[Chemistry Class Notes] Importance of Neutralization Reaction in Daily Life Pdf for Exam

When an acid and a base react together to form salt and water as the products of their chemical reaction, the process is termed a neutralisation reaction. For example, hydrogen ions from the acid combine with hydroxide ions of the base to form water. Strong acid and solid base neutralisation products have a pH equal to 7. Neutralising a strong acid and a weak base will have a product with a pH of less than 7, and conversely, the resulting pH will be greater than 7 when a strong base neutralises a weak acid. 

When a solution is neutralised, it means salts are formed out of the same acid and base weights. The amount of acid required is the amount that would give a one-mole proton (H⁺), and the amount of base needed is the amount that would give one (OH^–) mole. Since salts are formed from neutralisation reactions with equivalent acid and base in terms of weight concentrations: N parts of acid will always neutralise with N parts of the base.

Neutralisation reaction is given by: 

acid + base → water + salt

Neutralisation plays an extremely important role in our daily life. Let’s find out.

Examples of Neutralisation Reaction

Acid + Base —> H₂O + Salt

H⁺Cl  (acid)+ NaOH^– (base) —> H₂O + NaCl (salt)

H⁺NO₃ (acid) + NaOH^– (base) —> H₂O + NaNO₂(salt)

The Importance of Neutralisation Reaction in Daily Life

Let us look at some common neutralisation reactions that we experience on a daily basis and understand the importance of neutralisation reactions in our daily life.

Too much acid is produced inside the stomach during indigestion which results in stomach disorder or acidity. We take bases such as magnesium milk which contains magnesium hydroxide to retrieve the pain. Taking a base neutralises the excess acid in our stomach.

The ant sting can be painful as it has formic acid. We can neutralise this acid effect and relieve the pain caused by the sting by using moist baking soda which is basic in nature.

When we eat food, the food molecules get decomposed by the action of the microorganism present in the mouth. This results in the formation of acid. This acid is majorly responsible for tooth decay. Toothpaste is generally made by alkaline substances to make its nature basic. So, when you brush your teeth, this basic nature of the toothpaste reacts with the acid produced by the microorganisms. As a result, the harmful effect of the acid is neutralised, and it stops tooth decay.

Our hair becomes rough after a shampoo, but it becomes shiny after using a conditioner. This happens because shampoo is basic in nature and the conditioner is acidic. So, the conditioner neutralises its effect, and the hair becomes shiny.

Plants grow in soil that has a particular pH value. Plants cannot grow on soil that has an acidic composition. So, to neutralise its effect, bases are added to the soil. Compounds such as limestone, powdered lime, and also burnt wood ashes are added to the soil to make its pH less acidic. This technique helps in controlling the pH of the soil by neutralising the effect of acids in the soil.

Other Examples of Neutralisation Reaction in Daily Life

• In wastewater treatment, this method is used to reduce the damage caused by the effluents. 

• A neutralisation reaction is also used in the antacid tablet manufacturing process.

• The power stations and industries emit acidic gases such as sulphur dioxide in the air as a by-product of several chemical processes taking place during the operations. These gases are harmful to the body if inhaled and also harmful to the environment. As a result, these gases are treated with lime (CaO – calcium oxide) in order to neutralise and reduce their harmful effects. 

• In the industries, the coagulation of latex is prevented by the use of ammonia, NH₃. The bacteria in the latex produces acid, whose effect is neutralised by the basic nature of ammonia. 

Example Questions

1.  Give examples of strong acids and strong bases. 

Ans: Some examples of strong acids and strong bases are as follows: 

• Strong Acids: Hydrochloric acid, hydroiodic acid, nitric acid, chloric acid, hydrobromic acid, perchloric acid, and sulphuric acid.

• Strong Bases: Lithium hydroxide, calcium hydroxide, sodium hydroxide, potassium hydroxide, caesium hydroxide etc.