What Is Neutralization Reaction and Why It Is Important in Daily Life with Examples
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.
Indigestion
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.
Ant Sting
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.
Tooth Decay
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.
Shiny Hair Due to Conditioner
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.
Monitor pH of the Soil
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.
FAQs on Importance of Neutralization Reaction in Daily Life Explained
1. What is a neutralization reaction in chemistry?
A neutralization reaction is a chemical reaction in which an acid reacts with a base to form salt and water. The general form of a neutralization reaction is:
Acid + Base → Salt + Water
For example:
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
In this reaction, hydrochloric acid reacts with sodium hydroxide to produce sodium chloride (salt) and water. Neutralization reactions are important in daily life, laboratories, medicine, and industry.
2. Why is neutralization reaction important in daily life?
A neutralization reaction is important in daily life because it helps control excess acidity or basicity in the body, soil, water, and industries. Key examples include:
- Indigestion relief: Antacids neutralize excess stomach acid.
- Soil treatment: Farmers add lime to acidic soil to improve crop growth.
- Toothpaste action: Basic toothpaste neutralizes acids produced by bacteria.
- Wastewater treatment: Industries neutralize acidic or basic waste before disposal.
3. How do antacids work as a neutralization reaction?
Antacids work by neutralizing excess hydrochloric acid (HCl) in the stomach through a neutralization reaction. For example:
Mg(OH)2(s) + 2HCl(aq) → MgCl2(aq) + 2H2O(l)
Magnesium hydroxide, a common antacid, reacts with stomach acid to form magnesium chloride and water. This reduces acidity and relieves symptoms like heartburn and indigestion.
4. How is neutralization used in agriculture?
In agriculture, neutralization is used to reduce soil acidity and improve crop productivity. Farmers add basic substances such as:
- Calcium oxide (CaO)
- Calcium hydroxide (Ca(OH)2)
- Calcium carbonate (CaCO3)
5. What is the general equation for a neutralization reaction?
The general equation of a neutralization reaction is:
Acid + Base → Salt + Water
In ionic form, the net ionic equation is:
H+(aq) + OH-(aq) → H2O(l)
This shows that hydrogen ions from the acid combine with hydroxide ions from the base to form water, which is the key step in neutralization reactions.
6. How is neutralization used in treating insect stings?
Neutralization helps treat insect stings by counteracting the acidic or basic venom using an opposite substance. Examples include:
- Bee sting (acidic): Treated with baking soda (NaHCO3), a mild base.
- Wasp sting (basic): Treated with weak acids like vinegar (CH3COOH).
7. How is toothpaste related to neutralization reaction?
Toothpaste prevents tooth decay by neutralizing acids produced by bacteria in the mouth. These acids can erode enamel if not controlled. Toothpaste contains mild bases such as:
- Sodium bicarbonate (NaHCO3)
- Calcium carbonate (CaCO3)
8. How is neutralization reaction used in wastewater treatment?
In wastewater treatment, neutralization is used to adjust the pH of acidic or basic industrial effluents before discharge. For example:
- Acidic waste is treated with bases like Ca(OH)2.
- Basic waste is treated with acids like H2SO4.
9. What are some common examples of neutralization reactions in daily life?
Common examples of neutralization reactions in daily life include:
- Antacid and stomach acid: Mg(OH)2 + 2HCl → MgCl2 + 2H2O
- Lime and acidic soil: CaCO3 reacts with soil acids.
- Toothpaste and mouth acids: Bases neutralize bacterial acids.
- Insect sting treatment: Baking soda or vinegar neutralizes venom.
10. What is the difference between acid-base reaction and neutralization reaction?
A neutralization reaction is a specific type of acid–base reaction that produces salt and water as products. The differences are:
- Acid–base reaction: Any reaction involving transfer of H+ (Brønsted–Lowry concept).
- Neutralization reaction: Specifically forms salt and water.
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
All neutralization reactions are acid–base reactions, but not all acid–base reactions result in complete neutralization.
