Learning objectives
Introduction
Types of solvents
Acidimetry in non aqueous medium
Alkalimetry in non aqueous medium
Estimation of Sodium benzoate and Ephedrine HCl
Applications of non aqueous titrations in pharmacy
Conclusion
Reference
Non-aqueous titrations involve using a non-aqueous solvent instead of water. They are used when the reactant is insoluble in water, reactive with water, or too weak an acid or base. The document discusses different types of non-aqueous solvents and their properties, as well as considerations for non-aqueous titration procedures and methods. Common solvents, titrants, and indicators used are outlined. Examples of titrating weak bases with perchloric acid in acetic acid and weak acids with sodium methoxide are provided.
The document describes limit tests for various inorganic impurities that may be present in compounds. It discusses the principles, procedures, and observations for limit tests of chlorides, sulphates, iron, lead, arsenic, and heavy metals. The tests involve preparing test and standard solutions, and comparing a property such as turbidity, color formation, or stain intensity between the two. If the property from the test solution is less than the standard, then the sample passes the limit test for that impurity. The document provides detailed procedures for each limit test.
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.
This document discusses non-aqueous titrations, which are used to analyze organic acids and bases that are insoluble or weakly reactive in water. It describes the principles, reasons for using non-aqueous titrations, common solvents like acetic acid, and provides examples of procedures to titrate drugs like ephedrine hydrochloride and sodium benzoate. The key steps involve dissolving the analyte in a non-aqueous solvent, titrating with an acid or base, and determining the endpoint using an indicator reaction.
This document discusses non-aqueous titrations, including the types of solvents used, endpoint detection methods, and applications. It covers protogenic solvents like acetic acid that can act as both acids and bases, protophilic solvents with high proton affinity, and aprotic solvents like benzene that are inert. Common indicators and titrants used include crystal violet, perchloric acid, and sodium acetate. The document provides examples of using non-aqueous titrations to assay substances like sodium acetate and norfloxacin tablets that are insoluble or reactive in water.
This document describes a test to detect the presence of arsenic in medicinal substances. The test works by reducing any arsenic in the sample to arsine gas using zinc, acid, and other reducing agents. The arsine gas is carried through a glass tube to mercuric chloride paper, where it will produce a yellow stain if arsenic is present. The intensity of the stain is compared to standard stains produced using known quantities of arsenic to determine if the level of arsenic passes the limit test. The test is run for 40 minutes and any yellow stain less intense than the standard passes, indicating the level of arsenic is below the limit.
This document discusses precipitation titration methods. It describes the principles of precipitation titration where a titrant forms an insoluble precipitate with the analyte. Common methods like Mohr's, Volhard's, and Fajans are summarized. Factors affecting precipitate solubility and limitations of precipitation titration are also outlined. The document serves to introduce various techniques in precipitation titration.
The document provides information about diazotization titrations. It discusses the principle, theory, procedure, end point detection, factors affecting, applications, and advantages/disadvantages of diazotization titrations. The key points are:
- Diazotization titrations involve the reaction of a primary aromatic amine with sodium nitrite in acidic medium to form a diazonium salt, which is then titrated.
- The end point is detected using an external indicator like starch iodide paper or electrochemically.
- Factors like acid concentration, temperature, and reaction time must be controlled.
- It can be used to determine drugs and compounds containing
Non-aqueous titrations involve using a non-aqueous solvent instead of water. They are used when the reactant is insoluble in water, reactive with water, or too weak an acid or base. The document discusses different types of non-aqueous solvents and their properties, as well as considerations for non-aqueous titration procedures and methods. Common solvents, titrants, and indicators used are outlined. Examples of titrating weak bases with perchloric acid in acetic acid and weak acids with sodium methoxide are provided.
The document describes limit tests for various inorganic impurities that may be present in compounds. It discusses the principles, procedures, and observations for limit tests of chlorides, sulphates, iron, lead, arsenic, and heavy metals. The tests involve preparing test and standard solutions, and comparing a property such as turbidity, color formation, or stain intensity between the two. If the property from the test solution is less than the standard, then the sample passes the limit test for that impurity. The document provides detailed procedures for each limit test.
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.
This document discusses non-aqueous titrations, which are used to analyze organic acids and bases that are insoluble or weakly reactive in water. It describes the principles, reasons for using non-aqueous titrations, common solvents like acetic acid, and provides examples of procedures to titrate drugs like ephedrine hydrochloride and sodium benzoate. The key steps involve dissolving the analyte in a non-aqueous solvent, titrating with an acid or base, and determining the endpoint using an indicator reaction.
This document discusses non-aqueous titrations, including the types of solvents used, endpoint detection methods, and applications. It covers protogenic solvents like acetic acid that can act as both acids and bases, protophilic solvents with high proton affinity, and aprotic solvents like benzene that are inert. Common indicators and titrants used include crystal violet, perchloric acid, and sodium acetate. The document provides examples of using non-aqueous titrations to assay substances like sodium acetate and norfloxacin tablets that are insoluble or reactive in water.
This document describes a test to detect the presence of arsenic in medicinal substances. The test works by reducing any arsenic in the sample to arsine gas using zinc, acid, and other reducing agents. The arsine gas is carried through a glass tube to mercuric chloride paper, where it will produce a yellow stain if arsenic is present. The intensity of the stain is compared to standard stains produced using known quantities of arsenic to determine if the level of arsenic passes the limit test. The test is run for 40 minutes and any yellow stain less intense than the standard passes, indicating the level of arsenic is below the limit.
This document discusses precipitation titration methods. It describes the principles of precipitation titration where a titrant forms an insoluble precipitate with the analyte. Common methods like Mohr's, Volhard's, and Fajans are summarized. Factors affecting precipitate solubility and limitations of precipitation titration are also outlined. The document serves to introduce various techniques in precipitation titration.
The document provides information about diazotization titrations. It discusses the principle, theory, procedure, end point detection, factors affecting, applications, and advantages/disadvantages of diazotization titrations. The key points are:
- Diazotization titrations involve the reaction of a primary aromatic amine with sodium nitrite in acidic medium to form a diazonium salt, which is then titrated.
- The end point is detected using an external indicator like starch iodide paper or electrochemically.
- Factors like acid concentration, temperature, and reaction time must be controlled.
- It can be used to determine drugs and compounds containing
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.
The document describes procedures for limit tests to detect arsenic and lead impurities. For arsenic, the test uses Gutzeit apparatus to convert any arsenic present into arsine gas, which is detected by the formation of a yellow stain on mercuric chloride paper. For lead, the test uses dithizone to form a violet-colored lead dithizonate complex if lead is present, and the color is compared to a standard. Both tests involve extraction and color comparison to determine if the level of impurity exceeds the specified limit.
This document discusses various redox titration methods including permanganometry, dichrometry, cerimetry, iodimetry, and bromatometry. It defines oxidation, reduction, and redox reactions. It explains how to calculate equivalent weights of oxidizing and reducing agents and different methods to detect the endpoint of a redox titration including using internal indicators, self indicators, external indicators, and instrumental methods. It provides examples of applications for each type of redox titration.
The document describes the limit test for lead, which determines the allowable limit of heavy metal lead in a sample. The test involves reacting the sample with dithizone, which forms a violet-colored lead dithizonate complex in the presence of lead. The intensity of color in the sample is compared to that of a standard lead solution treated the same way. If the sample solution is less colored than the standard, the sample passes the lead limit test. The test is useful for detecting trace amounts of lead impurity from sources like equipment, storage containers, or packaging materials used during manufacturing or storage of medical compounds.
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.
This document describes the limit test for lead using diphenylthiocarbazone (dithizone) which forms a violet colored lead-dithizonate complex in an alkaline medium. The method separates any lead impurity in a substance by extracting an alkaline solution with dithizone chloroform solution. The intensity of the violet color complex is then compared to a standard lead solution to determine the amount of lead present.
This document provides an overview of non-aqueous titration as a technique used in pharmaceutical analysis. It discusses the need for non-aqueous titrations when analytes are not soluble or reactive in water. The principles and techniques of non-aqueous acid-base titration are explained, including the use of aprotic, protogenic, amphiprotic and protophilic solvents. Common titrants, indicators, and examples of pharmaceutical compounds analyzed by non-aqueous titration like sodium benzoate and ephedrine hydrochloride are outlined. The document also provides procedures for standardizing titrants and estimating drugs using this analytical method.
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
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
This document discusses various types of saline cathartics (laxatives) including their definitions, mechanisms of action, preparations, and uses. The main types discussed are bulk forming laxatives, osmotic laxatives, lubricant laxatives, surfactant laxatives, and purgatives. Specific saline cathartics described in detail include magnesium hydroxide, magnesium sulfate (Epsom salt), and magnesium carbonate. Their preparations, assays, uses as laxatives or other purposes, and dosages are provided.
This document discusses electrolyte therapy, including normal electrolyte requirements, solutions for initial and subsequent electrolyte replacement, and the ingredients and amounts in oral rehydration salts. It lists the normal requirements in meq/L or meq/liter for electrolytes like sodium, potassium, chloride, bicarbonate, magnesium, calcium, and phosphorous. It also provides the formulation for oral rehydration salts, including the active ingredients dextrose monohydrate, potassium chloride, sodium citrate, and the amounts needed to make up 1000ml of solution.
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.
The document provides instructions for performing an assay of calcium gluconate by complexometry, including preparing standard EDTA and magnesium sulfate solutions, titrating calcium gluconate against EDTA while using magnesium and an indicator to identify the endpoint, and calculating the percentage purity of calcium gluconate based on the titration results. The titration is a replacement complexometric titration that uses the stable magnesium-indicator complex to indirectly determine the endpoint of the calcium-EDTA reaction.
This document describes the procedure for performing a limit test for sulphate according to the Indian Pharmacopoeia. A barium sulphate reagent is prepared containing barium chloride, potassium sulphate, alcohol and water. Standard sulphate solutions are also prepared. The test involves adding nitric acid and the reagent to samples and standards, observing any turbidity formed, and comparing the sample to the standard. If the sample turbidity is less than the standard, it passes the limit test, and if greater, it fails the test.
This document describes 4 methods for performing a limit test for heavy metals according to the Indian Pharmacopoeia. Method A uses hydrogen sulfide to form metal sulfides from heavy metals in an acidic solution. Method B also uses hydrogen sulfide but first chars and digests the sample. Method C uses sodium sulfide to form metal sulfides in an alkaline solution. Method D uses thioacetamide to react with heavy metals in an acidic buffer solution. For each method, the color produced by the test solution is compared to a standard solution and must not be more intense to pass the limit test.
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.
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.
Non-aqueous titration allows for the titration of weak acids and bases that cannot be accurately measured in aqueous solution. It involves titrating the substance using a non-aqueous solvent and titrant. Various organic solvents like acetic acid, alcohols, and amines can be used that compete less than water for proton donation or acceptance. This allows for sharper endpoints compared to titration in water for very weak acids and bases. Selection of the appropriate non-aqueous solvent depends on factors like solubility of the sample and ability to produce a clear endpoint.
Non-aqueous titrations allow for the titration of weakly acidic or basic substances using non-aqueous solvents. This provides sharper endpoints compared to aqueous titrations. Common non-aqueous solvents include acetic acid, acetonitrile, alcohols, and dimethylformamide. Indicators are also used that change color at the titration endpoint. Examples given are the titration of ephedrine hydrochloride and sodium benzoate using perchloric acid in acetic acid with crystal violet indicator.
The need for non aqueous titration arises because water can behave as a weak base and a weak acid as well, and can hence compete in proton acceptance or proton donation with other weak acids and bases dissolved in it.
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.
The document describes procedures for limit tests to detect arsenic and lead impurities. For arsenic, the test uses Gutzeit apparatus to convert any arsenic present into arsine gas, which is detected by the formation of a yellow stain on mercuric chloride paper. For lead, the test uses dithizone to form a violet-colored lead dithizonate complex if lead is present, and the color is compared to a standard. Both tests involve extraction and color comparison to determine if the level of impurity exceeds the specified limit.
This document discusses various redox titration methods including permanganometry, dichrometry, cerimetry, iodimetry, and bromatometry. It defines oxidation, reduction, and redox reactions. It explains how to calculate equivalent weights of oxidizing and reducing agents and different methods to detect the endpoint of a redox titration including using internal indicators, self indicators, external indicators, and instrumental methods. It provides examples of applications for each type of redox titration.
The document describes the limit test for lead, which determines the allowable limit of heavy metal lead in a sample. The test involves reacting the sample with dithizone, which forms a violet-colored lead dithizonate complex in the presence of lead. The intensity of color in the sample is compared to that of a standard lead solution treated the same way. If the sample solution is less colored than the standard, the sample passes the lead limit test. The test is useful for detecting trace amounts of lead impurity from sources like equipment, storage containers, or packaging materials used during manufacturing or storage of medical compounds.
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.
This document describes the limit test for lead using diphenylthiocarbazone (dithizone) which forms a violet colored lead-dithizonate complex in an alkaline medium. The method separates any lead impurity in a substance by extracting an alkaline solution with dithizone chloroform solution. The intensity of the violet color complex is then compared to a standard lead solution to determine the amount of lead present.
This document provides an overview of non-aqueous titration as a technique used in pharmaceutical analysis. It discusses the need for non-aqueous titrations when analytes are not soluble or reactive in water. The principles and techniques of non-aqueous acid-base titration are explained, including the use of aprotic, protogenic, amphiprotic and protophilic solvents. Common titrants, indicators, and examples of pharmaceutical compounds analyzed by non-aqueous titration like sodium benzoate and ephedrine hydrochloride are outlined. The document also provides procedures for standardizing titrants and estimating drugs using this analytical method.
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
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
This document discusses various types of saline cathartics (laxatives) including their definitions, mechanisms of action, preparations, and uses. The main types discussed are bulk forming laxatives, osmotic laxatives, lubricant laxatives, surfactant laxatives, and purgatives. Specific saline cathartics described in detail include magnesium hydroxide, magnesium sulfate (Epsom salt), and magnesium carbonate. Their preparations, assays, uses as laxatives or other purposes, and dosages are provided.
This document discusses electrolyte therapy, including normal electrolyte requirements, solutions for initial and subsequent electrolyte replacement, and the ingredients and amounts in oral rehydration salts. It lists the normal requirements in meq/L or meq/liter for electrolytes like sodium, potassium, chloride, bicarbonate, magnesium, calcium, and phosphorous. It also provides the formulation for oral rehydration salts, including the active ingredients dextrose monohydrate, potassium chloride, sodium citrate, and the amounts needed to make up 1000ml of solution.
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.
The document provides instructions for performing an assay of calcium gluconate by complexometry, including preparing standard EDTA and magnesium sulfate solutions, titrating calcium gluconate against EDTA while using magnesium and an indicator to identify the endpoint, and calculating the percentage purity of calcium gluconate based on the titration results. The titration is a replacement complexometric titration that uses the stable magnesium-indicator complex to indirectly determine the endpoint of the calcium-EDTA reaction.
This document describes the procedure for performing a limit test for sulphate according to the Indian Pharmacopoeia. A barium sulphate reagent is prepared containing barium chloride, potassium sulphate, alcohol and water. Standard sulphate solutions are also prepared. The test involves adding nitric acid and the reagent to samples and standards, observing any turbidity formed, and comparing the sample to the standard. If the sample turbidity is less than the standard, it passes the limit test, and if greater, it fails the test.
This document describes 4 methods for performing a limit test for heavy metals according to the Indian Pharmacopoeia. Method A uses hydrogen sulfide to form metal sulfides from heavy metals in an acidic solution. Method B also uses hydrogen sulfide but first chars and digests the sample. Method C uses sodium sulfide to form metal sulfides in an alkaline solution. Method D uses thioacetamide to react with heavy metals in an acidic buffer solution. For each method, the color produced by the test solution is compared to a standard solution and must not be more intense to pass the limit test.
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.
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.
Non-aqueous titration allows for the titration of weak acids and bases that cannot be accurately measured in aqueous solution. It involves titrating the substance using a non-aqueous solvent and titrant. Various organic solvents like acetic acid, alcohols, and amines can be used that compete less than water for proton donation or acceptance. This allows for sharper endpoints compared to titration in water for very weak acids and bases. Selection of the appropriate non-aqueous solvent depends on factors like solubility of the sample and ability to produce a clear endpoint.
Non-aqueous titrations allow for the titration of weakly acidic or basic substances using non-aqueous solvents. This provides sharper endpoints compared to aqueous titrations. Common non-aqueous solvents include acetic acid, acetonitrile, alcohols, and dimethylformamide. Indicators are also used that change color at the titration endpoint. Examples given are the titration of ephedrine hydrochloride and sodium benzoate using perchloric acid in acetic acid with crystal violet indicator.
The need for non aqueous titration arises because water can behave as a weak base and a weak acid as well, and can hence compete in proton acceptance or proton donation with other weak acids and bases dissolved in it.
Non Aqueous Titration
Types of solvents used in non aqueous Titration
Compounds used for non aqueous Titration
Titration done for weak acid and weak base,
Non-aqueous titration has several advantages over aqueous titration:
1. Organic acids and bases insoluble in water can be soluble in non-aqueous solvents allowing them to be titrated.
2. A non-aqueous solvent may help separate two or more acids in a mixture so they can be titrated individually.
3. More substances can be titrated as the solubility and application ranges are enlarged for weak acids/bases that cannot be titrated in water.
Some common non-aqueous solvents used include acetic acid, acetonitrile, alcohols, DMF. Indicators suitable for specific titrations must be selected to indicate the endpoint
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.
This document discusses non-aqueous titration. It explains that non-aqueous titration uses solvents other than water and can titrate organic compounds that are insoluble in water. The key aspects covered include the theory behind acid-base chemistry in different solvents, properties of non-aqueous solvents, factors in solvent selection, and applications like titrating weak acids and bases. Detection methods for non-aqueous titration include potentiometric and indicator-based methods.
Non aqueous titration refers to a type of titration in which the analyte substance is dissolved in a solvent which does not contain water. This procedure is a very important one in pharmacopoeial assays.
non aqueous titration, pharmaceutical and cosmetic analysis,Pca seminarSharath Hns
Non-aqueous titration involves titrating substances dissolved in solvents other than water. It has several advantages over aqueous titration, such as allowing the titration of very weak acids and bases. It provides a solvent in which organic compounds are soluble. Common non-aqueous titrations include titrating organic bases with perchloric acid in acetic acid. The document discusses the classification of solvents, reactions that take place, and examples of titrating substances like pyridine and benzoic acid in solvents like acetic acid and DMF. Practical applications involving titrating drugs and calculating percentage purity are also presented.
Non aqoues tittrations FOR MPHARM IST YEARprakash64742
Non-aqueous titrations are commonly used in pharmaceutical assays. The most common procedure is titrating organic bases with perchloric acid in anhydrous acetic acid. Different non-aqueous solvents can be used including aprotic, protophilic, protogenic, and amphiprotic solvents. Examples are provided of titrating various weakly basic pharmaceutical compounds using mercuric acetate and indicators like crystal violet in acetic acid with perchloric acid as the titrant. Precise procedures and calculations are described.
Non aqueous titration (AB-Production) IUB-BWPAwais Basit
This document discusses non-aqueous titration. It defines non-aqueous titration as the titration of weakly acidic or basic substances using non-aqueous solvents to obtain a sharp endpoint. It describes the types of non-aqueous solvents that can be used, including aprotic, protogenic, protophilic, and amphiprotic solvents. Some common indicators used in non-aqueous titrations and their color changes are also outlined. Advantages include the ability to titrate organic substances that are insoluble in water and selectively titrate mixtures. Disadvantages include the need for strict temperature and moisture control along with the use of expensive and sometimes toxic or volatile solvents.
Non-aqueous titration, Introduction, Theory & Principle, Solvents & Types of solvents, Indicator, Types of Non-aqueous titration, Methods of determination of end point, Assay of Sodium benzoate
This document discusses non-aqueous titration and provides details about the process. It describes the four main types of non-aqueous solvents used - aprotic, protogenic, protophilic, and amphiprotic. The presence of water can interfere with titrations between weak acids and bases by making the titration between a strong and weak system. The basic principles of non-aqueous titration involve the formation of onium ions or acetate ions to create a strong acid or base. Common indicators and procedures for preparing and standardizing perchloric acid are also outlined.
This document discusses non-aqueous titration, which involves titrating weakly acidic or basic substances using non-aqueous solvents to obtain a sharp endpoint. It describes the different types of non-aqueous solvents that can be used, including aprotic, protophilic, protogenic, and amphiprotic solvents. The document also discusses how solvent properties affect acidity and outlines methods for titrating weak acids and bases via potentiometric or indicator methods. Key indicators and solvents used for titrating each are provided.
This presentation summarizes non-aqueous acid-base titration. It introduces the presenter, MD. Zahirul Isalam from the Department of Pharmacy at World University of Bangladesh. The presentation defines non-aqueous titration as titrating weakly acidic or basic substances using non-aqueous solvents to get a sharp endpoint. It discusses the different types of non-aqueous solvents including aprotic, protophilic, protogenic, and amphiprotic solvents. The presentation also covers determining the endpoint through potentiometric or indicator methods and describes examples of titrating weak bases and acids through non-aqueous methods.
The document discusses non-aqueous titrations, which involve dissolving the analyte substance in a non-aqueous solvent rather than water. This is necessary when water could compete with or interfere with the reaction of weak acids and bases. The key advantages of non-aqueous titrations are that they can titrate very weak acids/bases and dissolve organic compounds. The document describes different types of non-aqueous solvents and how indicators and titrants are selected for particular analytes.
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.
Non-aqueous titration is used when the analyte is insoluble, reactive, or too weak to be titrated in water. The amphoteric nature of water can interfere with titration of weak acids or bases. Key aspects include:
- Using a non-aqueous solvent like acetic acid or DMF that is inert, acidic, or basic as needed.
- Titrants like perchloric acid or potassium methoxide that are appropriate for the analyte and solvent.
- Visual indicators that change color at the endpoint, selected based on the solvent system.
- Potentiometric titration can also detect the endpoint.
- Temperature, moisture and CO2 must be
1) Nonaqueous titration involves titrating substances dissolved in solvents other than water, commonly using organic bases titrated with perchloric acid in acetic acid.
2) Solvents used include aprotic solvents which are inert, protogenic solvents which are acidic, protophilic solvents which attract protons, and amphiprotic solvents which have both acidic and basic properties like acetic acid.
3) Endpoints in nonaqueous titrations are detected visually using pH indicator dyes which change color at the equivalence point, such as crystal violet turning from violet to greenish-yellow.
This document provides an overview of antibiotics. It begins with definitions of antibiotics and their history. Alexander Fleming discovered penicillin in 1929 from the Penicillium mold, but it was not until the 1940s that Howard Florey and Ernst Chain discovered its therapeutic properties. The document classifies antibiotics based on their spectrum of activity (narrow vs broad), mechanism of action (bacteriostatic vs bactericidal), source (natural, semisynthetic, synthetic), and chemical nature. Key requirements for antibiotics are that they selectively kill microbes without host toxicity, are eliminated from the body, are stable for formulation, and are highly effective at low concentrations.
This document discusses acidifying reagents, including dilute hydrochloric acid and ammonium chloride. It provides details on their preparation, properties, tests for identification and purity, assays, storage, and uses. Dilute hydrochloric acid is a clear, colorless liquid prepared by diluting concentrated hydrochloric acid with water. Ammonium chloride is a white, crystalline powder prepared by neutralizing ammonia with hydrochloric acid. Both are used as acidifiers in pharmaceutical preparations and to treat conditions like metabolic alkalosis.
Introduction
Limit Test for Chlorides
Limit Test for sulphates
Limit Test for Heavy metals
Limit Test for Iron
Limit Test for Arsenic
Limit Test for Lead
Reference
This document provides an overview of gravimetric analysis. It describes gravimetric analysis as a quantitative method that involves separating a substance into an insoluble compound and weighing it to determine the amount of the original constituent. The key steps are precipitation, filtration, washing, drying, ignition, weighing, and calculation. Gravimetric analysis is accurate and precise but also time-consuming and requires careful technique.
This document discusses the theory of acid-base indicators used in titration reactions. It explains that indicators change color within a certain pH range, allowing determination of the endpoint. Two theories are presented: Ostwald's theory states that color change is due to ionization of the indicator, while quinonoid theory proposes the indicator exists in two tautomeric forms in equilibrium, with different colors. Common indicators like phenolphthalein and methyl orange are discussed in the context of the two theories.
Learning objectives
Introduction
Complexing agents
Complexing Titration using EDTA
Need for Maintenance of pH
pH Indicators used in complexometric Titrations
Types of EDTA Titration
Factors Influencing EDTA reaction
Masking and demasking agents
Conclusion
Reference
Acidimetry uses a standard acid solution in a burette to titrate a known volume of base in a conical flask. This allows determination of the concentration of the base. Alkalimetry uses a standard base solution in a burette to titrate a known volume of acid in a conical flask. This allows determination of the concentration of the acid. Both processes identify the equivalent point where equal amounts of acid and base have reacted. Acidimetry is used to find the concentration of bases while alkalimetry is used to find the concentration of acids.
Learning objectives
Introduction
Preparation of a standard solution used for redox titration
Oxidizing and reducing agents used in volumetric analysis
N/10 potassium permanganate preparation
N/10 potassium dichromate preparation
N/10 Iodine solution preparation
Examples of redox titrations
Conclusion
References
Learning objectives
Introduction
Conditions For Volumetric Analysis
Terms In Volumetric Analysis
Primary Standard
Methods Of Expressing Concentrations In Volumetric Analysis
Types of Titration Methods
Classification Of Titrimetric Or Volumetric Methods
Conclusion
References
This document discusses acid-base titrations, which are used in quantitative analysis to determine the concentration of an acid or base by neutralizing it with a standard solution of known concentration. Alkalimetry and acidimetry involve titrating a base or acid, respectively, with a standard acid or base. Indicators are used to monitor the reaction and change color at the equivalence point. Common indicators and their pH ranges are identified. The choice of indicator depends on whether the titrant and titrated substances are strong or weak acids and bases.
Introduction
error, accuracy, precision
Source of Errors
Types of Errors
Methods of minimizing errors
Test for rejection of data
Significant Level
Rounding of Figures
References
What is Pharmaceutical Chemistry
Introduction of Inorganic chemistry
What are Inorganic Compounds ??
Importance of Inorganic Pharmaceuticals Inorganic Chemistry ??
Difference between Organic Chemistry and Inorganic Chemistry
Definitions
Formulation and evaluation of oral fast dissolving films of projectNikithaGopalpet
The document describes the formulation and evaluation of oral fast dissolving films containing risperidone as a model drug. The objectives were to develop a fast dissolving film to improve bioavailability and facilitate rapid onset of action for risperidone. Various preformulation studies were conducted including solubility determination and calibration curves. Six formulations of risperidone films were prepared using solvent casting method and evaluated for weight variation, thickness, folding endurance, surface pH, drug content uniformity, in vitro disintegration and dissolution tests. The results and discussion section compares the performance of the different formulations.
Introduction.
Methods of Administration of Local Anaesthetics
Classification .
Drugs used in local anaesthetics.
Mechanism of action and SAR.
Structure and Synthesis.
Adverse Drug Reactions and Uses.
Reference
The document discusses anti-diabetic agents and provides details about sulfonylureas. It describes the mechanism of action of sulfonylureas, which involves binding to sulfonylurea receptors on pancreatic beta cells and extrapancreatic cells to stimulate insulin secretion and inhibit gluconeogenesis. Adverse effects include hypoglycemia and weight gain. Tolbutamide is provided as an example sulfonylurea drug, with its structure, synthesis, mechanism of action, pharmacokinetics, adverse effects, and therapeutic uses summarized.
This document provides information on drugs acting on the endocrine system. It discusses the introduction and nomenclature of steroids, including sex hormones and their biosynthesis. The structures, syntheses and properties of key sex hormones are described, such as testosterone, oestriol, oestradiol, diethylstilbestrol and progesterone. References on medicinal chemistry textbooks are also listed.
This document discusses drugs used to treat erectile dysfunction. It begins with an introduction to erectile dysfunction and benign prostatic hyperplasia. The main drugs discussed are PDE5 inhibitors including sildenafil, tadalafil, vardenafil and avanafil, as well as alprostadil. These drugs work by inhibiting the PDE5 enzyme and increasing levels of cGMP in the penis to produce an erection. The document provides details on the mechanism of action, pharmacokinetics, molecular structures, adverse effects and uses of these erectile dysfunction drugs.
This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
Executive Directors Chat Leveraging AI for Diversity, Equity, and InclusionTechSoup
Let’s explore the intersection of technology and equity in the final session of our DEI series. Discover how AI tools, like ChatGPT, can be used to support and enhance your nonprofit's DEI initiatives. Participants will gain insights into practical AI applications and get tips for leveraging technology to advance their DEI goals.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar Kanvaria
How to Setup Warehouse & Location in Odoo 17 InventoryCeline George
In this slide, we'll explore how to set up warehouses and locations in Odoo 17 Inventory. This will help us manage our stock effectively, track inventory levels, and streamline warehouse operations.
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
The event will cover the following::
Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
The simplified electron and muon model, Oscillating Spacetime: The Foundation...RitikBhardwaj56
Discover the Simplified Electron and Muon Model: A New Wave-Based Approach to Understanding Particles delves into a groundbreaking theory that presents electrons and muons as rotating soliton waves within oscillating spacetime. Geared towards students, researchers, and science buffs, this book breaks down complex ideas into simple explanations. It covers topics such as electron waves, temporal dynamics, and the implications of this model on particle physics. With clear illustrations and easy-to-follow explanations, readers will gain a new outlook on the universe's fundamental nature.
This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UP
5. non aqueous titrations
1. NON-AQUEOUS TITRATIONS
Prepared by
G. Nikitha, M.Pharmacy
Assistant Professor
Department of Pharmaceutical Chemistry
Sree Dattha Institute Of Pharmacy
Hyderabad
2. CONTENTS
Learning objectives
Introduction
Types of solvents
Acidimetry in non aqueous medium
Alkalimetry in non aqueous medium
Estimation of Sodium benzoate and Ephedrine HCl
Applications of non aqueous titrations in pharmacy
Conclusion
Reference
3. LEARNING OBJECTIVES
In these topic we will discuss about
Brief introduction of Non aqueous titration, definition
Indicators used in Non aqueous titration
Applications of non aqueous titrations in pharmacy
Acidimetry in non aqueous medium
Alkalimetry in non aqueous medium
Types of solvents
Estimation of Sodium benzoate and Ephedrine HCl
4. INTRODUCTION
Non aqueous titration are those in which the titration of weakly acidic or basic
substances are carried out using non aqueous solvents so as to get sharp end
point.
Such titrations are can also be used for the titration of substances not soluble in
water.
Before understanding the significance of the use of Non aqueous solvents some
important terms and concepts have to understood. The reactions which occur in
these Non aqueous solvents can be explain by using Lowry-Bronsted theory.
Acid is a proton donor
Base is a proton acceptor
Example:
Hcl H++Cl
HSO4- H++ SO4
2
5. Non aqueous titrations are simple and accurate. The apparatus needed have
almost the same as that used in classical titrations expect with some precautions
that moisture and carbon dioxide have to be excluded.
In presence of moisture water, being weakly basic would compete with the
week nitrogen base for HClO4.
H2O +HClO4 H3O+ ClO4
The sharpness of the end point may get lost. Moisture content in this non-
aqueous titrimetry should be less than 0.05%
Organic acids or bases that have been insoluble in water can be made to
dissolve in Non aqueous solvents and titrated.
6. The neutralization of a base with standard acid in non-aqueous titrimetry may
be put as fallows
BOH +CH3ONa BONa +CH3OH
A greater difference in the protophilic properties of various substances takes
place in non aqueous solution such as acetonitrile, acetone and dimethyl
formamide than in aqueous solutions due to the leveling effect of water.
Although the following acids have been of about equal strength in aqueous
solvents acidity has been found to decrease in the following order:
HClO4 > H2SO4 >HCl >HNO3
7. INDICATORS
In non-aqueous titrations the end point can located by the colour changes of this
suitable indicator. Few indicators used in non-aqueous titrations are given
below.
Indicator Basic Neutral Acids
1. Crystal violet Voilet Blue-Green Yellowish
green
2. Naphtolbenzene Blue or Green Orange Dark Green
3. Oracet Blue B Blue Purple Pink
4. Quinaldine Red Magneta ------- Almost
colourless
8. TYPES OF SOLVENTS
Solvents are classified according to their properties as fallows
1. Aprotic solvents
2. Protogenic solvents
3. Protophilic solvents
4. Amphiprotic solvents
9. 1. Aprotic solvents:
These are solvents which are chemically inert and are not involved in any chemical
reaction.
Example: Chloroform, Benzene.
2. Protogenic solvents:
These are acidic substances and yield protons.
Example: sulphuric acid, Hydrochloric acid, Nitric acid etc
10. 3. Protophilic solvents:
These solvents are of two types. They are strongly basic or weakly basic in nature.
A strongly basic solvent has stronger tendency to accept the proton. A weekly basic
solvent has weaker tendency to accept the proton.
A strongly basic solvents is called as a “Leveling solvent” (for weak and strong
acids) because it can abstract proton from any acid. Whether it is strong acid or
weak acid. This effect is called “Leveling effect”. As it does not differentiate
between strong or weak acid.
On the other hand a weakly basic solvent has weak tendency to accept the proton.
Hence this solvent is tendency to accept the proton called a “Differentiating
solvent”. Because it can abstract proton from strongly acidic substances and
from weak acids. This effect is called “Differentiating effect”. Differentiating
solvents are not useful in non-aqueous titrations.
11. Similarly strongly acidic solvents are leveling solvents for weak bases and strong
bases. strongly acidic solvents can donate proton to strong bases as well as
weak bases.
Example: Perchloric acid, acetic acid etc.
4. Amphiprotic solvents:
These have both protogenic and protophillic properties
Example: water, acetic acid, alcohols.
Water has both protogenic and protophillic properties. It can behave as a base or
acid.
12. ACEDIMETRY IN NON-AQUEOUS MEDIUM
It used for the quantitative estimation of weak base.
Titrant:
Titrant should be strongly acidic in nature.
It is the known concentration.
It should be taken in burette
Example: Perchloric acid
Titrate:
Titrate should be weakly basic in nature
It is unknown concentration.
It should be taken in conical flask
Example: alkali salts of organic acids, amines, heterocyclic nitrogen compounds
are analyzed.
Drugs : Ephedrine, Morphine, Acyclovir, caffeine etc.
13. Solvents:
The solvents are either neutral such as alcohol, chloroform, benzene etc or acidic
solvents such as acetic acid etc. solvents should be protogenic in nature.
Indicator:
Crystal violet, Quinoline red, thymol blue.
14. Reactions:
B+CH3COOH ⇌ BH++CH3COO
Here B= Base
CH3COOH= Acetic acid
BH+ = conjugate acid of base
CH3COO = conjugate base
Titrant reacts with the solvent and gets promoted as follows
HClO4+CH3COOH ⇌ CH3COO H2+ClO4
-
Here
HClO4 = Perchloric Acid
CH3COOH= Acetic acid
ClO4
- = Perchlorate
15. Titration reaction with conjugate base anion may be put as follows
CH3COO + CH3COO H2 ⇌ 2CH3COOH
So overall reaction may be put as follows:
B+HClO4 BH++ClO4
-
16.
17. Preparation of 0.1 N perchloric acid :
8.5 ml of perchloric acid + 500ml of glacial acetic acid + 30ml of acetic anhydrous
cooled and volume is made up to 1000ml
with glacial acetic acid
It is kept for a day for the excess acetic acid anhydride to combine with water
present
The molecular weight of the perchloric acid is 100.46. So 1 liter of 0.1N solution
can be prepared by using 10.046g
18. Standardization of 0.1 N perchloric acid:
700mg of potassium hydrogen phthalate + 500ml of glacial acetic acid
In 250 ml flask
To these 2 drops of crystal violet is added
This solution is titrated with perchloric acid
Untill the violet colour changes to emerald green
violet emerald green
19.
20. potassium hydrogen phthalate is reacted with perchloric acid to get Phthalic acid and potassium
perchlorate. Here Potassium (K) from potassium hydrogen phthalate is removed and replaced
with hydrogen (H) from perchloric acid .
1ml of 0.1N HClO4 ≡ 20.48 mg of C8H5KO4
21. Assay of Ephedrine Hydrochloride:
An accurate weight of the sample + glacial acetic acid + Mercuric acetate
Titrated with 0.1N perchloric acid
Using crystal violet as indicator
22.
23. Estimation of Ephedrine:
An accurate weight of the sample + glacial acetic acid
Titrated with 0.1N perchloric acid
Using crystal violet as indicator
24. Estimation of Sodium benzoate
Preparation of 0.1N solution of HClO4 and its standardization:
8.5 ml of perchloric acid + 500ml of glacial acetic acid + 30ml of acetic anhydrous
cooled and volume is made up to 1000ml
with glacial acetic acid
It is kept for a day for the excess acetic acid anhydride to combine with water
present
The molecular weight of the perchloric acid is 100.46. So 1 liter of 0.1N solution
can be prepared by using 10.046g
25. Standardization of 0.1 N perchloric acid:
500mg of potassium hydrogen phthalate + 25ml of glacial acetic acid
In 250 ml flask
To these 2 drops of crystal violet is added
This solution is titrated with perchloric acid
Untill the blue colour changes to blue green
blue blue green
26. Assay Procedure :
Weigh accurately about 0.25 g of Sodium Benzoate +20 ml of anhydrous glacial
acetic acid
warming to 50º if necessary, cool
Titrate with 0.1 M perchloric acid, using 0.05 ml of 1-naphtholbenzein solution as
indicator. Carry out a blank titration.
27. ALKALIMETRY IN NON-AQUEOUS MEDIUM
It used for the quantitative estimation of weak acid.
Titrant:
Titrant should be strongly basic in nature.
It is the known concentration.
It should be taken in burette
Example: sodium methoxide, Lithium methoxide , sodium amino methoxide,
sodium triphenyl methane
Titrate:
Titrate should be weakly acidic in nature
It is unknown concentration.
It should be taken in conical flask
Example: Benzoic acid etc
Drugs : Nalidix acid, Acetazolamide, Allopurine, Mercaptopurine etc
28. Solvents:
Dimethyl Formamide (DMF), Pyridine, ethylene diamine etc. Strong basic solvents
such as butyl amine, morpholine used for the titration of weak acids.
Indicator:
Thymol blue
29.
30. Preparation and standardization of 0.1N sodium Methoxide
Preparation:
2.5g of freshly cut sodium metal + 150 ml of ice cold methanol
Present in one liter of volumetric flask
When sodium metal gets dissolved,
Sufficient quantity of benzene is added to make the volume up to 1 liter.
31. standardization of 0.1N sodium Methoxide
400mg of benzoic acid +80m of Dimethyl Formamide (DMF)
In a flask
3 drops of thymol blue is added
Titrated with sodium methoxide
End point is blue colour
32. Assay of Benzoic acid:
Required quantity of Benzoic acid + butylamine
Titrated with sodium methoxide
thymol blue as indicator
End point is blue colour
33. APPLICATIONS
It is useful for the titrations of weak acids or weak bases.
It is simple, qualitative and selective method.
It can be used for titration of mixture of acids as well.
Many organic acids which are not soluble in water can be dissolved in non
aqueous solvents
34. CONCLUSION
In these topic we have discussed about
Brief introduction of Non aqueous titration, definition
Indicators used in Non aqueous titration
Applications of non aqueous titrations in pharmacy
Acidimetry in non aqueous medium
Alkalimetry in non aqueous medium
Types of solvents
Estimation of Sodium benzoate and Ephedrine HCl
35. REFERENCE
Pharmaceutical Chemistry -Inorganic Volume-1 by G. R. Chatwal.
Essentials of Inorganic Chemistry by Katja A. Strohfeldt.
Indian Pharmacopoeia.
M.L Schroff, Inorganic Pharmaceutical Chemistry.
P. GunduRao, Inorganic Pharmaceutical Chemistry, 3rd Edition
A.I. Vogel, Text Book of Quantitative Inorganic analysis.
Bentley and Driver's Textbook of Pharmaceutical Chemistry.