This document discusses acids, bases and buffers. It begins by defining acids and bases according to four main theories: traditional theory, Arrhenius theory, Bronsted-Lowry theory and Lewis theory. It then discusses the properties and uses of several specific acids and bases, including boric acid, hydrochloric acid, strong ammonium hydroxide, calcium hydroxide and sodium hydroxide. Finally, it defines buffers and buffer capacity, describes different types of buffers, and explains the role and selection factors of buffers.
Chapter No 1 : Acids, Bases and BuffersChetan Jain
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
Chem 132 principles of chemistry lab ii montgomeryAtherstonez
FOR MORE CLASSES VISIT
tutorialoutletdotcom
Principles of Chemistry Lab II Montgomery College, Rockville
Acids and Bases, pH, Buffers and Hydrolysis Introduction
Acids and Bases
Aqueous solutions of acids and bases are recognized as “acidic” or “basic” because they contain
appreciable concentrations of either hydronium (H3O+) or hydroxide (OH–) ions. Hydronium ions are
produced from the reaction of covalent molecules like HCl with water.
Chapter No 1 : Acids, Bases and BuffersChetan Jain
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
Chem 132 principles of chemistry lab ii montgomeryAtherstonez
FOR MORE CLASSES VISIT
tutorialoutletdotcom
Principles of Chemistry Lab II Montgomery College, Rockville
Acids and Bases, pH, Buffers and Hydrolysis Introduction
Acids and Bases
Aqueous solutions of acids and bases are recognized as “acidic” or “basic” because they contain
appreciable concentrations of either hydronium (H3O+) or hydroxide (OH–) ions. Hydronium ions are
produced from the reaction of covalent molecules like HCl with water.
Acids, Bases And Buffers Pharmaceutical Inorganic chemistry UNIT-II (Part-I)
Acids, Bases are defined by Four main theories,
1.Traditional theory / concept
2.Arrhenius theory
3.Bronsted and Lowry theory
4.Lewis theory
Importance of acids and bases in pharmacy
Buffers: Buffer action
Buffer capacity Buffers system
Types of Buffers : Generally buffers are of two types:
1. Acidic buffers
2. Basic buffers
There are some other buffer system:
3. Two salts acts as acid-base pair. Ex- Potassium hydrogen phosphate and potassium dihydrogen phosphate.
4. Amphoteric electrolyte. Ex- Solution of glycine.
5. Solution of strong acid and solution of strong base. Ex- Strong HCl with KCl Mechanism of Buffer action: Mechanism of Action of acidic buffers: Buffer equation-Henderson-Hasselbalch equation:
Standard Buffer Solutions Preparation of Buffer Solutions: Buffers in pharmaceutical systems or Application of buffer: Stability of buffers Buffered isotonic solution Types of Buffer Isotonic solution
1. Isotonic Solutions:
2. Hypertonic Solutions:
3. Hypotonic Solution:
Measurement of Tonicity: 1. Hemolytic method: 2. Cryoscopic method or depression of freezing point:
Methods of adjusting the tonicity:
Class I methods:
In this type, sodium chloride or other substances are added to the solution in sufficient quantity to make it isotonic. Then the preparation is brought to its final volume withan isotonic or a buffered isotonic diluting solution.
These methods are of two types:
Cryoscopic method
Sodium chloride equivalent method.
Class II methods:
In this type, water is added in sufficient quantity make the preparation isotonic. Then the preparation is brought to its volume with an isotonic or a buffered isotonic diluting solution.
These methods are of two types:
White-Vincent method
Sprowls method.
Chapter No 1 : Acids, Bases and BuffersChetan Jain
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
Non- aqueous titrations are those in which the titrations of too weakly acidic or basic substances are carried out using non-aqueous solvents so as to get sharp end point.
Such titrations can also be used for the titration of the substances not soluble in water.
The speed, precision and accuracy of the non-aqueous method are close to those of classical acidimetric and alkalimetric titrations.
First reported successful quantitative titration of organic acid and base in non-aqueous solvent: 1910.
To an understanding of non-aqueous acid base titrimetry the theories of acid and base is very important. The theories are:
Acids are hydrogen containing compounds that dissociates to yield hydrogen ions (H+) when dissolved in water.
Bases are compounds that dissociates to yield hydroxide/hydroxyl ions (OH-) when dissolved in water.
Volumetric Analysis
Titration Basics
Reaction, End point & Indicators
Types of Titrations
Acid – Base Theory & Principles
Acid Base titration
Non- Aqueous Titration
Precipitation Titration
Complexometric Titration
Oxidation- Reduction Titration
Calculation
General Information
Errors
Volumetric Analysis
Types of titration
Acid- Base Theory
Reaction, End Point & Indicators
Acid- Base titration
Titration curve
Non- Aqueous Titration
Precipitation Titration
Complexometric Titration
Oxidation- Reduction Titration,
Calculation. Errors
General Informations,
Acids, Bases And Buffers Pharmaceutical Inorganic chemistry UNIT-II (Part-I)
Acids, Bases are defined by Four main theories,
1.Traditional theory / concept
2.Arrhenius theory
3.Bronsted and Lowry theory
4.Lewis theory
Importance of acids and bases in pharmacy
Buffers: Buffer action
Buffer capacity Buffers system
Types of Buffers : Generally buffers are of two types:
1. Acidic buffers
2. Basic buffers
There are some other buffer system:
3. Two salts acts as acid-base pair. Ex- Potassium hydrogen phosphate and potassium dihydrogen phosphate.
4. Amphoteric electrolyte. Ex- Solution of glycine.
5. Solution of strong acid and solution of strong base. Ex- Strong HCl with KCl Mechanism of Buffer action: Mechanism of Action of acidic buffers: Buffer equation-Henderson-Hasselbalch equation:
Standard Buffer Solutions Preparation of Buffer Solutions: Buffers in pharmaceutical systems or Application of buffer: Stability of buffers Buffered isotonic solution Types of Buffer Isotonic solution
1. Isotonic Solutions:
2. Hypertonic Solutions:
3. Hypotonic Solution:
Measurement of Tonicity: 1. Hemolytic method: 2. Cryoscopic method or depression of freezing point:
Methods of adjusting the tonicity:
Class I methods:
In this type, sodium chloride or other substances are added to the solution in sufficient quantity to make it isotonic. Then the preparation is brought to its final volume withan isotonic or a buffered isotonic diluting solution.
These methods are of two types:
Cryoscopic method
Sodium chloride equivalent method.
Class II methods:
In this type, water is added in sufficient quantity make the preparation isotonic. Then the preparation is brought to its volume with an isotonic or a buffered isotonic diluting solution.
These methods are of two types:
White-Vincent method
Sprowls method.
Chapter No 1 : Acids, Bases and BuffersChetan Jain
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
Non- aqueous titrations are those in which the titrations of too weakly acidic or basic substances are carried out using non-aqueous solvents so as to get sharp end point.
Such titrations can also be used for the titration of the substances not soluble in water.
The speed, precision and accuracy of the non-aqueous method are close to those of classical acidimetric and alkalimetric titrations.
First reported successful quantitative titration of organic acid and base in non-aqueous solvent: 1910.
To an understanding of non-aqueous acid base titrimetry the theories of acid and base is very important. The theories are:
Acids are hydrogen containing compounds that dissociates to yield hydrogen ions (H+) when dissolved in water.
Bases are compounds that dissociates to yield hydroxide/hydroxyl ions (OH-) when dissolved in water.
Volumetric Analysis
Titration Basics
Reaction, End point & Indicators
Types of Titrations
Acid – Base Theory & Principles
Acid Base titration
Non- Aqueous Titration
Precipitation Titration
Complexometric Titration
Oxidation- Reduction Titration
Calculation
General Information
Errors
Volumetric Analysis
Types of titration
Acid- Base Theory
Reaction, End Point & Indicators
Acid- Base titration
Titration curve
Non- Aqueous Titration
Precipitation Titration
Complexometric Titration
Oxidation- Reduction Titration,
Calculation. Errors
General Informations,
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Acid-bases-buffers.pptx
1. Presented By
Mrs. Sonawane.M.D. (Pharmaceutical
Chemistry) M.Pharm
Pravara Rural College of Pharmacy,loni
1
ACIDS, BASESAND BUFFERS
2. ACIDS, BASESAND BUFFERS
Mrs. Sonawane M.D.
Assistant Professor
Department of Pharmaceutical Chemistry
M.E.S’s College of Pharmacy, Sonai
2
3. Learning Outcomes
At the end of topic , students are able to …
The learning outcomes are…..
1. Define acids and bases with examples using different theories.
2. Define neutralization reaction with example.
3. Explain the limitations ofArrhenius theory.
4. Define buffer, buffer capacity.
5. Classify buffers with examples.
6. Write the physical and chemical properties, method of
preparation , uses of HCl, BoricAcid,Ammonium Hydroxide,
NaOH and so on.
3
4. Acids,Bases are defined byFour main theories,
1. Traditional theory / concept
2. Arrhenius theory
3. Bronsted and Lowry theory
4. Lewis theory
4
5. 1. Traditional theory / concept -Acid:
Acids: are the substances
Which converts blue litmus paper to red
Having the PH <7
Sour taste
React with bases to form salts and water
Eg :- Hydrochloric acid (HCl)
5
6. Base: are the substances
Which converts red litmus paper to blue
Having the PH >7
Bitter taste
React withAcids to form salts and water
Eg: Sodium Hydroxide (NaOH)
1. Traditional theory / concept -Base:
6
7. 2. Arrhenius theory:
In 1884 of SvanteArrhenius stated the theory
Also known as,
a)Arrhenius theory of ionization
b)Electron dissociation theory
This theory define acids & bases according to there
formation of ions when dissolved in water
7
8. Acids:
“AnAcid is a substance that can release hydrogen ion
(H+) when dissolved in water” or
“A substance which when dissolved in water gives
hydrogen ions (H+) is known as acid”
Eg: Hydrochloric acid.
2. Arrhenius theory- Acids
HCl H
+
+ Cl
-
8
9. Base:
“ABase is a substance that can release a Hydroxyl ion
(OH-) when dissolved in water” or
“A substance which when dissolved in water gives
Hydroxyl ion(OH-)is known as Base”
Eg : Sodium Hydroxide
2. Arrhenius theory- Base
NaOH Na + O H
+ -
9
10. Acid react Base
Salt & Water
Eg: Hydrochloric acid react sodium hydroxide
Sodium chloride (Salt) & water
Neutralization reaction
NaOH + HCl
Base acid
NaCl + H2O
salt
10
11. “Neutralization as the process in which hydrogen ion
and hydroxyl ion combine to form unionized
molecule or water”
According to Arrhenius theory,
HCl
NaOH
-
NaOH + HCl NaCl + H2O
H
+
+ Cl
-
H
+
+ OH
-
Na
+
+ OH
H2 O
11
12. Limitations:
1. Water is essential
2. Not explain acidity or basisity of non aqueous
Solvent Eg :benzene
3. Basisity ofAmmonia (No OH- ion)is not explained
4. Acidity of BF3,AlCl3 (No H+ ion)is not explained
5. Acidity of oxides of P block element (CO2) is
not explained
6. Basicity of oxides of S block element (Na2o) is
not explained
7. Neutralization with out absence of solvent is not
explained
12
13. 3. Lowry Bronsted theory:
Proton theory of acids and bases
In 1923 the Danish chemist Johannes Nicolaus Bronsted
and the English chemist Thomas Martin Lowry, proposed
the theory
Acid:Acid is the substance which donate proton
Base: Base is the substance which accept proton.
13
14. 1. Amphoteric: a species that can act as an acid or a
base water is an example of an amphoteric species.
2. Conjugate base: species that remains after an acid
donates its H+.
3. Conjugate acid: species that forms after a base
accepts a H+
Some terminology:
14
15. 4. Lewis theory:
In 1923 of scientist G.N. Lewis proposed the theory in
terms of chemical structure
Acid: acid is the molecule or ion that accept the lone pair of
electrons.
Example: H+, NH4+, Na+, Cu++,Al+++
Base: Base is the molecule or ion that donate the lone pair
of electrons.
Example: OH-, Cl-, CN-
15
17. Buffers:
• A buffer is a solution that can resist pH change upon
the addition of an acidic or basic components.
• It is able to neutralize small amounts of added acid or
base, thus maintaining the pH of the solution relatively
stable.
• This is important for processes and/or reactions which
require specific and stable pH ranges.
17
18. A buffer system can be made of a weak acid and its salt or a weak
base and its salt.
A classic example of a weak acid based buffer is acetic acid
(CH3COOH) and sodium acetate (CH3COONa).
A common weak base buffer is made of ammonia (NH3) and
ammonium chloride (NH4Cl)
Buffers system:
18
19. Types of Buffers :
1. On the basis of chemical nature:
a) Acidic buffers
b) Basic buffers
c) Neutral buffers
2. On the basis of use:
a) Analytical buffers
b) Pharmaceutical buffers
19
20. 1. On the basis of chemical nature:
a) Acidic buffers-It is combination of weak acid and its
corresponding salt .
Ex. Mixture of acetic acid, sodium acetate
b) Basic buffers- buffers-It is combination of weak base and its
corresponding salt .
Ex. Mixture ofAmmonium hydroxide and ammonium chloride
c) Neutral buffers: It is single substance showing properties of
buffers.
Ex.Ammonium acetate
Types of Buffers :
20
21. Buffer Capacity :
It is defined as moles of strong acid or strong base
required to change the pH of 1 lit. solution by 1 unit.
Properties of Buffer :
1. The pH of buffer solution is constant.
2. The pH does not changes with dilution.
3. The pH does not changes with even after addition of
small quantities of acid or bases
21
22. Factors for selection of Buffer :
1. Chemical factors
2. Pharmaceutical factors
Chemical factors:
1. The buffer system should not react with other
chemicals in the preparation.
2. It should have reasonable chemical stability.
3. Buffer capacity depends on absolute concentration
of each buffer compound.
22
23. Pharmaceutical factors:
1. Toxicity of buffers: some of the buffers have
limited use in the pharmaceutical practice because
of there toxicity.
2. Effect on pharmaceutical actions of the
preparation: buffer system should not interact
with the action of ingredient of preparation.
3. Contamination by microorganism.: many buffers
system support the microbial growth as they can
serve as nutrient media for moulds when their Ph is
at neutrality.
Factors for selection of Buffer :
23
24. Role of Buffer :
1. The buffers are in pharmaceutical preparation to ensure
the stable
compounds.
2. Solubility
pH conditions for medicinally active
of many compound is controlled by
providing suitable pH.
3. Color of many compound is pH dependent.
4. pH gives stability to different preparations.
5. It provides patient comfort.
6. Penicillin preparation are stabilized by addition of
carbonates.
7. Citric acid is used for stabilizing milk magnesia.
24
25. Molecularformula/Mol.:H3BO3 / 61.83
Synonym: OrthoboricAcid,Aecidium boricum
Method of Preparation:- Borax with Sulphuric acid in
presence of water
Na2B4O7 + H2SO4 + 5H2O 4H3BO3+ Na2SO4
1. Boric acid :
25
26. Properties :-
a) Physical Properties:
White crystalline powder
Odorless
Soluble in water
Soluble in Ethanol
Soluble in glycerin
26
27. Properties :-
b) Chemical Properties
a) Reaction with turmeric paper: Boric acid turn
into brown color
b) Reaction with glycerin:
Boric acid + glycerin
dissolve
Glyceroboric acid
27
28. c)Action on heating :-
Boric acid (H3BO3)
1000C
Metaboric acid (HBO2)
1600C
Tetra boric acid (H2B4O7)
Up to red hot
Boron trioxide (B2O3)
28
29. Local anti-infective
To maintain acidic pH medium in Medicament
Preparation of buffer solution
In ophthalmic preparation
Dusting powder
Preparation of ointement
Uses :-
Storage :-
“ It should be stored in well closed container at a
cool Place.”
29
31. a) Physical Properties:
Clear colorless liquid
Pungent odour
Miscible with water
Miscible with alcohol
fuming liquid
Properties :-
31
32. Properties :-
b) Chemical Properties:-
i)Reaction with metals :hydrochloric acid react with
sodium gives sodium chloride & evolution of hydrogen
gas.
2Na + 2HCl 2NaCl + H2
ii)Reaction with alkali hydrochloric acid react with
sodium hydroxide gives sodium chloride & water
HCl + NaOH NaCl+ H2O
32
33. 1) As a pharmaceutical aid ( acidifying agent)
2) Solvent in industry
3)For manufacturing of basic pharmaceuticals
4) Reagent in Laboratory
Uses :-
Storage :-
“ It should be stored in well closed container of glass at
a temperature not exceeding 300
C
33
35. a)Physical Properties:
Clear colorless liquid
Pungent odour
Characteristic taste
Miscible with water
Aqueous solution is strongly alkaline in nature
Properties :-
35
36. b) Chemical Properties:-
i) Reaction with acid :
React with acid it form salts and water
NH4OH + HCl NH4Cl + H2O
ii) Reaction with cations :
React with acid it form complex
Properties :-
36
38. “ It should be stored in well closed amber colored
container with a rubber stopper at a cool Place.”
- With iodine (Explosive compound)
- heavy metals, silver salts and tannins
Storage :-
Incompatibility :-
38
41. b) Chemical Properties:-
i)Reaction with hydrochloric acid :On
eaction with hydrochloric acid gives
calcium chloride and water
Ca(OH)2 + 2HCl CaCl2 + 2H2O
ii) Effect of heating :
On strongly heating it looses water and
converted into calcium oxide
Ca(OH)2 Cao + H2O
Properties :-
41
42. Antacid
Astringent
Fluid electrolyte
Emulsifying agent
Absorb carbon dioxide
Making of glass
White washing of cloth
Uses :-
Storage :-
“ It should be stored in air tight container at a
cool Place.”
42
43. Molecularformula/MolNaOH / 40
Synonym: Caustic soda, soda lye
Method of Preparation:By treating sodium carbonate
with lime water
Na2CO3 + Ca(OH)2 2NaOH + CaCO3
5. Sodium Hydroxide :-
43
44. a)Physical Properties:
White amorphous pellets
Slight bitter taste
Soluble in water
Soluble in alcohol
Soluble in glycerin
Deliquescent in nature
Properties :-
44
45. b) Chemical Properties:-
i)Reaction with HCl :Sodium hydroxide react
with Hydrochloric acid gives sodium chloride &
water
HCl + NaOH NaCl+ H2O
ii) Reaction with carbon dioxide:
It absorb carbon dioxide from air to
Na2CO3 + H2O
Properties :-
form sodium carbonate
⚫2NaOH + CO2
45
46. Alkalizing agent
Disinfectant for animal houses
For preparation of soap
Absorb CO2 gas
Common laboratory reagent
Uses :-
“ It should be stored in air tight container at a
cool Place.”
Storage :-
46
47. Common Properties
H3BO3, HCl, NH3 , Ca(OH)2 &NaOH
Colorless or white color
HCl & NH3 : Liquid
H3BO3,Ca(OH)2, NaOH : Solid
characteristic odor
Soluble in water
Soluble in alcohol
(expect calcium Hydroxide)
47