Classification of salts

There are six types of salts –

Normal Salts

Simple salts that do not contain substitutable H⁺ or OH^– are called normal salts.

Example – NaCl and KNO₃ are normal salts.

Acidic Salts

Acidic Salts: The salts that contain substitutable H⁺ are called acidic salts.

NaHSO₄ and NaHCO₃ are acidic salts.

Basic Salts

Those salts which contain substitutable OH^– are called basic salts.

Example: Mg(OH)Cl ZnCl, Pb(OH)NO₃ and Zn(OH)Cl is basic salts.

Mixed Salts

Those salts which contain more than one type of cation or anion are called mixed salts. NaKSO₄ and Ca(OCl)Cl are mixed salts.

Double Salts

The salts obtained from the evaporation of aqueous solution of two simple salts are called double salts. The ratio of normal salts in double salts is fixed and they exist only in solid state. In aqueous solutions, they dissociate into ions of normal salts.

Example: potash alum[K₂SO₄.Al₂(SO₄)₃.24H₂O] and mohr salt[FeSO₄.(NH₄)₂SO₄.6H₂O] are double Salts.

Complex Salts

The salts in which ion or neutral molecules form a co-connective bond with a metallic cation are called complex salts.

Example:

K₄[Fe(CN)₆] and [Cu(NH₃)₄]Cl₂ are complex salts.

K₄[Fe(CN)₆] has a sub-valence bond between Fe²⁺ and CN^– and [Cu(NH₃)₄]Cl₂ has a sub-valence bond between Cu²⁺ and NH₃.

Complex ions are obtained by dissolving complex salts in water. Complex ions in solutions do not dissociate in their components or have very small amounts of ionization.

K₄Fe(CN)₆(aq) ⇌ 4K⁺ + [Fe(CN)₆]^4-

Salt Hydrolysis

Decomposition of a compound by water is called hydrolysis. The solution obtained after hydrolysis of a salt is neutral, basic and acidic.

Example:

Aqueous solutions of NH₄Cl and CuSO₄ are acidic, aqueous solutions of Na₂CO₃ and CH₃COONa are basic. And the aqueous solutions of NaCl and KNO₃ are neutral. Reaction in which a salt is reacted with water to form an acidic, basic or neutral solution. This is called hydrolysis of salt.

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The ionization of water is like this.

H₂O ⇌ H⁺ + OH^–

It is neutral due to the same amount of H⁺ and OH^– ion in pure water. If there is more H⁺ ion in the solution when salt is dissolved in water, then that solution will be acidic and if OH^– ion is more, then this solution will be basic.

To simplify the study of the hydrolysis of salts, the salts are divided into four parts –

Hydrolysis of salt made from weak acid and strong base

The solution obtained from hydrolysis of salt made from a weak acid and strong base is basic.

Example: Aqueous solution of sodium carbonate is basic. On dissolving Na₂CO₃ in water, the following actions take place –

H₂O ⇌ H⁺ + OH^–

Na₂CO₃ ⇌ 2Na⁺ + CO₃^2-

2Na⁺ + 2OH^– ⇌ 2NaOH (strong base)

2H⁺ + CO₃^2- ⇌ H₂CO₃

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NaOH is a strong base and is almost completely ionized. H₂CO₃ is weak acid and the number of H⁺ ions obtained from its ionization is less. Hence the number of OH^– ions in the solution is high and the solution is basic.

Similarly, CH₃COONa and KCN are also salts made from weak acid and strong base and their aqueous solutions are basic.

Hydrolysis of salt made from strong acid and weak base

The solution obtained from hydrolysis of salt made from strong acid and weak base is acidic.

Example: Aqueous solution of ammonium chloride is acidic. The following actions take place when NH₄Cl is dissolved in water.

H₂O ⇌ H⁺ + OH^–

NH₄Cl ⇌ NH₄⁺ + Cl^–

NH₄⁺ + OH^– ⇌ NH₄OH (weak base)

H⁺ + Cl^– ⇌ HCl (strong acid)

HCl is strong acid and almost completely ionized NH₄OH is a weak base and the number of OH ions obtained from its ionization is low. It is acidic due to the high number of H ions in the solution.

Similarly Cu and HeSO₄ are obtained by dissolving CuSO₄ in water. Which are weak base and strong acid respectively. Hence the aqueous solution of CuSO₄ is also acidic. Similarly, FeCl₃ is also a salt of this category and its aqueous solution is acidic.

Hydrolysis of salt made from strong acid and weak base

CO₃ and CH₃COONH₄ are salts of this category. The solution obtained from hydrolysis of this category of salts can be acidic, basic or neutral. It depends on the relative strength of acid and base.

Example: On dissolving ammonium carbonate in water, the following actions take place.

H₂O ⇌ H⁺ + OH^–

(NH₄)₂CO₃ ⇌ 2NH₄⁺ + CO₃^2-

NH₄⁺ + OH^– ⇌ NH₄OH (weak base)

2H⁺ + CO₃^2- ⇌ H₂CO₃   (weak acid)

NH₄OH is weak base and H₂CO₃ is weak acid. The ionization of NH₄OH is higher than that of H₂CO₃. Hence the concentration of OH^– in the solution is high and the solution is basic.

On dissolving ammonium carbonate in water, the following actions take place –

H₂O ⇌ H⁺ + OH^–

CH₃COONH₄ ⇌ CH₃COO^– + NH₄⁺

CH₃COO^– + H⁺ ⇌ CH₃COOH                       (weak acid)

NH₄⁺ + OH^– ⇌ NH₄OH            (weak base)

CH₃COOH is weak acid and NH₄OH is weak base. Their values of K_a and K_b are 1.80 x 10^-5 and 1.78 x 10^-5 respectively. Hence, their ionisation volumes are almost the same. Hence, the number of H⁺ and OH^– ions in the solution is almost equal and the solution is neutral.

Hydrolysis of salt made from strong acid and strong base

NaCl is the salt in this category. When this salt is dissolved in water, it gets ionized but there is no action with water.

The reason for this is that strong acid and strong base completely dissociate in aqueous solution and no new substance is formed.

Because of this there is no change in the number of H⁺ and OH^– ions and the solution is neutral. Therefore, salt water of this category is not decomposed and their aqueous solution is neutral.