This document provides an overview of gastrointestinal agents used to treat various gastrointestinal disorders. It discusses acidifiers that increase acid in the stomach and are used to treat achlorhydria. It also covers antacids that neutralize excess stomach acid and are used for hyperacidity/hyperchlorhydria. Finally, it discusses cathartics/laxatives that relieve constipation through increasing bowel movements. Specific agents covered include ammonium chloride, dilute hydrochloric acid, sodium bicarbonate, aluminum hydroxide gel, and magnesium hydroxide mixture.
Non-aqueous titration is used when reactants are insoluble or reactive with water, or are very weak acids or bases that do not fully dissociate. Water is replaced by other solvents like perchloric acid. Non-aqueous titration can estimate weak acids and bases that cannot be easily titrated in water due to its amphoteric nature. Common types of non-aqueous titration include acidimetry, using acidic solvents and perchloric acid as the titrant to estimate weak bases, and alkalimetry, using basic solvents and sodium methoxide as the titrant to estimate weak acids.
This document discusses non-aqueous titration including reasons for using non-aqueous solvents, common solvent types, and examples of acidimetry and alkalimetry titrations. Protogenic, protophilic, and aprotic solvents are described. Acidimetry involves titrating weak bases like ephedrine HCl with perchloric acid in glacial acetic acid. Alkalimetry involves titrating weak acids like sodium benzoate with sodium methoxide in DMF. The document provides procedures for standardizing a perchloric acid solution and estimating the percentage of ephedrine HCl and sodium benzoate in samples.
The document discusses the limit test for chloride. It defines a limit test as a quantitative or semi-quantitative test to identify and control small amounts of impurities likely to be present in a substance. The limit test for chloride determines the allowable limit of chloride in a sample. It involves dissolving the sample and standard sodium chloride solution, adding nitric acid and silver nitrate, and observing any opalescence or turbidity after 3 minutes. The sample passes the limit test for chloride if the opalescence is less than or equal to the standard solution.
The document provides information on the preparation, properties, assays, and uses of several inorganic compounds including sodium chloride, calcium gluconate, ammonium chloride, sodium bicarbonate, hydrogen peroxide, chlorinated lime, copper sulphate, ferrous sulphate, and sodium thiosulphate. For each compound, methods of preparation, physical and chemical properties, assay methods (often titration based), and common uses are described. The compounds discussed are commonly used in pharmaceutical, medical, industrial, and laboratory applications.
pharmacopoeia and monograph, pharmaceutical inorganic chemistrynehla313
The document discusses various pharmacopoeias including the Indian Pharmacopoeia, British Pharmacopoeia, and United States Pharmacopoeia. It provides details on the history, editions, contents and features of these pharmacopoeias. The key points are:
- Pharmacopoeias are official books that provide drug standards and monographs. They are usually issued by government authorities.
- The first edition of the Indian Pharmacopoeia was published in 1955. It has since been revised periodically with additions of new monographs and analytical methods.
- The British Pharmacopoeia was first published in 1864 and has been published annually since 1953. It contains over 3,000 monographs for substances
This document discusses various types of cathartics/laxatives including bulk forming, stimulant, stool softeners, and osmotic laxatives. It provides examples of specific cathartics that fall into each category such as magnesium sulfate, sodium orthophosphate, kaolin, and bentonite. Details are given on the properties, identification tests, uses and methods of preparation/assay for some of these cathartic agents. Constipation and the role of laxatives in treating it are also briefly covered.
This document provides information on saline cathartics, also known as osmotic laxatives. Saline cathartics work by drawing water from the circulation into the gastrointestinal tract through osmosis, which increases intestinal bulk and produces diarrhea. Two examples are discussed in detail: magnesium sulfate (Epsom salt) and sodium potassium tartrate. Magnesium sulfate occurs as colorless needle-like crystals with a bitter taste. It is used to treat constipation and electrolyte deficiencies. Sodium potassium tartrate, also called Rochelle salt, is obtained by neutralizing sodium carbonate with potassium bitartrate and is used as a laxative and food additive.
Non-aqueous titration is used when reactants are insoluble or reactive with water, or are very weak acids or bases that do not fully dissociate. Water is replaced by other solvents like perchloric acid. Non-aqueous titration can estimate weak acids and bases that cannot be easily titrated in water due to its amphoteric nature. Common types of non-aqueous titration include acidimetry, using acidic solvents and perchloric acid as the titrant to estimate weak bases, and alkalimetry, using basic solvents and sodium methoxide as the titrant to estimate weak acids.
This document discusses non-aqueous titration including reasons for using non-aqueous solvents, common solvent types, and examples of acidimetry and alkalimetry titrations. Protogenic, protophilic, and aprotic solvents are described. Acidimetry involves titrating weak bases like ephedrine HCl with perchloric acid in glacial acetic acid. Alkalimetry involves titrating weak acids like sodium benzoate with sodium methoxide in DMF. The document provides procedures for standardizing a perchloric acid solution and estimating the percentage of ephedrine HCl and sodium benzoate in samples.
The document discusses the limit test for chloride. It defines a limit test as a quantitative or semi-quantitative test to identify and control small amounts of impurities likely to be present in a substance. The limit test for chloride determines the allowable limit of chloride in a sample. It involves dissolving the sample and standard sodium chloride solution, adding nitric acid and silver nitrate, and observing any opalescence or turbidity after 3 minutes. The sample passes the limit test for chloride if the opalescence is less than or equal to the standard solution.
The document provides information on the preparation, properties, assays, and uses of several inorganic compounds including sodium chloride, calcium gluconate, ammonium chloride, sodium bicarbonate, hydrogen peroxide, chlorinated lime, copper sulphate, ferrous sulphate, and sodium thiosulphate. For each compound, methods of preparation, physical and chemical properties, assay methods (often titration based), and common uses are described. The compounds discussed are commonly used in pharmaceutical, medical, industrial, and laboratory applications.
pharmacopoeia and monograph, pharmaceutical inorganic chemistrynehla313
The document discusses various pharmacopoeias including the Indian Pharmacopoeia, British Pharmacopoeia, and United States Pharmacopoeia. It provides details on the history, editions, contents and features of these pharmacopoeias. The key points are:
- Pharmacopoeias are official books that provide drug standards and monographs. They are usually issued by government authorities.
- The first edition of the Indian Pharmacopoeia was published in 1955. It has since been revised periodically with additions of new monographs and analytical methods.
- The British Pharmacopoeia was first published in 1864 and has been published annually since 1953. It contains over 3,000 monographs for substances
This document discusses various types of cathartics/laxatives including bulk forming, stimulant, stool softeners, and osmotic laxatives. It provides examples of specific cathartics that fall into each category such as magnesium sulfate, sodium orthophosphate, kaolin, and bentonite. Details are given on the properties, identification tests, uses and methods of preparation/assay for some of these cathartic agents. Constipation and the role of laxatives in treating it are also briefly covered.
This document provides information on saline cathartics, also known as osmotic laxatives. Saline cathartics work by drawing water from the circulation into the gastrointestinal tract through osmosis, which increases intestinal bulk and produces diarrhea. Two examples are discussed in detail: magnesium sulfate (Epsom salt) and sodium potassium tartrate. Magnesium sulfate occurs as colorless needle-like crystals with a bitter taste. It is used to treat constipation and electrolyte deficiencies. Sodium potassium tartrate, also called Rochelle salt, is obtained by neutralizing sodium carbonate with potassium bitartrate and is used as a laxative and food additive.
The document discusses non-aqueous titration. It describes how non-aqueous titration is used to titrate weakly acidic or basic substances using non-aqueous solvents instead of water to obtain sharp endpoints. It discusses solvent selection and properties like dissociation ability, dielectric constant, and acid/base character. It also describes methods for determining the endpoint, including indicator methods and potentiometry. An example procedure is given for the estimation of sodium benzoate by titrating it with hydrochloric acid in a non-aqueous solvent system.
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.
This document appears to be a list of antimicrobial agents from the year 2016. It includes many entries listing only the year "2016" with no other details provided. The only other entries are "Boric Acid Glycerine" which are listed together without any additional context. In summary, the document seems to be a list of antimicrobial agents and years but provides very little substantive information.
Dental hygiene and products that promote it are important for oral and overall health. There are many dental products on the market, including anticaries agents to prevent tooth decay like fluoride and ammoniated toothpastes, dentifrices for cleaning teeth, desensitizing agents for tooth sensitivity, mouthwashes with antiseptic and other properties, and temporary or permanent fillings and cements. Proper dental hygiene can be maintained through the regular use of evidence-based dental products.
This is chapter No 3 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy) Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
This document describes the limit test for sulfate. The test is based on the reaction between barium chloride and soluble sulfates in the presence of hydrochloric acid. This results in the precipitation of barium sulfate. The turbidity produced by the test solution is compared to that of a standard sulfate solution. If the turbidity of the test solution is less than the standard, then the sample passes the limit test for sulfate.
This document discusses pharmaceutical impurities. It defines impurity as unwanted foreign particles other than the active drug. Impurities can come from raw materials, reagents, manufacturing processes, storage conditions, or deliberate adulteration. The types and amounts of impurities depend on factors like purity of starting materials and purification methods. Limit tests are used to detect and limit specific impurities like chlorides, sulphates, and iron according to pharmacopeia limits. The tests use reactions like precipitation or color changes to compare a sample to a standard of a known impurity level. Maintaining low impurity levels is important for safety, efficacy, and stability of pharmaceutical products.
Major extra and intracellular electrolytes. Pharmaceutical Inorganic chemistr...Ms. Pooja Bhandare
Major extra and intracellular electrolytes. Pharmaceutical Inorganic chemistry UNIT-II (Part-II)
Electrolyte: Intracellular fluid
Interstitial fluid
Plasma (Vascular fluid)
Anionic electrolytes- HCO₃⁻, Cl⁻, SO₄²⁻, HPO₄²⁻
Cationic electrolytes- Na⁺, K⁺, Ca²⁺, Mg²⁺
Concentration of important Electrolytes:
Electrolytes used in the replacement therapy: Sodium
chloride*, Potassium chloride, Calcium gluconate* and Oral Rehydration Salt
(ORS), Physiological acid base balance.
Anatacid || B pharmacy First Year || Presentation || kkwagh ||
This presentation is helpful for your study
This Presentation Contain
• Introduction
• characteristics of ideal antacid
• classification of antacid
• Some common use antacid
Practical notes for Pharmacy (Synopsis and viva questions included) reference...Payaamvohra1
This document provides practical tips and guidance for first semester pharmacy students according to the PCI syllabus. It outlines important topics to study in subjects like Human Anatomy and Physiology, Pharmaceutical Analysis, Pharmaceutics, and Pharmaceutical Inorganic Chemistry. These include experiments, formulations, limit tests, and preparations. It also recommends books for remedial math and biology, focusing on topics like body fluids, respiration, photosynthesis, limits, and differentiation. The goal is to help students understand the essential theoretical and practical components of the syllabus.
Non-aqueous titration has several advantages over aqueous titration including enabling the titration of organic acids and bases that are insoluble in water. Key types of non-aqueous solvents used in titration include aprotic, protogenic, protophillic, and amphiprotic solvents. Common indicators used in non-aqueous titration include crystal violet and oracet blue B. Example applications of non-aqueous titration include determination of active ingredients in pharmaceutical preparations like ephedrine and codeine. Proper preparation and standardization of titrants such as perchloric acid in acetic acid or potassium methoxide in toluene-methanol is important for accurate non-aqueous tit
Buffer solutions maintain a fairly constant pH even when small amounts of acid or base are added. There are isotonic, hypotonic, and hypertonic solutions depending on their solute concentration compared to blood or other fluids. Buffer solutions are important for intravenous injections, which should be isotonic with blood plasma. Tonicity can be measured using haemolytic or colligative methods. The colligative method involves measuring properties like freezing point depression, which should be -0.52°C for a solution to be considered isotonic with blood plasma. Calculating tonicity is important for parenteral and ophthalmic preparations.
In this experiment I have provided the complete information regarding limit test for sulphate and also preparation of 0.1 N sulphuric acid and barium sulphate reagent for your better understanding.
Arsenic is well known under desirable hand harmful due to its toxic nature, it poses the serious health hazard, which is present in medical substance, many qualitative and quantitative test for arsenic known, however Pharmacopoeia method is based on ‘Gutzeit Method’.
Concentration of arsenic beyond 0.01 mg/L in pollutant by the World Health Organization (WHO).
Reasons:
• Stannous chloride is used for complete evolution of arsine.
• Zinc, potassium iodide and stannous chloride is used as a reducing agent.
• Hydrochloride acid is used to make the solution acidic.
• Lead acetate pledger or papers are used to trap any hydrogen sulphide, which may be evolved along with arsine.
This document provides information on various pharmaceutical compounds including expectorants, potassium iodide, copper sulfate, iron sulfate, zinc sulfate, and methods for their analysis. It discusses the definition, chemical and physical properties, preparation, uses and assays of these compounds by redox titration, gravimetric analysis, and complexometric titration. The document also covers emetics, astringents, antidotes and poisons including sodium nitrite, sodium thiosulfate and activated charcoal.
This document describes the Gutzeit test for detecting arsenic. The test works by first converting any arsenic in a sample into arsenious acid, then reducing it to arsine gas. Mercuric chloride paper placed in the apparatus will turn yellow if arsine gas is present, indicating the presence of arsenic in the original sample. The document provides details of the test apparatus, reagents used, procedure, and precautions to get accurate results and avoid contamination.
This document discusses posology, which is the science of calculating drug doses. It defines posology and explains that many factors can influence the appropriate dose of a drug for a patient, including age, sex, body weight, route of administration, and medical conditions. The document provides details on calculating doses for children, adjusting for body weight, and determining veterinary doses for animals based on surface area and weight. Overall, the document outlines the key principles of posology and the various considerations involved in accurately prescribing medication doses for both human and animal patients.
This document discusses electrolyte replacement therapy and lists three common electrolyte compounds used: sodium chloride, potassium chloride, and calcium gluconate. Sodium chloride and potassium chloride are described in detail, including their molecular formulas, properties, preparation methods, assays, and uses. Calcium gluconate is also described briefly, noting its use as an electrolyte replenisher and to treat conditions caused by low calcium levels such as osteoporosis and rickets. The main purpose of electrolyte replacement therapy is to restore electrolyte and fluid balance in the body.
Gastrointestinal agents are drugs used to treat gastrointestinal disorders like achlorhydria, hyperacidity, constipation, and diarrhea. Acidifiers increase acid concentration in the GI tract and are used to treat achlorhydria. Dilute hydrochloric acid maintains or increases stomach acid levels and pH. Antacids neutralize excess stomach acid in hyperacidity. Common acidifiers and antacids include ammonium chloride, dilute hydrochloric acid, and sodium bicarbonate.
Major intra & extra cellular electrolytes ATTRIRAKESH1
This document discusses various electrolytes used in acid-base therapy and their properties and uses. It describes sodium acetate, potassium acetate, sodium bicarbonate, sodium citrate, potassium citrate, sodium lactate, ammonium chloride, and potassium bicarbonate. It also discusses oral rehydration solutions, their formulations and benefits. The World Health Organization recommends reduced osmolarity oral rehydration solutions containing sodium, potassium, citrate, magnesium, zinc, and glucose to effectively treat diarrhea and dehydration.
The document discusses non-aqueous titration. It describes how non-aqueous titration is used to titrate weakly acidic or basic substances using non-aqueous solvents instead of water to obtain sharp endpoints. It discusses solvent selection and properties like dissociation ability, dielectric constant, and acid/base character. It also describes methods for determining the endpoint, including indicator methods and potentiometry. An example procedure is given for the estimation of sodium benzoate by titrating it with hydrochloric acid in a non-aqueous solvent system.
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.
This document appears to be a list of antimicrobial agents from the year 2016. It includes many entries listing only the year "2016" with no other details provided. The only other entries are "Boric Acid Glycerine" which are listed together without any additional context. In summary, the document seems to be a list of antimicrobial agents and years but provides very little substantive information.
Dental hygiene and products that promote it are important for oral and overall health. There are many dental products on the market, including anticaries agents to prevent tooth decay like fluoride and ammoniated toothpastes, dentifrices for cleaning teeth, desensitizing agents for tooth sensitivity, mouthwashes with antiseptic and other properties, and temporary or permanent fillings and cements. Proper dental hygiene can be maintained through the regular use of evidence-based dental products.
This is chapter No 3 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy) Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
This document describes the limit test for sulfate. The test is based on the reaction between barium chloride and soluble sulfates in the presence of hydrochloric acid. This results in the precipitation of barium sulfate. The turbidity produced by the test solution is compared to that of a standard sulfate solution. If the turbidity of the test solution is less than the standard, then the sample passes the limit test for sulfate.
This document discusses pharmaceutical impurities. It defines impurity as unwanted foreign particles other than the active drug. Impurities can come from raw materials, reagents, manufacturing processes, storage conditions, or deliberate adulteration. The types and amounts of impurities depend on factors like purity of starting materials and purification methods. Limit tests are used to detect and limit specific impurities like chlorides, sulphates, and iron according to pharmacopeia limits. The tests use reactions like precipitation or color changes to compare a sample to a standard of a known impurity level. Maintaining low impurity levels is important for safety, efficacy, and stability of pharmaceutical products.
Major extra and intracellular electrolytes. Pharmaceutical Inorganic chemistr...Ms. Pooja Bhandare
Major extra and intracellular electrolytes. Pharmaceutical Inorganic chemistry UNIT-II (Part-II)
Electrolyte: Intracellular fluid
Interstitial fluid
Plasma (Vascular fluid)
Anionic electrolytes- HCO₃⁻, Cl⁻, SO₄²⁻, HPO₄²⁻
Cationic electrolytes- Na⁺, K⁺, Ca²⁺, Mg²⁺
Concentration of important Electrolytes:
Electrolytes used in the replacement therapy: Sodium
chloride*, Potassium chloride, Calcium gluconate* and Oral Rehydration Salt
(ORS), Physiological acid base balance.
Anatacid || B pharmacy First Year || Presentation || kkwagh ||
This presentation is helpful for your study
This Presentation Contain
• Introduction
• characteristics of ideal antacid
• classification of antacid
• Some common use antacid
Practical notes for Pharmacy (Synopsis and viva questions included) reference...Payaamvohra1
This document provides practical tips and guidance for first semester pharmacy students according to the PCI syllabus. It outlines important topics to study in subjects like Human Anatomy and Physiology, Pharmaceutical Analysis, Pharmaceutics, and Pharmaceutical Inorganic Chemistry. These include experiments, formulations, limit tests, and preparations. It also recommends books for remedial math and biology, focusing on topics like body fluids, respiration, photosynthesis, limits, and differentiation. The goal is to help students understand the essential theoretical and practical components of the syllabus.
Non-aqueous titration has several advantages over aqueous titration including enabling the titration of organic acids and bases that are insoluble in water. Key types of non-aqueous solvents used in titration include aprotic, protogenic, protophillic, and amphiprotic solvents. Common indicators used in non-aqueous titration include crystal violet and oracet blue B. Example applications of non-aqueous titration include determination of active ingredients in pharmaceutical preparations like ephedrine and codeine. Proper preparation and standardization of titrants such as perchloric acid in acetic acid or potassium methoxide in toluene-methanol is important for accurate non-aqueous tit
Buffer solutions maintain a fairly constant pH even when small amounts of acid or base are added. There are isotonic, hypotonic, and hypertonic solutions depending on their solute concentration compared to blood or other fluids. Buffer solutions are important for intravenous injections, which should be isotonic with blood plasma. Tonicity can be measured using haemolytic or colligative methods. The colligative method involves measuring properties like freezing point depression, which should be -0.52°C for a solution to be considered isotonic with blood plasma. Calculating tonicity is important for parenteral and ophthalmic preparations.
In this experiment I have provided the complete information regarding limit test for sulphate and also preparation of 0.1 N sulphuric acid and barium sulphate reagent for your better understanding.
Arsenic is well known under desirable hand harmful due to its toxic nature, it poses the serious health hazard, which is present in medical substance, many qualitative and quantitative test for arsenic known, however Pharmacopoeia method is based on ‘Gutzeit Method’.
Concentration of arsenic beyond 0.01 mg/L in pollutant by the World Health Organization (WHO).
Reasons:
• Stannous chloride is used for complete evolution of arsine.
• Zinc, potassium iodide and stannous chloride is used as a reducing agent.
• Hydrochloride acid is used to make the solution acidic.
• Lead acetate pledger or papers are used to trap any hydrogen sulphide, which may be evolved along with arsine.
This document provides information on various pharmaceutical compounds including expectorants, potassium iodide, copper sulfate, iron sulfate, zinc sulfate, and methods for their analysis. It discusses the definition, chemical and physical properties, preparation, uses and assays of these compounds by redox titration, gravimetric analysis, and complexometric titration. The document also covers emetics, astringents, antidotes and poisons including sodium nitrite, sodium thiosulfate and activated charcoal.
This document describes the Gutzeit test for detecting arsenic. The test works by first converting any arsenic in a sample into arsenious acid, then reducing it to arsine gas. Mercuric chloride paper placed in the apparatus will turn yellow if arsine gas is present, indicating the presence of arsenic in the original sample. The document provides details of the test apparatus, reagents used, procedure, and precautions to get accurate results and avoid contamination.
This document discusses posology, which is the science of calculating drug doses. It defines posology and explains that many factors can influence the appropriate dose of a drug for a patient, including age, sex, body weight, route of administration, and medical conditions. The document provides details on calculating doses for children, adjusting for body weight, and determining veterinary doses for animals based on surface area and weight. Overall, the document outlines the key principles of posology and the various considerations involved in accurately prescribing medication doses for both human and animal patients.
This document discusses electrolyte replacement therapy and lists three common electrolyte compounds used: sodium chloride, potassium chloride, and calcium gluconate. Sodium chloride and potassium chloride are described in detail, including their molecular formulas, properties, preparation methods, assays, and uses. Calcium gluconate is also described briefly, noting its use as an electrolyte replenisher and to treat conditions caused by low calcium levels such as osteoporosis and rickets. The main purpose of electrolyte replacement therapy is to restore electrolyte and fluid balance in the body.
Gastrointestinal agents are drugs used to treat gastrointestinal disorders like achlorhydria, hyperacidity, constipation, and diarrhea. Acidifiers increase acid concentration in the GI tract and are used to treat achlorhydria. Dilute hydrochloric acid maintains or increases stomach acid levels and pH. Antacids neutralize excess stomach acid in hyperacidity. Common acidifiers and antacids include ammonium chloride, dilute hydrochloric acid, and sodium bicarbonate.
Major intra & extra cellular electrolytes ATTRIRAKESH1
This document discusses various electrolytes used in acid-base therapy and their properties and uses. It describes sodium acetate, potassium acetate, sodium bicarbonate, sodium citrate, potassium citrate, sodium lactate, ammonium chloride, and potassium bicarbonate. It also discusses oral rehydration solutions, their formulations and benefits. The World Health Organization recommends reduced osmolarity oral rehydration solutions containing sodium, potassium, citrate, magnesium, zinc, and glucose to effectively treat diarrhea and dehydration.
Gastrointestinal agents
Inorganic chemicals used to treat Castro intestinal tract by different class of agents
Acidifying Agents
ANTACID
PROTECTIVE AND ADSORBENTS
SALINE CATHARTICS
Unit-III Gastro-intestinal agent for B&D Pharmacy.pptx by Bulet Kumar GuptaChevallaMaheshwari
The document discusses various agents used to treat gastrointestinal conditions. It describes the anatomy and functions of the gastrointestinal tract. It then discusses different types of gastric antacids including their classification, mechanisms of action, and examples like aluminum hydroxide, magnesium hydroxide, and sodium bicarbonate. It also covers acidifiers, cathartics, and their uses to treat conditions like achlorhydria, constipation, and diarrhea.
This document provides information about gastrointestinal agents (GI agents), which are drugs used to treat GI disorders. It discusses the classifications of GI agents including acidifying agents, antacids, protectives, adsorbents, and cathartics. It then describes common antacids including aluminum hydroxide gel, calcium carbonate, and magnesium salts. The ideal characteristics of antacids are outlined. Common calcium-containing and magnesium-containing antacids are also discussed in more detail.
This document discusses electrolyte replenishers and their uses. It defines electrolytes as minerals in the body that have an electric charge and are present in blood, urine, tissues, and other body fluids. Electrolytes help balance the amount of water in the body. Replacement therapy aims to restore normal volume and composition of body fluids. Various electrolytes used in replacement therapy are discussed, including sodium chloride, potassium chloride, calcium chloride and bicarbonates. Combination electrolyte therapies and oral rehydration salts are also summarized.
The document discusses gastrointestinal agents and provides information about antacids. It defines antacids as alkaline substances used to neutralize hydrochloric acid in the stomach and provides relief from pain caused by excess stomach acid. The summary discusses classification of antacids as systemic or non-systemic based on absorption and criteria for an ideal antacid preparation. It also mentions combination antacid preparations can help avoid side effects of individual compounds.
Cathartics are drugs used to relieve constipation by stimulating bowel movements. They include mild laxatives that soften stool and strong purgatives that cause complete bowel evacuation. Constipation can be caused by factors like weak intestines, diet, drugs, or ignoring the urge to defecate. Cathartics work by irritation, increasing stool bulk, lubrication, or drawing water into the intestines. Common cathartics discussed include magnesium sulfate, sodium phosphate, kaolin, and bentonite.
non aqueous titrations of acid and base .pptxDeepali69
Non-aqueous titrations allow for the titration of substances that cannot be titrated in aqueous solutions, such as mixtures of acids/bases, organic acids/bases insoluble in water, and very weak acids/bases. Solvents used include acetic acid, acetonitrile, alcohols, and DMF. Indicators change color in acidic and basic conditions. Common titrations include primary/secondary/tertiary amines with perchloric acid and acids with sodium/potassium methoxide. Proper preparation of titrants and indicators, choice of solvent, and accounting for temperature effects are important for accurate non-aqueous titrations.
The document discusses the gastrointestinal tract and its components and functions. It then discusses various types of acidifying reagents or acidifiers that can increase acidity in the gastrointestinal tract, including gastric, urinary, and systemic acidifiers. It provides ammonium chloride as an example of an acidifier, discussing its preparation, properties, identification tests, purity tests, and uses to produce mild acidosis.
This document provides information about antacids, including their mechanism of action, classification, and examples. It discusses how antacids work by neutralizing gastric acid through chemical reactions or by forming protective coatings in the stomach. Antacids are classified as systemic or non-systemic. Systemic antacids like sodium bicarbonate can cause alkalosis while non-systemic antacids like aluminum hydroxide, magnesium hydroxide, and magnesium carbonate act locally in the stomach without systemic absorption. Common antacids are discussed in detail with their chemical reactions, effects, uses, and side effects.
Emetics are drugs that induce vomiting by causing the contents of the stomach to be expelled through the mouth. They are important for treating poisoning cases. Copper sulfate is a common emetic that is blue crystalline powder. It can be assayed through an oxidation-reduction titration with iodine and sodium thiosulfate. Sodium potassium tartrate, also known as Rochelle salt, is a crystalline powder that is soluble in water. It has uses as a laxative, diuretic, and food additive.
The document discusses electrolyte replacement therapy used to treat dehydration and describes the concentrations of various electrolytes like sodium, potassium, calcium, and magnesium that must be replaced. It also provides information on common electrolyte solutions used for replacement including their compositions, properties, methods of preparation, and uses. Specific electrolytes discussed in more detail include sodium chloride, potassium chloride, and calcium gluconate.
MAKAUT/SEM 1/ PHARMACEUTICAL INORGANIC CHEMISTRY/ UNIT 3/GASTROINTESTINAL AGENTS_CATHARTICS
BY
KUNAL DATTA
ASSISTANT PROFESSOR
B.PHARM , M.PHARM
NETAJI SUBHAS CHANDRA BOSE INSTITUTE OF PHARMACY
This document discusses several types of gastrointestinal agents including acidifiers, antacids, cathartics, and antimicrobials. It provides details on specific agents such as ammonium chloride, dilute hydrochloric acid, aluminum hydroxide gel, milk of magnesia, sodium bicarbonate, and their uses, preparations, and assays. Antacids are discussed in terms of their ideal properties and combinations used. Acidifiers are described as agents that increase acidity in the gastrointestinal tract for various purposes.
Gastrointestinal agents are classified into different groups based on their mechanism of action. These include acidifying agents, antacids, adsorbents, laxatives, cathartics, purgatives, and protective agents. Acidifying agents like dilute hydrochloric acid are used to increase acid levels in the stomach. Antacids like aluminum hydroxide gel and magnesium hydroxide are used to neutralize excess stomach acid in conditions like hyperacidity. Laxatives, cathartics and purgatives help promote bowel movements and treat constipation.
This document discusses gastrointestinal agents including acidifying agents, antacids, and cathartics. It provides details on various acidifying agents such as ammonium chloride, hydrochloric acid, and dilute hydrochloric acid. It also discusses antacids including sodium bicarbonate, aluminium hydroxide gel, and magnesium hydroxide mixture. Finally, it covers cathartics such as magnesium sulphate, sodium orthophosphate, and kaolin. The document provides information on the uses, properties, preparations and other details of these various gastrointestinal agents.
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2. INTRODUCTION
⚫ The gastrointestinal (GI) tract is composed of various organs and tissues
that have different forms and functions.
⚫ It includes the esophagus, stomach, small intestine, large intestine, colon,
rectum, biliary tract, gallbladder, liver, and pancreas.
⚫ The gastrointestinal track suffers from various disorders likeachlorhydria,
hyperacidity, constipation and diarrhea.
⚫ And these disorder s treated with the help of some substances or agent
called as gastrointestinal agents.
GASTROINTESTINAL AGENTS:
⚫ These are the drugs or substances which are used in treatment of various
types of gastrointestinal disorders such as achlorhydria, hyperacidity,
constipation and diarrhea.
3.
4. 1.ACIDIFYING AGENT OR ACIDIFIERS
⚫ Acidifiers or Acidifying agents are the inorganic agent which increases acid
concentration in GI Track (stomach).
⚫ Basically these types of drugs are used in treatment of achlorhydia.
⚫ The empty stomach has pH 1.5 -2 and increases to pH 5-6 when food is
ingested.
⚫ Because of the secretion of HCl the pH of stomach is low.
⚫ Gastric acid act by destroying the bacteria present in the ingested food and
drinks.
⚫ It softens the fibrous food and promotes the formation of the proteolytic
enzyme pepsin.
⚫ This pepsin enzyme Acidifiers or Acidifying agents are the inorganic agent
which either formed or increases acid concentration in GI Track (stomach).
⚫ Acholorhydria: It is an condition in which there is absence or insufficient
secretion of hydrochloric acid in stomach called as achlorhydria.
⚫
5. Classification of Acidifying agent or Acidifiers
⚫ Acidifying agent or Acidifiers are classified in to four types
⚫ Gastric Acidifiers
⚫ Urinary Acidifiers
⚫ Systemic Acidifiers
⚫ Acids
1.Gastric Acidifiers: These are the drugs which are used to increase the acidity of
the stomach in patient suffering from Achlorhydria. So dilute Hydrochloric acid
is used to maintain or raises the level of hydrochloric acid (HCl) in stomach,
thus maintaining proper pH of the stomach.
2.Urinary Acidifiers: These are the drugs which are used to remove acidic urine
from the body or to maintain the Ph of the urine. These type of acidifiers
widely used to cure some type of urinary tract infection (UTI)
3.Systemic Acidifiers: These are the drug which is able to neutralize the alkaline
body fluids, especially blood. These type of acidifiers used to treat patient
suffering from systemic alkalosis.
4.Acids: These are used as pharmaceutical aids in the preparation of
medicaments.
6. 1.Ammonium chloride*
⚫ Method of Preparation:
⚫ 1.It is prepared by neutralization of hydrochloric acid with the help of
ammonium hydroxide and the solution get evaporates to the dryness
followed by crystallization.
⚫ NH4
OH + HCl ---------- NH4
Cl + H2
O
⚫ 2. It is prepared by treating ammonia with hydrochloric acid.
⚫ NH3
+HCl --------------- NH4
Cl
⚫ Assay:
⚫ Principle: Assay of ammonium chloride is performed using argentimetric
titration.
⚫ Reactions :
7. ⚫ Procedure:
Conical Flask: Take a conical flask having 250ml capacity and add 0.1 gm
ammonium chloride & 20 ml distilled water then add 1.5 ml of conc. Nitric
acid, 2.5 ml nitrobenzene & 25 ml (0.1N) sliver nitrate.
Burette: Titrate the above solution using Standardized ammonium thiocynate
solution.
Indicator: 2 to 3 drops of ferric ammonium sulphate.
End point: It is colorless to reddish brown.
⚫ Properties:-
Physical properties: It is….
⚫ White colorless, crystalline or a coarse powder,Odorless.
⚫ Cooling saline in taste,Slightly hygroscopic in nature.
⚫ Very soluble in water, sparingly soluble in alcohol and freely soluble in glycerin.
⚫ Neutral to litmus but become quickly acidic on standing due to hydrolysis.
Chemical properties:
⚫ Ammonium Chloride when heated it loses a acid
⚫ NH4
Cl ----------------- HCl + NH3
⚫ Ammonium Chloride when react with base strong sodium hydroxide it
liberates ammonia gas.
⚫ NH4
Cl + NaOH ---------- H2
O +NaCl + NH3
8. Uses: It is ………
⚫ Used in Maintains of acid-base equilibrium of body fluids.
⚫ showing diuretic effect.
⚫ used as systemic acidifiers.
⚫ used in lead poisoning.
⚫ used in treatment of UTI.
⚫ Used as thickening agent in preparation of hair shampoos.
⚫ Also act as a flavoring agent.
⚫ Also acts as mild expectorant. Therefore in cough preparation it is
used because of local irritation this produces increased secretion of
respiratory tract and makes the mucus less viscous.
⚫ used as emetics.
9. 2.Dilute Hydrochloric acid
Properties:
Physical properties: It is……..
clear, colorless fuming liquid,tasteless.pungent in odour.
soluble in water & alcohol ,acidic to litmus.
Having specific gravity of about 1.18.
Chemical properties: It
Get dissociate at 1500c into hydrogen and chloride
2HCl ---------- H2
+ Cl2
Reacts with ammonia gas to produce white dense fumes.
HCl + NH3
------ NH4
Cl
Uses: It is……
⚫ used as acidifying agent.
⚫ Used as pharmaceutical aid.
⚫ Used as reagent in various strength.
⚫ Used in treatment of achlorhydria.
⚫ Used as solvent.
10. 2: ANTACID
⚫ Antacids are the agent or substances which neutralize the excess of
hydrochloric acid in stomach are called as antacid.
⚫ So it is used in hyperacidity or hperchlorhydria
(Excessive secretion of gastric HCL).
⚫ Antacids which on ingestion react with the gastric acid and lower the acidity of
gastric content.
⚫ They produce a Symptomatic relief of heart burn, pain by neutralizing excess
of HCl.
⚫ Ideal properties / Requirement / Characteristics of antacids:
⚫ Insoluble in water except systemic antacid e.g. sodium bicarbonate
⚫ Should have fine particle size
⚫ should not be absorbable
⚫ should not causes constipation
⚫ should not be act as a laxative
⚫ should exert effect rapidly
⚫ should not causes systemic alkalosis
⚫ Should effect over a long period of time
⚫ Probably inhibit pepsin
⚫ Easily available,Non toxic,Not causes any side effect,Should be stable
⚫ Antacid should be inexpensive and palatable.
12. Sodium bicarbonate
Methods of preparation : A highly concentrated water solution of sodium
chloride is saturated with ammonia to removes impurities, then filtered the
solution and passes through the carbonating tower .In this reaction it is
allowed to interact with a current of CO2 and the tower is cooled to enhance
precipitation. Finally the precipitation is get filtered out and dried.
⚫ Sodium bicarbonate is prepared in laboratory by passing CO2 gas through
sodium hydroxide solution. Finally the solution is concentrated to obtain the
final product.
Assay:
⚫ Principle: Assay of sodium bicarbonate is depends on acid-base reaction. In
which sodium bicarbonate act as weak base and hydrochloric acid act as strong
acid.
⚫ Reaction:
⚫ 2NaHCO3
+HCl --------------- NaCl + 2H2
O + CO2
13. Procedure:
⚫ Conical flask: Dissolve 1.5 gm of sodium bicarbonate in 50 ml
carbon dioxide free water in a conical flask having 250ml capacity.
⚫ Indicator: Add 0.2 ml of methyl orange solution.
⚫ Burette: Titrate the above solution using standardized hydrochloric
acid.
⚫ End point: Solution becomes pink.
Properties:- Physical properties: It is…..
⚫ whitecoloured crystalline powder.
⚫ odourless.
⚫ saline in taste.
⚫ soluble in water.
⚫ insoluble in alcohol.
⚫ basic in nature in aqueous solution.
⚫ having ph 8.2 in aqueous solution
14. Chemical properties:
⚫ It is stable in air but get degrade in presence of heat or moist air.
⚫ 2NaHCO3
-------------- H2
O + CO2
+ Na2
CO3
Uses:- Sodium bicarbonate : It is
⚫ used as systemic antacid.
⚫ used as an electrolyte regenerator.
⚫ used in the treatment of acidosis.
⚫ used as expectorant.
⚫ Helps to produce systemic alkalosis.
⚫ used in eye drops and ear drops formulation to remove the wax.
⚫ used to control vomiting.
⚫ Used used as 1-2% solution for rinsing the contact lens.
15. Aluminium Containing Antacid:
ex. Aluminum hydroxide gel
⚫ Aluminium hydroxide gel:-
Properties –
⚫ Physical Properties: It is…..
⚫ A white, viscous suspension, from which small amounts of clear liquid may
separate on standing.
⚫ translucent in nature.having pH range in between 3-5.sweet in taste.
⚫ Chemical Properties: It is
⚫ When interact with hydrochloric acid to form Aluminium chloride (salt) and
water
⚫ Al (OH)3
+ 3HCl ---------- AlCl3
+ 3H2
O
⚫ Uses:-It is….
⚫ non-absorbable OR non systemic antacid.
⚫ used as mild Astringent & Demulcent when applied externally.
⚫ used as protective in the treatment of Diarrhea & Cholera .
⚫ used as dusting powder when applied externally
16. • Magnesium Containing Antacid:
• Magnesium hydroxide mixture
⚫ Magnesium Hydroxide Mixture
Properties:
⚫ Physical properties: It is…..
⚫ white amorphous powder.
⚫ odorless.
⚫ practically insoluble in water.
⚫ soluble in dilute mineral acids.
⚫ Chemical properties:
⚫ At high temperatures, solid magnesium hydroxide undergoes a very
endothermic (absorbs heat from atmosphere) degradation into magnesium
oxide and water, making it a good smoke suppressing and fire-fighting
agent.
⚫ Mg (OH)2
→ MgO + H2
O
Uses: It is…..
⚫ used as antacid.
⚫ used as laxative.
⚫ Used as Antiperspirant
⚫ used in waste water treatment.
17. 3: CATHARTICS
Saline catharitics : These are the agents/ substances which are used
to relive the constipation.
The term laxative is used for mild cathartic whereas a purgative is
used for strong cathartics.
These are the agent which increases the evacuation of fecal matter
from the bowel by increasing osmotic pressure.
ex. Magnesium sulphate, Sodium orthophosphate, Kaolin and
Bentonite
Classification of Saline cathartics/ Osmotic laxatives
⚫ Sodium containing products- Sodium potassium tartarate, Sodium
phosphate
⚫ Magnesium containing products- Magnesium hydroxide,
Magnesium sulphate, Magnesium Citrate.
⚫ Sulfur as cathartic
⚫ Non official Cathartics- Sodium sulphate, Potassium phosphate.
18. Magnesium sulphate
Properties:-.
⚫ Physical propertires: It is….
⚫ shiny white or colourless needle like crystals
⚫ soluble in water and very soluble in boiling water
⚫ insoluble in most of the organic solvent. odourless.having saline taste
⚫ It evolve efflorescence in dry air
⚫ Chemical Properties:
⚫ The aqueous solution of sodium bicarbonate is treated with magnesium sulphate,
precipitate is not produced, but upon boiling white precipitate of magnesium carbonate is
produced.
⚫ MgSO4
+ NaHCO3 -----------------------
No reaction
boil
⚫ NaHCO3 -----------
Na2
CO3
⚫ Na2
CO3
+ 5MgSO4 ------------------------
4MgCO3.
Mg(OH)2
5H2
O + CO2
Uses:
⚫ About 5gm of magnesium sulphate produces laxative effect.
⚫ It is used as antidote in heavy metal poisoning.
⚫ It is used as saline cathartics.
⚫ It is used in enema.
⚫ It is used as anticonvulsant given by parenteral route.
⚫ It used to reduce pain, inflammation& cramps.
19. Sodium orthophosphate:
⚫ Properties: It is……
⚫ White to off-white powder, crystals, or granules
⚫ It is salt of sodium hydroxide and phosphoric acid.
⚫ Uses: - It is
⚫ used as a laxative.It is used in constipation.
Kaolin
⚫ Properties: - It is…..
⚫ As a soft, white or yellowish white powder,having a clay like earthy taste
⚫ When it is moistened with water, assumes a darker colour,
⚫ insoluble in water, in cool dilute acids or in solution of alkali hydroxide.
⚫ Uses: - It is…….
⚫ used as dusting powder.used as adsorbent.
⚫ used as diluents in tablet formulation.
⚫ used as clarifying agent.used in alkaloidal& food poisoning.
⚫ used in treatment of diarrhea and dysentery.used in treatment of cholera.
20. Bentonite:
⚫ Physical Properties:
⚫ Bentonite is a natural, colloidal, hydrated aluminium silicate
⚫ It is a very fine, pale buff or cream-coloured to greyish-white powder .
⚫ It is insoluble in water,
⚫ It is also insoluble in organic solvents.
⚫ Uses:
⚫ Pharmaceutical aid (suspending agent).
⚫ Bentonite is used as a binding agent in the production of iron ore
pellets.
⚫ It acts as lubricant agent.
⚫ It is used in production of cement and mortars.
⚫ It is used in waste water purification.
⚫ It is used in extraction of oils.
⚫ Bentonite is used as an antidote in heavy metal poisoning.
21. 4.ANTIMICROBIALS
Antimicrobial agent: The substances which are used to kill microorganisms are
called antimicrobial agents.
Such as Hydrogen peroxide, potassium permagnate, chlorinated lime. Etc.
⚫ Classification of antimicrobial agent
⚫ Antiseptics: Substances or agent that have the power to kill the microbes and
stop the expansion of microbes once applied on living material, for example
oxide like Hydrogen peroxide
⚫ Disinfectant: Substances or agent that have the power to kill microbes and
stopthe expansion of microbes when applied on non- living material/
inanimate object, for example cresol.
⚫ Bactericidal: Substances or agents that have the power to kill bacteria for
examplePot. Permagnate.
⚫ Bacteriostatic: Substances or agent that have the ability to prevent the
growth of the bacteria, for example Borax
⚫ Fungicidal: Substances or agent that have the power to kill the fungi for
example Iodine
⚫ Fungi static: Substances or agent that have the ability to prevent the growth
of the fungi.
⚫ Germicide: Substances or agent that have the power to kill the germs for
example Iodine
22. Potassium permagnate :-
Properties :-
⚫ Physical Properties: It is….
⚫ occurs as darker purple, slender, prismatic by a dark bronze like
appearance. odorless.
⚫ Having sweet and astringent taste. soluble in water.
⚫ Chemical Properties:
⚫ Potassium acts as strong oxidizing agents
⚫ KMnO4
+ H2
O + KI → 2 MnO2
+ KIO3
+ KOH
⚫ 2 KMnO4
+ 10 KI + 8 H2
SO4
→ 6 K2
SO4
+ 2 MnSO4
+ 5 I2
+ 8 H2
O
⚫ Uses: It is…
⚫ used as disinfectant and deodorant due to its strong oxidising
properties.
⚫ also used as astringents, anti-infective and bactericidal.
⚫ Used as a bleaching agent.
⚫ used extensively in the water treatment.
⚫ Used in the form of aqueous solution for gargles and as mouth wash.
23. Boric Acid
Physical properties:It is…..
⚫ white crystalline powder with soapy touch.
⚫ odourless and stable in air. bitter in taste
⚫ soluble in boiling water & freely soluble in Glycerine.
⚫ slightly acidic in nature.(Ph between 3.8-4.8)
⚫ Chemical properties:
⚫ Boric acid is soluble in boiling water. When heated above 1000
C it converted to
metaboric acid (HBO2
) and when metaboric acid heated at 1600
C it converted into
tetraboric acid or pyroboric acid (H2
B4
O7
) and when pyroboric acid is heated above
2000
C it degrade into boron trioxide (B2
O3
):
Uses:
⚫ used in preparation of buffer solution.
⚫ used in various topical medications to maintain acidic pH
⚫ Dusting powder as ingredient because boric acid has smooth unctuous nature
⚫ used mainly as eye & mouth wash for local anti-infective action in the form of solution
⚫ used as Insecticide
24. ⚫ Chlorinated lime (Bleaching powder); Method of Preparation:
⚫ Calcium hypochlorite is produced industrially by passing chlorine gas in to calcium
hydroxide (slaked lime) to produce chlorinated lime.
⚫ 2 Cl2
+ 2 Ca(OH)2
→ Ca(OCl)2
+ CaCl2
+ 2 H2
O
⚫ Assay: Principle: Assay is based on Iodometric type of titration.
⚫ Reaction: 2KI + Cl2
---------- 2KCl + I
⚫ Na2S2O3 + I2
--------- Na2
S4
O6
+ 2NaI
⚫ Procedure: Conical flask: Chlorinated lime react with carbon dioxide and chlorine gas is
liberated it further react with potassium iodide to liberate Iodine
⚫ Burette:0.1 N Sodium thiosulphatesolution.
⚫ Indicator:Starch paste. End point:Violet colour.
⚫ Properties :- Physical properties: It is….
⚫ white/gray powder. Having strong odour of chlorine.
⚫ on expose to air it becomes moist ,sparingly soluble in water and soluble in alcohol.
⚫ Chemical properties:
⚫ When calcium hypochlorite react with hydrochloric acid to produce calcium chloride,
water and chlorine:
⚫ Ca(OCl)2
+ 2HCl CaCl2
+ H2
O + Cl2
25. Uses: It is….
⚫ Used to kills most of the bacteria, some fungi, yeast, algae, viruses and protozoa.
⚫ commonly used to sanitize public swimming pools and disinfect drinking water.
⚫ is also used in kitchens to disinfect surfaces and equipment. used in preparation of
detergents
⚫ used as bleaching agent, to decolorize most of dyes.
⚫ Used as bathroom cleansers, household disinfectant sprays, algaecides and herbicides.
Iodine:
⚫ Properties of Iodine: Physical properties: It is….
⚫ a heavy, greyish violet, brittlele, plates or metallic luster/ small crystals.
⚫ having metallic shine, irritating odour ,volatizes at ordinary room temperature.
⚫ Melt at higher or room temperature, snsoluble in glycerine , very slightly soluble in
water
⚫ Chemical properties: It….
⚫ Produces various forms of iodates such as Fe, Hg,Pb, etc
⚫ 3Fe + 4I2 -------------------
Fe3
I8
, Hg + I2
---------- Hg I2
and Pb+ I2
----------Pb I2
⚫ Use / Role: It is used in treatment of goiter.
⚫ Used as antimicrobial agent.
⚫ Used as germicides & fungicide in the form of aqueous & alcoholic solution.
⚫ Used in purification of drinking water.
⚫ Used as bacteriocidal and amoebicidal.
⚫ Used for disinfecting unbroken skin.