Organic Chemistry Acids presentation

2. Learning Objectives:-
Definition
Nomenclature
Classification with their Uses
Reactions
Nature of Acids
Types with their Structures
Factors affecting Strength of Acids
Indicators

3. Introduction:-
An Acid is any hydrogen containing
substance that is capable of donating a
proton or hydrogen Ion to another
substance.

4.  The word “Acid” is derived from
Latin word “ACIDUS” meaning
“SOUR”
 It refers to the sharp odor and sour
taste of many acids

5. Arrhenius Definition:-
Any substance that , when dissolved in water, increases the
concentration of hydronium ion (𝐻3𝑂+
) is called an Acid.
Thus Acids are proton donors or electrons acceptors.
EXAMPLES:-
𝐻2S𝑂4, HCl, C𝐻3COOH

6. Nomenclature

14. Binary Acids
It is an acid which consists of only two elements, of
which one is hydrogen and the second is a non metal
element.
EXAMPLES:-
HCl, HF, HI

15. Oxyacid
It is an acid which consists of more than two
elements, of which one is hydrogen, one is oxygen
and at least one is other element
EXAMPLES:-
𝐻2S𝑂4, 𝐻3P𝑂4, HN𝑂3

17. Based on Chemical Reactions
Lewis Acid:
A compound or ionic specie which can accept an electron
pair from a donor compound.
EXAMPLE:
C𝑢2
, 𝐹𝑒2+
, 𝐹𝑒3+
Uses:
Used as ligands in coordination chemistry

18. Lowry- Bronsted acid
A substance which donates an 𝐻+
ion or a
proton and forms its conjugate base.
EXAMPLE:-:
HCl, C𝐻3COOH, N𝐻3

19. Arrhenius Acid:-
A substance which has a hydrogen atom and can
easily give hydrogen ion or proton in its aqueous
solution.
EXAMPLES
𝐻2S𝑂4, HBr

20. Based on origin:-
Mineral Acid:
It is any acid derived from any inorganic compound that dissociates to
produced hydrogen ions in water.
EXAMPLES
𝐻2S𝑂4, HN𝑂3
Uses:
In Chemical Industry as feed stocks for the synthesis of other
chemicals, both organic and inorganic.

21. Organic Acid:
An organic compound that is characterized by weak acidic
properties and does not dissociate completely in the presence of
water.
EXAMPLES:-
C𝐻3𝐶𝑂𝑂𝐻, 𝐶2𝐻2𝑂4
Uses:
In foods as acidulants, flavourants, or preservatives, inactivating or
inhibiting the growth of spoilage microorganisms.

22. Based on acidic strength:-
Strong Acid:
An acid that is completely dissociated in an aqueous solution. It is a
chemical specie with a high capacity to lose proton.
EXAMPLES:
HCl, HBr
Uses:
In batteries, used to start vehicle motors
In the industrial production of explosives, dyes, paints and
fertilizers

23. Weak Acid:-
An acid that does not completely dissociate in solution.
EXAMPLE:-
C𝐻3𝐶𝑂𝑂𝐻, 𝐻3𝑃𝑂4
Uses:
In the preservation of acid foods, due to effective
antimicrobials in their protonated form

24. Based on number of protons donated

25. Reactions of Acids
Types:-
Reactions with metals
Reactions with bases
Reactions with ammonia

26. Reactions with Metals

27. Reactions with Bases

28. Reactions with Ammonia

29. Nature Of Acids
Sour Taste
Turns Blue Litmus Red
Turns Methyl Orange to Red
Acids are Electrolyte
Strong Acids Destroy Fabric
PH Less than 7
Cause Burn on Skin

30. Types Of Acids:-

35. Factors Affecting the Strength of Acids:
Strength of H-A Bond
Polarity of H-A Bond
Oxidation Number

36. Strength of H-A Bond:
Acidic Strength ∝
1
𝑆𝑡𝑟𝑒𝑛𝑔𝑡ℎ 𝑜𝑓 𝐻−𝐴 𝐵𝑜𝑛𝑑
Dominate to decide acid strength of the
elements of same GROUP
H-F H-Cl H-Br H-I

37. Polarity of H-A Bond:
Strength of Acid ∝ Polarity of H-A Bond
Decide strength of acids of elements in the
same PERIODS.
B𝐻3 C𝐻4 N𝐻3 𝑂2H HF

38. Oxidation State:
Oxidation State ∝ Acid Strength
 Oxidation State increases along the Period
thus acidic character increases along the period

39. Indicators

40. Natural Indicators

41. Natural Indicators

42. Synthetic indicators

43. Olfactory Indicators