This document discusses carboxylic acids. It provides their structural formulas, naming conventions, acidity, sources, reactions, and uses. Carboxylic acids contain the carboxyl functional group (-COOH). They are named by replacing the ending of the parent alkane with 'oic acid'. Being acidic, they can donate protons and exist in equilibrium between the acid and conjugate base forms. Common reactions include esterification, reactions with alcohols to form esters, and reactions with metal ions or bases to form salts. Important carboxylic acids include acetic acid, which is used widely in food production and manufacturing.

2. Structural Formula Chemical Formula
CH3COOH
or
CH3CO2H
=

3.  Methanoic acid
 Total of one
carbon atom
(meth-)
 C0H1COOH
 Ethanoic acid
 Total of two
carbons atoms
(eth-)
C1H3COOH
 Propanoic acid
 Total of three
carbon atoms
(propan-)
 C2H5COOH
*Take note of the functional group’s location, highlighted by the
dotted box

4.  Replace the ‘e’ with ‘oic acid’ at the end of
the name of the hydrocarbon
Example:
H H
H C C H
H H
ethane
H O
H C C O H
H
ethanoic acid

5. Since these are acidic compounds, therefore easily
lose H+ ion and covert in carboxylate ion (RCOO-)

6.  Hence carboxylic acids can be represented by to
resonance structures.
 COOH is less electrophile than aldehyde and
ketone.
120̊̊
planer structure
sp2 hybridized

7. 1. From primary alcohol and
aldehyde(O)
2. From alkyl benzene(O)
3. From Nitriles and amides ( by
hydrolysis)
4. From Dry ice( by carboxylation of
Grignard reagent)
5. From acyl chlorides and acid
anhydrides( by hydrolysis)
6. From esters ( by hydrolysis)

8. Example- 2-methylbutan-1-ol.

10. n- butylbenzene
Potassium benzoate

11. Chromic acid

12. Eg. CH3 –C≡N (acetonitrile)
CH3- CH2 - C≡N (propanitrile)
(HCl)
(NH4Cl)
(NaOH) (HCl)
Na
+ NaCl

13.  Eg. Phenyl magnesium halide.

14. R- CO – Cl + HOH → R-COOH + HCl
Acyl chloride acid

15. (CH3 –CO-)2O + H2O → 2CH3 –COOH
Ethanoic anhydride ethanoic acid
(C6H5 –CO-)2O + H2O → 2C6H5 –COOH
Benzoic anhydride benzoic acid

16. Ester heated with dil. H2SO4 undergoes
hydrolysis.
R-COOR’ + H2O → R-COOH + R-OH
Ester acid
Eg.

17. C1-C9 acid – colourles liquids (high smell)
C9 – more – wax like solid ( odourless)
B.P.-
-COOH > HC > CHO > RCOR > R-OH
Mass = B.P ( mass increase B.P increase)
Solubility-
Solubility = molar mass
Polarity-
COOH < ROR < R-OH etc.

18.  Because of liquid phase acid shows dimers.
 Vapour phase also show same properties.
 Similarly acid bonding with water molecule.

19. 6-8% acetic acid
Present in water.
Pure acetic acid
Glacial acetic acid
at 289.5K acid
become solid
And water as liquid
by filter
We can remove
acid from
Water.

20. A. Reaction involving Cleavage of OH
bond
B. Reaction involving cleavage of C-OH
bond
C. Reaction involving –COOH bond
D. Substitution reactions

21. (a) Acidity of Carboxylic Acids:
1. Action of active metals
2. Action of alkali on acetic acid
3. Action of sodium carbonate and
sodium bicarbonate on acetic
acid

22.  Carboxylic acids can be easily ionize and exist in a
dynamic equilibrium between the carboxylate ion and
hydronium ion. Hence they show acidic nature.
R COOH + H2O ⇌ RCOO- + H3O+
 The equilibrium constant K for given,
 K = [RCOO−][H3O+][RCOOH][H2O]
Since water present in large excess; the same equation
is written as,

K x [H2O] = [RCOO−][H3O+][RCOOH]

Ka = [RCOO−][H3O+][RCOOH]

23.  Ka show acidic value can also be expressed
in terms of pKa. pKa= -logKa
 Larger the Ka value larger the ion and
stronger the acid.
 Acid is more acidic then phenol and alcohol
because of OH of acid readily loses a H ion
then alcohol and phenol.

24.  Due to Delocalization phenoxide ion is
more stable then phenol.

25. Reaction with metal-Carboxylic acids
react with active metals like; K, Ca, Mg to
form their respective salts and release
hydrogen gas.
2RCOOH + 2Na → 2RCOONa +H2

26. Similarly carboxylic acids react with
alkalis like sodium hydroxide to form
salts and water and show simple acid-
base neutralization reaction.
RCOOH +NaOH → RCOONa + H2O

27. Eg. Acetic acid.
2 H2O2

28. 1. Formation of acyl chloride
2. Formation of ester
3. Formation of anhydrides
4. Formation of amides

30.  Forward rxn called Fischer esterification.
 Reverse rxn called hydrolysis of ester.
 Sulphuric acid acts as catalyst as well as
dehydrating agent.

31. Based on esterification order of reactivity is
1 > 2 > 3 Alcohol
C1 > C2 > C3 etc. Carboxylic acid

32. Step 1 – addition of alcohol to acid group.

33. ROH
ROH2
Step2- Acid catalyzed dehydration

35.  Reversible rxn dehyrating agent P2O5 or conc.
H2SO4.
RCOOH + HOOCR → RCOOCOR+ H2O
Eg.
CH3COOH + HOOCCH3 → CH3COOCOCH3 + H2O

36.  RCOOH + NH3 → RCOO-NH4
+ → RCONH2 + H2O
 RCOOCl + NH3 → RCONH2 + HCl
 Eg. Acetic acid(ethanoic acid)
 First product is NH4acetate and final is
acetamide.
First step is reversible Heat to decompose

37. 1. Formation of Primary
Alcohols (Reduction)
2. Formation of Hydrocarbon
(Decarboxylation)

38.  eg.
Cyclopropane carboxylic acid
diborane

39.  Eg.

40. 1.α – Halogenation
2.Ring substitution

41.  The reaction is called as Hell-Volhard-Zelinsky
reaction.
 it takes place with Cl or Br in the presence of
small quantities of red phosphorus.
 Attack take place only α – H-atom.
HCl

43.  Carboxylic acids do not undergo the Friedel
Crafts reaction because the carboxyl group is
deactivating and the catalyst Aluminium
chloride which is a Lewis acid will reacts with
Carboxyl group.

44. Ethanoic acid(acetic acid) is the most
important organic acid
It is used in vinegar as preservative and
flavourings.

48. Making of drugs, dyes, paints, insecticides,
plastics.
Making of esters.

49. Organic
acid
Where it is found
Lactic acid Sour milk
Oxalic acid Rhubarb plant
Citric acid Limes, lemons
Formic acid Insect bites
Tartaric
acid
Grape juice
Acetic acid Vinegar
Malic acid Apples and pears