Importance of pH in Everyday Life & Salts

# Importance of pH in Everyday Life & Salts - Science Class 10

## pH Scale

S.P.L. Sorenson, a Danish Chemist in 1909 introduced the concept of measuring the concentration of hydrogen ions (H+(aq)) in a particular solution. The p in pH stands for 'potenz' in German, meaning power. On the pH scale we can measure pH from "0" (very acidic) to 14 (very alkaline).pH Scale

### Universal Indicator

A universal indicator has a pH range from 0 to 14 that indicates the acidity or alkalinity of a solution.

A neutral solution has pH=7

### pH

pH=−log10[H+]

In pure water, [H+]=[OH−]=10−7 mol/L. Hence, the pH of pure water is 7.

The pH scale ranges from 0 to 14.

If pH < 7 → acidic solution

If pH > 7→ basic solution

Question for Importance of pH in Everyday Life & Salts
Try yourself:
Which chemist introduced the concept of measuring the concentration of hydrogen ions in a solution?

### Variation of pH with the Change in Concentration of H+(aq) and OH- (aq) Ions

The concentration of H+ (aq) and OH- (aq) ions in pure water is 1 × 10-7 mol litre-1. This means that all aqueous solutions contain both H+(aq) and OH- (aq) ions.

The product of concentration of H+(aq) and OH-(aq) in water is constant (equal to 1 × 10-14 mol2 litre-2 at 25°C) and is known as the ionic product of water (KW).
KW = [H+(aq)] [OH- (aq)]
= (1 × 10-7) (1 × 10-7
= 1 × 10-14 mol2 litre-2 at 25°C

• If [H+(aq)] = [OH-(aq)] = 1 × 10-7 mol litre-1, then the solution is neutral.
• If H+(aq) > OH- (aq) or (H+ (aq) > 1 × 10-7 mol litre-1), then the solution should be acidic and if H+(aq) < OH-(aq).
• If H+(aq) < 1 × 10-7 mol litre-1, then the solution should be basic or alkaline.

## Importance of pH in Everyday Life

### Are Plants and Animals pH Sensitive?

The pH plays an important role in the survival of animals, including human being. Our body works well with in a narrow pH range of 7.0 to 7.8. The aquatic animals (Fish) can survive in river water with in a narrow range of pH change.
Example: When the pH of rain water is about 5.6, it is called acid rain. Too much acid rain can lower the pH of river water to such an extent and make it so acidic that the survival of aquatic animals becomes difficult or kill the aquatic animals.

### What is the pH of Soil pH?

Most of the plants grow best when the pH of soil is close to 7. If the soil is too acidic or too basic (too alkaline), the plants grow badly or do not grow at all.

Treatment of Acidic or Basic Soil: The pH of acidic soil can reach as low as 4 and that of the basic soil can go up to 8.3. Chemicals can be added to soil to adjust its pH and make it suitable for growing plants. If the soil is too acidic, then it is treated with materials like quicklime (calcium oxide) or slaked lime (Calcium hydroxide) or chalk (Calcium carbonate). All these materials are bases and hence react with the excess acid present in soil and reduce its acidity. If the soil is too basic (or too alkaline) then its alkalinity can be reduced by adding decaying organic matter (manure or compost).

### pH in our Digestive System

As we know our stomach produces gastric juice which contains large amount of hydrochloric acid (pH about 1.4). The acid so produced does not harm the stomach walls, but kills germs and bacteria which enter in our digestive system along with food, thus in a way it protects us from diseases and helps in digestion. Sometimes excess of acid is produced in the stomach due to overeating or eating spicy foods. This stage is called acidity. To get relief from this pain, we take tablets known as antacids. These contain bases to neutralise the excess acids.
Example: Magnesium hydroxide (milk of magnesia).Mg(OH)2

### pH Change as the cause of Tooth Decay

pH Level of Tooth

Generally, the pH in the mouth is more than 7, as the saliva produced in the mouth is basic in nature. However, when we take food, some food particles remain in the mouth after eating and bacteria present in the mouth produce acids by degradation of food particles. This acid lowers the pH in the mouth, tooth decay starts when the pH of acid formed in the mouth falls below 5.5. Therefore to prevent tooth decay, it is advised to clean the mouth and use toothpaste which is generally basic, for cleaning the teeth. It neutralises the excess acid and prevents tooth decay.

### Self-defence by Animals and Plants through Chemical Warfare

The sting of the honey bee contains formic acid, this acid causes a lot of irritation and pain. The pain can be reduced by applying baking soda paste on the affected region as the acid gets neutralised.
In plant kingdom nettle (Bichu Booti) is a herbaceous plant which grows in wild. The nettle leaves have stinging hair. When a person happens to touch the leaves of a nettle plant accidently, the stining hair of nettle leaves inject methanoic acid (HCOOH) into the skin of the person causing burning pain. The nettle sting, being acidic can be neutralised by rubbing baking soda on the skin. Nature provides remedy for the nettle sting in the form of a 'dock' plant, which often grows besides the nettle plants. The leaves of dock plant contain some basic chemicals which neutralises methanoic acid.

Question for Importance of pH in Everyday Life & Salts
Try yourself:
What is the pH range in which our body functions optimally?

## Salts

A substance formed by the partial or complete replacement of H+(aq) ions of an acid by a metal or electropositive ion, is called a salt.
Example:

(Partial replacement: only one hydrogen atom is replaced)

(Complete replacement: Both the hydrogen atom are replaced)
Example:

A salt is an ionic compound which dissolved in water dissociate into positive ions other than hydrogen ions (H+) and negative ions other than hydroxyl ions (OH-) are called salts.
Example:
NaCl + Water → Na+(aq) + Cl-(aq)
CuSO4 + Water → Ca2+(aq) + SO42- (aq)

### Naming of Salts

(a) Salt obtained from "Sulphuric acid" are called "Sulphates".
Example: Na2SO4, CuSO4
(b) Salt obtained from "nitric acid" are called "Nitrates".
Example:  KNO3, NaNO3
(c) Salt obtained from "hydrochoric acid" are called "Chlorides".
Example: NaCl, CaCl2, KCl
(d) Salt obtained from "phosphoric acid" are called "Phosphates".
Example: Ca3(PO4)2, Na3PO4, Mg3(PO4)2
(e) Salt obtained from "carbonic acid" are called "Carbonates".
Example: Na2CO3, K2CO3, CaCO3.
(f) Salt obtained from acetic acid are called "Acetates".
Example: CH3COONa, (CH3COO)2Ca, CH3(COO)2Pb.

### Classification of Salts

The salts may be classified in the following ways:
1. Normal Salts: These salts are formed as a result of reaction between strong acid and strong base.
Examples:

Some Normal Salts with their Parent Acids

2. Acidic Salts: The salts which are obtained by the partial replacement of ionisable hydrogen atoms of a polybasic acid by a metal or an ammonium ion are called Acid Salts.

3. Basic Salts: The salt which are formed by partial replacement of hydroxyl (-OH) groups of a polyacidic base by an acid radial are called basic salts.

### Family of Salts

Salts having the same cation or anion belong to the same family. For example, NaCl, KCl, LiCl.

### pH of Salts

A salt of a strong acid and a strong base will be neutral in nature. pH = 7 (approx.).

A salt of a weak acid and a strong base will be basic in nature. pH > 7.

A salt of a strong acid and a weak base will be acidic in nature. pH < 7.

The pH of a salt of a weak acid and a weak base is determined by conducting a pH test.

### General Methods of Preparation of Soluble Salts

(i) By direct combination of elements: By heating two elements together

(ii) By the action of dilute mineral acids on active metals:
Zn + dil. H2SO4 → ZnSO4 + H2(g)
2Al + dil 6HCl → 2AlCl3 + 3H2 (g)
2Na + dil. 2HCl → 2NaCl + H(g)

(iii) By Decomposition:
(a) By Decomposition of metal hydrogen carbonates:
NaHCO3(s) + HCl (dil) → NaCl + H2O + CO2(g)
(b) By Decomposition of metal carbonates:
CuCO3(s) + 2HCl (dil) → CuCl2 + H2O + CO2(g)
(c) By decomposition of metal chloride:

(iv) By the process of neutralization:

(v) By the action of alkalis on metal:

### General Methods of Preparation of Insoluble Salts

(i) By direct combination of elements:
When metal powder is heated with sulphur, we get corresponding metal sulphides which are insoluble salts.

(ii) By double decomposition of two soluble salt:

### Sodium Chloride (Common Salt / Table Salt)

We know that hydrochloric acid and sodium hydroxide combine with each other to form sodium chloride (NaCl) which in common language is also known as common salt. This is the salt that you sprinkle on your salads and use in your kitchens. Common salt is an ionic compound of sodium and chlorine (Na+Cl-)n.

The main source of common salt (sodium chloride) is the sea water. Sea water contains about 3.5% of soluble salts, the most common of which is sodium chloride (2.7 to 2.9%). Sambhar lake in Rajasthan is also a good source of common salt (sodium chloride) is also found as rock salt. Beds of rock salt were formed when lakes/Seas dried up in past. Use the above point in form of “do you know”

Chemicals from Common Salt
Common salt is a raw material for chemicals and play an important role for making various materials of daily use. Such as sodium hydroxide, baking soda, washing soda, bleaching powder and many more.
Sodium hydroxide: Commercially, sodium hydroxide is also called caustic soda because of its corrosive action on animal and vegetable tissues.

Chlor-alkali Process for obtaining Sodium Hydroxide
When we pass electricity through a solution of sodium chloride, commonly called brine. It decomposes to form sodium hydroxide according to the following equation:

Chlor-alkali Process

On electrolysis, chlorine gas is formed at anode and hydrogen at cathode sodium hydroxide solution is formed near the cathode. All these products are commercially important. The process of production of sodium hydroxide from sodium chloride is known as chlor-alkali process because of products formed - chlor for chlorine and alkali for sodium hydroxide.

The document Importance of pH in Everyday Life & Salts | Science Class 10 is a part of the Class 10 Course Science Class 10.
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## Science Class 10

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## FAQs on Importance of pH in Everyday Life & Salts - Science Class 10

 1. What is the pH scale?
Ans. The pH scale measures the acidity or basicity of a solution. It ranges from 0 to 14, with 0 being the most acidic, 7 being neutral, and 14 being the most basic.
 2. Why is pH important in everyday life?
Ans. pH is important in everyday life because it affects many aspects of our lives, such as the taste of food and beverages, the effectiveness of cleaning products, and even the health of our bodies. For example, the pH of our blood must remain within a narrow range to maintain proper bodily function.
 3. What are salts?
Ans. Salts are ionic compounds made up of a positively charged metal ion and a negatively charged non-metal ion. They can be formed by the reaction between an acid and a base, or by the reaction between a metal and a non-metal.
 4. How do salts relate to pH?
Ans. Salts can affect the pH of a solution depending on their chemical properties. Some salts, such as sodium chloride (table salt), do not affect the pH of a solution. Other salts, such as ammonium chloride, can make a solution more acidic, while still others, such as sodium bicarbonate (baking soda), can make a solution more basic.
 5. What are some examples of everyday products that involve pH and salts?
Ans. Many products we use on a daily basis involve pH and salts. Examples include cleaning products such as bleach and ammonia, which are basic and acidic, respectively, and use salts to enhance their cleaning properties. Personal care products such as shampoos and soaps also use a combination of pH and salts to achieve the desired cleansing and moisturizing effects. Additionally, food and beverages like coffee and orange juice have varying pH levels that affect their taste and acidity.

## Science Class 10

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