Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

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Class 10 : Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

The document Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev is a part of the Class 10 Course Science Class 10.
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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).Importance of pH in Everyday Life and Salts Class 10 Notes | EduRevFig. pH scaleVariation 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 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) 
or 
H+(aq) < 1 × 10-7 mol litre-1, then the solution should be basic or alkaline.

Table - pH Value of Some Common Substances 

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev


IMPORTANCE OF PH IN EVERYDAY LIFE
1. Plants and Animals are 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.

Soil pH and Plants: 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).

2. Importance of 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

3. PH change as the cause of tooth decay:

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRevFig. pH level of toothGenerally, 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 toothpastes which are generally basic, for cleaning the teeth. It neutralise the excess acid and prevent tooth decay.

4. 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.

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.
For Example-
Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev
(Partial replacement : only one hydrogen atom is replaced)
Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev
(Complete replacement : Both the hydrogen atom are replaced)
Example-

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev
A salt is a ionic compound which dissolved in water dissociate to 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: 

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev
Some Normal salts with their parent acids

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

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.

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

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

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

GENERAL METHODS OF PREPARATION OF SOLUBLE SALTS
(i) By direct combination of elements - By heating two elements together

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev
(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 -
Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

(IV) By the process of neutralization -
Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

(V) By the action of alkalis on metals - 
Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

General methods of preparation of insoluble salts -

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

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

By double decomposition of two soluble salt -

Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev

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 which 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.
(i) 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:
Importance of pH in Everyday Life and Salts Class 10 Notes | EduRev
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.

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