plz!!!!!!!!!!!! give me uses of acids bases and salts 6pages=12pages ?

Acids Bases and Salts Use

You must have tasted a piece of orange or a slice of lemon.
The sour taste of an orange or lemon is because of the presence of acids in them.
Acids could be easily identified by their typical sour taste.
These could be found in many of the available substances, including food.
Some common examples include the citric acid present in citrus fruits like oranges and lemons and acetic acid in vinegar.
Some acids are widely used in the laboratory like hydrochloric acid, sulphuric acid and nitric acid.
Human body also contains a very common acid that is dilute hydrochloric acid in stomach, which helps us digest our food.
Any substances which ionize in water solutions to produce a hydrogen ion (H⁺) are known as acid.
They are sour and react with metal to release hydrogen gas. For example; hydrochloric acid dissolved in water to produce hydronium ion and chloride ion.
HCl + H₂O ==> H₃O⁺ + Cl^-Citrus fruits like lemon, lime and grapefruit contain citric acid which is widely used as flavouring agent, preservative and cleaning agent.
Citric acid is also used in many other products.
It acts as a preservative in foods, and is even used in production of hair cleaners or gels and low –pH shampoos and toothpastes.
In fact, Carboxylic acids are also used industrially in the use of fatty acids for making soaps, detergents and shampoos.
Other acid like sulfuric acid is most widely used in automobile industries for car batteries and for removing rust from metal surface.
Nitric Acid is used in the manufacture of fertilizers, plastics and dyes.
Some common acids with their formula and uses are as follows;

Apart from acid, bases are substance which releases hydroxyl ion (OH^-) in their aqueous solution.
In our everyday life, bases are found in household cleaners, soap, toothpaste, egg whites, dishwashing liquids and household ammonia.
They are also present in urine, blood, and intestinal fluid, and other things that we intake like dairy and "TUMS". Blood is also slightly basic in nature.
Sodium hydroxide which is also known as caustic soda and usually exists as semi-spherical pellets is most common base.
NaOH (sodium hydroxide) quickly reacts with the carbon dioxide in air, to form sodium carbonate.
It is used in many industries, mostly as a strong base in paper and textiles industries, in manufacturing of soaps and detergents and as a drain cleaner. Some other bases with their uses are as follows;

The reaction of an acid and a bases yields two products; water and an ionic compound known as salt.
This kind of reaction is called a neutralization reaction.
For examples; sodium hydroxide reacts with hydrochloric acid and form sodium chloride and water.

Na⁺ OH^- + H⁺Cl^- ==> H₂O + Na⁺Cl^–Because the salt produced in reaction is ionic in nature hence exists in the form of ions just as it did before the reaction.
The most common salt is sodium chloride or table salt which produced from the neutralization reaction of sodium hydroxide (base) and hydrochloric acid.
Sodium chloride is mainly used as a raw material in the preparation of other salts such as NaHCO₃, Na₂CO₃, NaOH etc.
The most common salt of sodium is sodium carbonate or soda (Na₂CO₃) used in manufacturing of glass.
It is also used in water purification and sewage treatment systems.
Other examples include epsom salts (MgSO₄) used in bath salts, ammonium nitrate (NH₄NO₃) used as a fertiliser and baking soda (NaHCO₃) used for making breads, cakes and cookies.
Ammonium sulphate or ammonium nitrate salts are important agro-chemical fertilisers for better plant growth.
Harmful acidic sulphur dioxide gas that emerges as a waste product from power station smoke can be absorbed by basic calcium hydroxide solutions to form harmless calcium sulphate.

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Definition of acids , bases and salts:

Acids Bases Salts

Sour in taste Bitter in taste &

soapy to touch

Acid + Base → Salt

+ Water

Give H+

or H3O

ions in aqueous

solutions

Give OH-

ions in

aqueous solutions

2. On the basis of origin, acids are classified as:

a. Organic acids: Acids derived from living organisms like plants and

animals are called organic acids. They are weak acids and are not

harmful for living organisms. For example: citric acid is present in

fruits, acetic acid present in vinegar, oxalic acid present in

tomato, tartaric acid present in tamarind, lactic acid present in

sour milk and curd.

b. Mineral acids: They are also called inorganic acids. They are

dangerous and corrosive. Special precautions have to be taken

while handling them. For example: sulphuric acid (H2SO4),

hydrochloric acid (HCl) etc.

3. On the basis of their strength, acids are classified as:

a. Strong acids: Strong acids are those acids which completely

dissociate into its ions in aqueous solutions. Example: nitric acid

(HNO3), sulphuric acid (H2SO4), hydrochloric acid (HCl).

b. Weak acids: Weak acids are those acids which do not completely

dissociate into its ions in aqueous solutions. For example:

carbonic acid (H2CO3), acetic acid (CH3COOH).

4. On the basis of their concentration, acids are classified as:

a. Dilute acids: Have a low concentration of acids in aqueous

solutions.

b. Concentrated acids: Have a high concentration of acids in

aqueous solutions.

5. Alkalies: Water soluble bases are called alkalies. For example: Sodium

hydroxide (NaOH), potassium hydroxide (KOH).

6. On the basis of their strength, bases are classified as:

a. Strong bases: Strong bases are those bases which completely

dissociate into its ions in aqueous solutions. Example: sodium

hydroxide (NaOH), potassium hydroxide (KOH).

b. Weak bases: Weak bases are those bases which do not

completely dissociate into its ions in aqueous solutions. For

example: ammonium hydroxide (NH4OH).

7. On the basis of their concentration, bases are classified as:

a. Dilute bases: Have a low concentration of alkali in aqueous

solutions.

b. Concentrated bases: Have a high concentration of alkali in

aqueous solutions.

8. Acids and bases conduct electricity because they produce ions in

water. There is a flow of electric current through the solution by ions.

9. Indicators are those chemical substances which behave differently in

acidic and basic medium and help in determining the chemical nature

of the substance. Acid base indicators indicate the presence of an acid

or a base by a change in their colour or smell.

10. Indicators can be natural or synthetic.

11. Olfactory indicators: These are those indicators whose odour changes

in acidic or basic medium. Example: onion

12. Onion: Smell of onion diminishes in a base and remains as it is in an

acid.

13. Vanilla essence: The odour of vanilla essence disappears when it is

added to a base. The odour of vanilla essence persists when it is added

to an acid.

14. Turmeric: In acids, yellow colour of turmeric remains yellow. In bases,

yellow colour of turmeric turns red.

15. Litmus: Litmus is a natural indicator. Litmus solution is a purple dye

which is extracted from lichen. Acids turn blue litmus red. Bases turn

red litmus blue. Water is essential for acids and bases to change the

colour of litmus paper. Remember that litmus paper will act as an

indicator only if either the litmus paper is moist or the acid or base is

in the form of aqueous solution. This is because acids and bases

release H+

and OH-

ions respectively in aqueous solutions.

16. Phenolphthalein: Phenolphthalein remains colourless in acids but turn

pink in bases.

17. Methyl orange: Methyl orange turns pink in acids and becomes yellow

in bases.Get the Power of Visual Impact on your side

18. Reaction of acids and bases with water:

Acids Bases

Release H+

or H3O

ions in water Release OH-

ions in water

HCl + H2O → H3O

+ Cl- NaOH(s) Na (aq) OH (aq) → + H O2 + −

19. Reaction of acids and bases with metals:

Metals displace hydrogen from the acids and form salt and hydrogen

gas. This is a displacement reaction. So, acids react with only those

metals which are placed above hydrogen in the reactivity series so that

metals can displace hydrogen from acids.

Zn + H2SO4 → ZnSO4 + H2

Metal Acid Salt Hydrogen gas

Bases react with some metals to form salt and hydrogen gas.

Zn + 2 NaOH → Na2ZnO2 + H2

Metal Base Sodium Hydrogen gas

zincate

(salt)

Bases do not react with all the metals to form salt and water.

20. Reaction of acids and bases with metal carbonates:

Acids react with metal carbonate to form salt, water and release

carbon dioxide.

Na CO 2HCl 2 NaCl CO H O 2 3 + → + +2 2

Bases do not react with metal carbonates.

21. Reaction of acids and bases with metal bicarbonates:

Acids react with metal bicarbonate to form salt, water and release

carbon dioxide.

NaHCO HCl NaCl CO H O 3 2 2 + → + +

Bases do not react with metal bicarbonates.

22. Reaction of acids with bases: Neutralisation reaction:

Acids react with bases to form salt and water.

HCl + NaOH → NaCl + H2O

H+

+OH- → H2O

23. Reaction of acids with metallic oxides:

Metallic oxides are basic. Therefore, acids react with metallic oxides to

form salt and water.

HCl + CuO → CuCl2 + H2O Get the Power of Visual Impact on your side

24. Reaction of bases with non-metallic oxides: Non – metallic oxides are

acidic in nature. Bases react with non- metallic oxides to form salt and

water. Example: CO2

Ca(OH)2 + CO2 → CaCO3 + H2O

25. Amphoteric oxides: Oxides which show acidic as well as basic

properties. For example: ZnO, Al2O3

HCl + ZnO → ZnCl2 + H2O

Zn + 2 NaOH → Na2ZnO2 + H2O

26. Neutral oxides: Oxides which are neither acidic nor basic are called

neutral oxides. Example: CO

27. pH: It is used to find out the strength of acids and bases i.e., how

strong or weak the acid or a base is. p in pH stands for ‘potenz’ in

German. The strength of acids and bases depends on the number of

ions and OH-

ions produced respectively.

28. pH scale: A scale for measuring hydrogen ion concentration in a

solution is called pH scale.

29. On pH scale, we measure pH from 0 to 14.

pH value:

pH Type of solution

Less than 7 Acidic

Equal to 7 Neutral

More than 7 Basic

30. More the hydrogen ion (or hydronium ion) concentration, lower is the

pH value.

31. More the hydroxyl ion concentration, higher is the pH value.

32. Variation in pH:

33. Acids which produce more hydrogen ions are said to be strong acids

and acids which produce less hydrogen ions are said to be weak acids.

In other words, strong acids have a lower pH value than weak acids.34. Bases which produce more hydroxyl ions are said to be strong bases

and bases which produce less hydroxyl ions are said to be weak bases.

In other words, strong bases have a higher pH value than weak bases.

35. Living organisms are pH sensitive. Human body works within a pH

range of 7.0 to 7.8.

36. Rain water with a pH less than 5.6 is called acid rain. This acid rain if it

flows into river water makes the survival of aquatic life difficult.

37. Plants also require a specific pH range of soil for their healthy growth.

38. pH of our digestive system: Our stomach produces hydrochloric acid

for digestion of food. But during indigestion, excess of acid is produced

in the stomach and therefore, the pH decreases. This causes pain and

irritation. So, to neutralise this excess acid, a mild base is used. This

mild base works as an antacid. An antacid is any substance, generally

a base or basic salt, which counteracts stomach acidity.

39. Tooth decay: Tooth decay starts when the pH of the mouth is lower

than 5.5. Tooth enamel is made up of calcium phosphate which is the

hardest substance in the body. It does not dissolve in water, but is

corroded when the pH in the mouth is below 5.5. If food particles

remain in the mouth after eating, bacteria present in our mouth

produce acid by degradation of sugar. This decreases the pH of mouth

and hence tooth decay occurs. The best way to prevent this is to clean

the mouth after eating food. Using toothpastes, which are generally

basic, for cleaning the teeth can neutralise the excess acid and prevent

tooth decay.

40. pH is also significant as it is used in self defence by animals and

plants. Bees use acids in their sting. To neutralise the effect a mild

base like baking soda can be used.

41. Sodium hydroxide (NaOH)

Preparation:

Chlor Alkali process:

In this process, electricity is passed through an aqueous solution of

Sodium chloride (called brine). Sodium chloride decomposes to form

sodium hydroxide. Chlorine gas is formed at the anode, and hydrogen

gas at the cathode. Sodium hydroxide solution is formed near the

cathode.

2NaCl(aq) + 2 H2O (l) → 2NaOH(aq) + Cl2(g) + H2(g)

42. Bleaching powder: Bleaching powder is represented as CaOCl2, though

the actual composition is quite complex.

Preparation: Bleaching powder is produced by the action of chlorine on

dry slaked lime. Get the Power of Visual Impact on your side

Ca(OH)2 + Cl2 → CaOCl2+ H2O

43. Baking soda: Sodium hydrogen carbonate (NaHCO3)

Preparation:

NaCl + H2O + CO2+ NH3 → NH4Cl + NaHCO3

44. Washing soda: Sodium carbonate Na2CO3 .10H2O

Preparation:

In the first step, sodium carbonate is obtained by heating baking

soda.

2 NaHCO3 → Heat Na2CO3 + H2O + CO2

Then washing soda is produced by recrystallisation of sodium

carbonate.

Na2CO3 + 10H2O → Na2CO3 .10H2O

45. Plaster of Paris: Calcium sulphate hemihydrate CaSO4. ½ H2O

Preparation: Plaster of Paris is prepared by heating Gypsum at 373K.

CaSO4. 2H2O → Heat at 373K CaSO4. ½ H2O + 1½ H2O

46. Water of crystallisation: It is the fixed number of water molecules

present in one formula unit of a salt.