Conductometric analysis measures the electrical conductivity of solutions to determine analyte concentration. It works by measuring how easily ions move through the solution when a current is applied. There are several types of conductometric titrations including acid-base, redox, and complexometric titrations. Conductometric titrations can determine the endpoint graphically without needing indicators and work well for colored, weak, or turbid solutions. The conductivity is measured using a conductometer with conductivity cells and platinum electrodes to apply a current and measure the solution's resistance.
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.
Complexometric titrations involve the formation of a soluble, stoichiometric complex during the titration of a sample solution. EDTA titrations are commonly used for complexometric titrations. EDTA forms stable complexes with metal ions and produces a sharp color change at the equivalence point. The stability and selectivity of metal-EDTA complexes can be increased through factors like pH, ligand properties, and use of metallochromic indicators that form colored complexes with metal ions.
Polarography is an electroanalytical technique invented by Jaroslav Heyrovsky in 1922. It involves using a dropping mercury electrode and measuring the current in the solution at different applied potentials to generate a current-voltage curve called a polarogram. There are four main types of current measured: residual, migration, diffusion, and limiting current. The construction includes a dropping mercury electrode, supporting electrolyte, mercury reservoir, and capillary tube. Polarography can be used for qualitative and quantitative analysis of samples without separation and allows analysis of small amounts of inorganic and organic substances.
Polarography is an electroanalytical technique that uses a dropping mercury electrode (DME) and measures the current between two electrodes when a gradually increasing voltage is applied. The current-voltage curve obtained is used to determine analyte concentration from the diffusion current and identify species from the characteristic half-wave potential. The Ilkovic equation relates diffusion current to analyte properties like concentration, number of electrons involved, and diffusion coefficient. Polarography finds applications in qualitative and quantitative analysis of metals, drugs, and organic compounds.
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.
Potentiometry, Electrochemical cell, construction and working of indicator an...Vandana Devesh Sharma
Potentiometry - Electrochemical cell -Construction and working of reference (Standard hydrogen, silver chloride electrode and calomel electrode)
Indicator electrodes (metal electrodes and glass electrode)
Methods to determine end point of potentiometric titration
and applications
Potentiometry is the method to find the concentration of solute in
A given solution by measuring the potential between two Electrodes
(reference and Indicator electrode) . Potentiometric titration involves
the measurement of the potential of the indicator electrode and
reference electrode.
In potentiometric titration reference and indicator electrodes are
immersed in the solution of particular analyte (titrand) and
potential of indicator electrode is measured with relation to
reference electrode.
Titrant is added in analyte (Titrand) and change in potential is noted
down.
At the end point there is sharp change in potential on indicator
electrode.
Graph is plotted between the indicator electrode potential and
volume of titrant added.
This method is used for determination of sharp end point.
Types of Potentiometric Titration
1. Acid-base titration 2. Redox Titration 3.Complexometric titration 4. Precipitation Titration
Conductometric analysis measures the electrical conductivity of solutions to determine analyte concentration. It works by measuring how easily ions move through the solution when a current is applied. There are several types of conductometric titrations including acid-base, redox, and complexometric titrations. Conductometric titrations can determine the endpoint graphically without needing indicators and work well for colored, weak, or turbid solutions. The conductivity is measured using a conductometer with conductivity cells and platinum electrodes to apply a current and measure the solution's resistance.
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.
Complexometric titrations involve the formation of a soluble, stoichiometric complex during the titration of a sample solution. EDTA titrations are commonly used for complexometric titrations. EDTA forms stable complexes with metal ions and produces a sharp color change at the equivalence point. The stability and selectivity of metal-EDTA complexes can be increased through factors like pH, ligand properties, and use of metallochromic indicators that form colored complexes with metal ions.
Polarography is an electroanalytical technique invented by Jaroslav Heyrovsky in 1922. It involves using a dropping mercury electrode and measuring the current in the solution at different applied potentials to generate a current-voltage curve called a polarogram. There are four main types of current measured: residual, migration, diffusion, and limiting current. The construction includes a dropping mercury electrode, supporting electrolyte, mercury reservoir, and capillary tube. Polarography can be used for qualitative and quantitative analysis of samples without separation and allows analysis of small amounts of inorganic and organic substances.
Polarography is an electroanalytical technique that uses a dropping mercury electrode (DME) and measures the current between two electrodes when a gradually increasing voltage is applied. The current-voltage curve obtained is used to determine analyte concentration from the diffusion current and identify species from the characteristic half-wave potential. The Ilkovic equation relates diffusion current to analyte properties like concentration, number of electrons involved, and diffusion coefficient. Polarography finds applications in qualitative and quantitative analysis of metals, drugs, and organic compounds.
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.
Potentiometry, Electrochemical cell, construction and working of indicator an...Vandana Devesh Sharma
Potentiometry - Electrochemical cell -Construction and working of reference (Standard hydrogen, silver chloride electrode and calomel electrode)
Indicator electrodes (metal electrodes and glass electrode)
Methods to determine end point of potentiometric titration
and applications
Potentiometry is the method to find the concentration of solute in
A given solution by measuring the potential between two Electrodes
(reference and Indicator electrode) . Potentiometric titration involves
the measurement of the potential of the indicator electrode and
reference electrode.
In potentiometric titration reference and indicator electrodes are
immersed in the solution of particular analyte (titrand) and
potential of indicator electrode is measured with relation to
reference electrode.
Titrant is added in analyte (Titrand) and change in potential is noted
down.
At the end point there is sharp change in potential on indicator
electrode.
Graph is plotted between the indicator electrode potential and
volume of titrant added.
This method is used for determination of sharp end point.
Types of Potentiometric Titration
1. Acid-base titration 2. Redox Titration 3.Complexometric titration 4. Precipitation Titration
This document provides an overview of conductometry. It discusses how conductometry measures the conductance of electrolyte solutions using a conductivity cell and conductometer. It describes different types of conductivity cells and how conductometric titrations work by measuring changes in conductance during titrations. Examples of various acid-base titrations are given. Conductometric titrations can be used to analyze many different samples and have advantages like not requiring indicators. Applications include measuring water pollution, food analyses, and more.
This document discusses conductometric titration, which is an electrochemical analytical method that measures the electrical conductance of an electrolyte solution. It describes the principles and instrumentation of conductometry, including how conductivity is measured using a conductivity meter or by performing a titration. Some key applications of conductometric titration are determining the end point of acid-base and precipitation titrations, and it has various uses in fields like environmental analysis, food testing, and quality control.
Polarographic technique is applied for the qualitative or quantitative analysis of electroreducible or oxidisable elements or groups.
It is an electromechanical technique of analyzing solutions that measures the current flowing between two electrodes in the solution as well as the gradually increasing applied voltage to determine respectively the concentration of a solute and its nature.
The principle in polarography is that a gradually increasing negative potential (voltage) is applied between a polarisable and non-polarisable electrode and the corresponding current is recorded.
Polarisable electrode: Dropping Mercury electrode
Non-polarisable electrode: Saturated Calomel electrode
From the current-voltage curve (Sigmoid shape), qualitative and quantitative analysis can be performed. This technique is called as polarography, the instrument used is called as polarograph and the current-voltage curve recorded is called as polarogram
This document discusses electrochemical methods and conductometry. It introduces conductometry as the determination of electrical conductance of an electrolyte solution using a conductometer. Conductometry is based on how ions in solution affect conductivity, which depends on ion type, concentration, temperature and mobility. The principles of conductometry and conductometric titration are explained. Conductometric titration involves substituting ions of one mobility for ions of another mobility until the equivalence point is reached. Examples of different types of titrations such as strong acid-strong base, strong acid-weak base, weak acid-strong base, and weak acid-weak base are provided.
Potentiometric - Pharmaceutical Analysis (101T)RAHUL PAL
Potentiometric methods of analysis measure the potential of electrochemical cells under conditions of zero current. The potential difference between a sensing electrode and a reference electrode is measured. A salt bridge containing an inert electrolyte connects the two half-cells and allows ionic movement to complete the electrical circuit. Common reference electrodes include the standard hydrogen electrode, saturated calomel electrode, and silver-silver chloride electrode. Potentiometry is used for applications such as determining electrode potentials, measuring pH, and analyzing samples in clinical chemistry, environmental chemistry, agriculture, and food processing.
Potentiometry involves measuring the potential of electrochemical cells under conditions of no current flow. There are two types - direct potentiometry measures the potential of indicator electrodes related to analyte concentration, while indirect potentiometry involves measuring potential changes during titrations. A potentiometric cell consists of a reference electrode that maintains a constant potential, an indicator electrode whose potential varies with analyte concentration, and a salt bridge. The Nernst equation describes the relationship between electrode potential and analyte concentration or activity.
This document provides an overview of conductometry and its applications. It discusses Ohm's law and how conductivity is measured using electrodes, standard solutions, and a conductivity cell. Factors that affect conductivity include ion size, temperature, charge, and number. Conductometric titrations can be used to determine endpoints and are advantageous because no indicator is needed. Types of titrations discussed include acid-base, precipitation, replacement, redox, and complexometric. Recent applications include use in refineries, estimating polyelectrolytes, and biotechnology/environmental monitoring.
Complexometric titration involves the titration of a metal ion solution with a chelating agent or ligand until the metal ion forms a stable complex. It is useful for determining mixtures of metal ions. The document discusses various types of complexometric titrations including direct titration, back titration, and replacement titration. It also covers the use of metal ion indicators, masking and demasking reagents, and provides examples of complexometric titration for determining compounds like magnesium sulfate, calcium gluconate, and auric ions in ores.
The document discusses the dropping mercury electrode (DME), which is a working electrode used in polarography where mercury drops from a reservoir through a capillary tube into the solution being analyzed. It provides details on the structure of the DME including the mercury reservoir and capillary tube. The document also describes how the DME works, lists different types of mercury electrodes, and discusses the advantages, disadvantages, and precautions of using the DME.
This document discusses the principles and procedures of conductometric analysis. Conductometric analysis measures the electrical conductivity of a solution due to ion mobility. The conductivity is affected by factors like number, charge, size of ions, and temperature. It involves titrating a solution containing ions and measuring the change in conductivity. This allows determination of the endpoint of the titration from the plotted conductivity-volume curve. The document defines key terms, describes instrumentation including conductivity cells and electrodes, and discusses different types of conductometric titrations like acid-base, redox, and complexometric titrations. Conductometric titrations provide accurate results for analyses without requiring indicators.
Polarography uses a dropping mercury electrode (DME) to measure the current flowing through an electrochemical cell as a function of the applied potential. A polarogram plots this current versus potential and provides qualitative and quantitative information about species undergoing oxidation or reduction reactions. Jaroslav Heyrovsky invented the polarographic method in 1922 and won the Nobel Prize for his contributions to electroanalytical chemistry. All modern voltammetric methods originate from polarography. The DME provides advantages like a reproducible surface area and the ability to form amalgams with metal ions.
Potentiometry uses a reference electrode and an indicator electrode to measure the potential difference in a sample solution. When the electrodes are placed in the solution, the potential is generated based on the concentration of ions present. There are several types of potentiometric titrations including acid-base, redox, complexometric, and precipitation titrations. Potentiometry has many applications in fields like clinical chemistry, environmental analysis, potentiometric titrations, agriculture, detergent manufacturing, food processing and more. It is used to analyze important ions and determine equivalence points during titrations.
It is an electrochemical method of analysis used for the determination or measurement of the electrical conductance of an electrolyte solution by means of a conductometer.
Electric conductivity of an electrolyte solution depends on :
Type of ions (cations, anions, singly or doubly charged
Concentration of ions
Temperature
Mobility of ions
The main principle involved in this method is that the movement of the ions creates the electrical conductivity. The movement of the ions is mainly depended on the concentration of the ions.
The electric conductance in accordance with ohms law which states that the strength of current (i) passing through conductor is directly proportional to potential difference & inversely to resistance.
i =V/R
This document discusses conductometry, which is a method of analysis based on measuring the electrolytic conductance of a solution. It begins by classifying different electrochemical methods, including conductometry and electrophoresis which do not involve redox reactions. It then discusses key concepts in conductometry such as conductivity, conductance, equivalent conductance, and how various factors like ion nature, temperature, concentration, and electrode size affect conductance. It also provides examples of calculating conductance and equivalent conductance from experimental measurements. Instrumentation for conductometric determination includes a conductance cell and conductivity bridge.
Potentiometry involves measuring the potential or electromotive force of a sample solution using an electrochemical cell containing a reference electrode and an indicator electrode. The potential is directly proportional to the ion concentration in the solution. Common reference electrodes include the standard hydrogen electrode, silver chloride electrode, and saturated calomel electrode. Indicator electrodes can be metal electrodes or ion-selective electrodes like the glass membrane pH electrode. Potentiometric titration determines the concentration of an analyte by measuring the potential change as a titrant is added, with the endpoint indicated by an abrupt potential shift. Applications of potentiometry include acid-base, redox, complexometric, and precipitation titrations.
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EDTA Titration
Amperometric titration involves measuring the electric current produced by a titration reaction while keeping the voltage constant between electrodes. It can determine the endpoint of titrations involving an electroreducible ion being titrated with a counter ion. The diffusion current is measured and plotted against the titrant volume added. At the endpoint, there is a sharp change in current. Amperometric titration offers advantages like rapid analysis, ability to work with dilute solutions, and determination of insoluble substances. It finds applications in areas like determining water content and quantification of ions.
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.
This document discusses precipitation titration methods. It describes Mohr's method, Volhard's method and Fajan's method. Mohr's method uses potassium chromate as an indicator. Volhard's method indirectly titrates excess silver ions with thiocyanate using ferric ammonium sulfate as an indicator. Fajan's method uses adsorption indicators like fluorescein that change color upon adsorption to the precipitate formed at the endpoint. Key factors that influence precipitation titrations like solubility products, common ion effect and temperature are also discussed.
This document discusses redox titrations and provides examples of different types of titrations including acid-base, complexometric, precipitation, and redox titrations. It defines oxidation and reduction in terms of the gain or loss of electrons. Redox titrations involve the transfer of electrons between reactants. The document provides examples of balancing redox equations using half-reactions and discusses how oxidation numbers are used to identify oxidation and reduction in redox reactions.
Conductometry is an electrochemical method of analysis involve the measurement of the electrical conductivity of a solution. The conductance is defined as the current flow through the conductor.
In other words, it is defined as the reciprocal of the resistance.
This document provides an overview of conductometry. It discusses how conductometry measures the conductance of electrolyte solutions using a conductivity cell and conductometer. It describes different types of conductivity cells and how conductometric titrations work by measuring changes in conductance during titrations. Examples of various acid-base titrations are given. Conductometric titrations can be used to analyze many different samples and have advantages like not requiring indicators. Applications include measuring water pollution, food analyses, and more.
This document discusses conductometric titration, which is an electrochemical analytical method that measures the electrical conductance of an electrolyte solution. It describes the principles and instrumentation of conductometry, including how conductivity is measured using a conductivity meter or by performing a titration. Some key applications of conductometric titration are determining the end point of acid-base and precipitation titrations, and it has various uses in fields like environmental analysis, food testing, and quality control.
Polarographic technique is applied for the qualitative or quantitative analysis of electroreducible or oxidisable elements or groups.
It is an electromechanical technique of analyzing solutions that measures the current flowing between two electrodes in the solution as well as the gradually increasing applied voltage to determine respectively the concentration of a solute and its nature.
The principle in polarography is that a gradually increasing negative potential (voltage) is applied between a polarisable and non-polarisable electrode and the corresponding current is recorded.
Polarisable electrode: Dropping Mercury electrode
Non-polarisable electrode: Saturated Calomel electrode
From the current-voltage curve (Sigmoid shape), qualitative and quantitative analysis can be performed. This technique is called as polarography, the instrument used is called as polarograph and the current-voltage curve recorded is called as polarogram
This document discusses electrochemical methods and conductometry. It introduces conductometry as the determination of electrical conductance of an electrolyte solution using a conductometer. Conductometry is based on how ions in solution affect conductivity, which depends on ion type, concentration, temperature and mobility. The principles of conductometry and conductometric titration are explained. Conductometric titration involves substituting ions of one mobility for ions of another mobility until the equivalence point is reached. Examples of different types of titrations such as strong acid-strong base, strong acid-weak base, weak acid-strong base, and weak acid-weak base are provided.
Potentiometric - Pharmaceutical Analysis (101T)RAHUL PAL
Potentiometric methods of analysis measure the potential of electrochemical cells under conditions of zero current. The potential difference between a sensing electrode and a reference electrode is measured. A salt bridge containing an inert electrolyte connects the two half-cells and allows ionic movement to complete the electrical circuit. Common reference electrodes include the standard hydrogen electrode, saturated calomel electrode, and silver-silver chloride electrode. Potentiometry is used for applications such as determining electrode potentials, measuring pH, and analyzing samples in clinical chemistry, environmental chemistry, agriculture, and food processing.
Potentiometry involves measuring the potential of electrochemical cells under conditions of no current flow. There are two types - direct potentiometry measures the potential of indicator electrodes related to analyte concentration, while indirect potentiometry involves measuring potential changes during titrations. A potentiometric cell consists of a reference electrode that maintains a constant potential, an indicator electrode whose potential varies with analyte concentration, and a salt bridge. The Nernst equation describes the relationship between electrode potential and analyte concentration or activity.
This document provides an overview of conductometry and its applications. It discusses Ohm's law and how conductivity is measured using electrodes, standard solutions, and a conductivity cell. Factors that affect conductivity include ion size, temperature, charge, and number. Conductometric titrations can be used to determine endpoints and are advantageous because no indicator is needed. Types of titrations discussed include acid-base, precipitation, replacement, redox, and complexometric. Recent applications include use in refineries, estimating polyelectrolytes, and biotechnology/environmental monitoring.
Complexometric titration involves the titration of a metal ion solution with a chelating agent or ligand until the metal ion forms a stable complex. It is useful for determining mixtures of metal ions. The document discusses various types of complexometric titrations including direct titration, back titration, and replacement titration. It also covers the use of metal ion indicators, masking and demasking reagents, and provides examples of complexometric titration for determining compounds like magnesium sulfate, calcium gluconate, and auric ions in ores.
The document discusses the dropping mercury electrode (DME), which is a working electrode used in polarography where mercury drops from a reservoir through a capillary tube into the solution being analyzed. It provides details on the structure of the DME including the mercury reservoir and capillary tube. The document also describes how the DME works, lists different types of mercury electrodes, and discusses the advantages, disadvantages, and precautions of using the DME.
This document discusses the principles and procedures of conductometric analysis. Conductometric analysis measures the electrical conductivity of a solution due to ion mobility. The conductivity is affected by factors like number, charge, size of ions, and temperature. It involves titrating a solution containing ions and measuring the change in conductivity. This allows determination of the endpoint of the titration from the plotted conductivity-volume curve. The document defines key terms, describes instrumentation including conductivity cells and electrodes, and discusses different types of conductometric titrations like acid-base, redox, and complexometric titrations. Conductometric titrations provide accurate results for analyses without requiring indicators.
Polarography uses a dropping mercury electrode (DME) to measure the current flowing through an electrochemical cell as a function of the applied potential. A polarogram plots this current versus potential and provides qualitative and quantitative information about species undergoing oxidation or reduction reactions. Jaroslav Heyrovsky invented the polarographic method in 1922 and won the Nobel Prize for his contributions to electroanalytical chemistry. All modern voltammetric methods originate from polarography. The DME provides advantages like a reproducible surface area and the ability to form amalgams with metal ions.
Potentiometry uses a reference electrode and an indicator electrode to measure the potential difference in a sample solution. When the electrodes are placed in the solution, the potential is generated based on the concentration of ions present. There are several types of potentiometric titrations including acid-base, redox, complexometric, and precipitation titrations. Potentiometry has many applications in fields like clinical chemistry, environmental analysis, potentiometric titrations, agriculture, detergent manufacturing, food processing and more. It is used to analyze important ions and determine equivalence points during titrations.
It is an electrochemical method of analysis used for the determination or measurement of the electrical conductance of an electrolyte solution by means of a conductometer.
Electric conductivity of an electrolyte solution depends on :
Type of ions (cations, anions, singly or doubly charged
Concentration of ions
Temperature
Mobility of ions
The main principle involved in this method is that the movement of the ions creates the electrical conductivity. The movement of the ions is mainly depended on the concentration of the ions.
The electric conductance in accordance with ohms law which states that the strength of current (i) passing through conductor is directly proportional to potential difference & inversely to resistance.
i =V/R
This document discusses conductometry, which is a method of analysis based on measuring the electrolytic conductance of a solution. It begins by classifying different electrochemical methods, including conductometry and electrophoresis which do not involve redox reactions. It then discusses key concepts in conductometry such as conductivity, conductance, equivalent conductance, and how various factors like ion nature, temperature, concentration, and electrode size affect conductance. It also provides examples of calculating conductance and equivalent conductance from experimental measurements. Instrumentation for conductometric determination includes a conductance cell and conductivity bridge.
Potentiometry involves measuring the potential or electromotive force of a sample solution using an electrochemical cell containing a reference electrode and an indicator electrode. The potential is directly proportional to the ion concentration in the solution. Common reference electrodes include the standard hydrogen electrode, silver chloride electrode, and saturated calomel electrode. Indicator electrodes can be metal electrodes or ion-selective electrodes like the glass membrane pH electrode. Potentiometric titration determines the concentration of an analyte by measuring the potential change as a titrant is added, with the endpoint indicated by an abrupt potential shift. Applications of potentiometry include acid-base, redox, complexometric, and precipitation titrations.
more chemistry contents are available
1. pdf file on Termmate: https://www.termmate.com/rabia.aziz
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EDTA Titration
Amperometric titration involves measuring the electric current produced by a titration reaction while keeping the voltage constant between electrodes. It can determine the endpoint of titrations involving an electroreducible ion being titrated with a counter ion. The diffusion current is measured and plotted against the titrant volume added. At the endpoint, there is a sharp change in current. Amperometric titration offers advantages like rapid analysis, ability to work with dilute solutions, and determination of insoluble substances. It finds applications in areas like determining water content and quantification of ions.
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.
This document discusses precipitation titration methods. It describes Mohr's method, Volhard's method and Fajan's method. Mohr's method uses potassium chromate as an indicator. Volhard's method indirectly titrates excess silver ions with thiocyanate using ferric ammonium sulfate as an indicator. Fajan's method uses adsorption indicators like fluorescein that change color upon adsorption to the precipitate formed at the endpoint. Key factors that influence precipitation titrations like solubility products, common ion effect and temperature are also discussed.
This document discusses redox titrations and provides examples of different types of titrations including acid-base, complexometric, precipitation, and redox titrations. It defines oxidation and reduction in terms of the gain or loss of electrons. Redox titrations involve the transfer of electrons between reactants. The document provides examples of balancing redox equations using half-reactions and discusses how oxidation numbers are used to identify oxidation and reduction in redox reactions.
Conductometry is an electrochemical method of analysis involve the measurement of the electrical conductivity of a solution. The conductance is defined as the current flow through the conductor.
In other words, it is defined as the reciprocal of the resistance.
DETERMINATION OF STRENGTH OF MIXTURE USING CONDUCTOMETRY METHOD.pdfGangapuramRohith
This document describes a laboratory experiment on conductometric titration conducted by students to determine the strength of a mixture of acetic acid and hydrochloric acid. The students measured the conductance of the mixture as it was titrated with sodium hydroxide solution. By plotting a graph of conductance versus volume of sodium hydroxide added, they determined the equivalence points that corresponded to the neutralization of hydrochloric acid and acetic acid. From these volumes and the normality of the sodium hydroxide solution, they calculated the normalities or strengths of the hydrochloric acid and acetic acid in the original mixture to be 0.075 N and 0.10 N respectively.
Conductometry measures the conductivity or resistance of a solution between two electrodes. Only ionizable molecules conduct electricity, and the magnitude of conductivity depends on the amount of ions present. Conductivity is affected by electrolyte type, concentration, and temperature. Conductometry is used to determine ion concentrations through titrations, where changes in conductivity indicate the equivalence point. It can be applied to dilute, colored, or turbid solutions where other methods cannot be used. Typical titration curves show changes in conductivity as strong/weak acids and bases are neutralized.
Amperometry is an electroanalytical technique that measures current using an amperometer. It can be used for titrations where the endpoint is determined by measuring the electric current produced by the titration reaction. In amperometric titration, the voltage is kept constant and the diffusion current passing through the cell is measured and plotted against the reagent volume added. Diffusion current is produced when charge carriers move from a higher concentration region to a lower concentration region. Amperometric titration is accurate and can determine traces of elements. It has advantages over other methods and is commonly used to titrate reducible and non-reducible substances.
This document provides an overview of conductometry and its applications. It discusses Ohm's law and how conductivity is measured using electrodes, standard solutions, and a conductivity cell. Factors that affect conductivity include ion size, temperature, charge, and number. Conductometric titrations can be used to determine endpoints and are advantageous because no indicator is needed. Types of titrations discussed include acid-base, precipitation, replacement, redox, and complexometric. Recent applications include use in refineries, biotechnology, and environmental monitoring.
Conductometry is a simple electroanalytical technique that measures the ability of a solution to conduct electricity via ion movement. Conductivity depends on the number and mobility of ions present. Factors like ion size/hydration, temperature, and viscosity affect ion mobility. Specific conductance and molar conductance are used to compare conductivities between solutions. Conductometric titrations can determine endpoints accurately without indicators and are used to analyze solubility, equilibria, salinity, and more. Titration curves are plotted from changes in conductivity as a function of titrant added.
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Physical Chemistry
This document provides an overview of conductometry, including:
1. The principles of conductometry involve measuring the electrical conductance of an electrolyte solution using a conductometer. Conductance depends on ion type, concentration, temperature, and mobility.
2. Instrumentation includes a current source, conductivity cells with platinum electrodes, and a conductance bridge to measure resistance and calculate conductivity.
3. Conductometric titrations can be used for acid-base, redox, precipitation, and complexometric titrations. They do not require indicators and can be used for colored or turbid solutions.
This document provides an overview of conductometry, including:
1. The principles of conductometry involve measuring the electrical conductance of an electrolyte solution using a conductometer. Conductance depends on ion type, concentration, temperature, and mobility.
2. Instrumentation includes a current source, conductivity cells with platinum electrodes, and a conductance bridge to measure resistance and calculate conductivity.
3. Conductometric titrations can be used for acid-base, redox, precipitation, and complexometric titrations. They do not require indicators and can be used for colored or turbid solutions.
Conductometry is used to analyze ionic species and to monitor a chemical reaction by studying the electrolytic conductivity of the reacting species or the resultant products.
Introduction
Ohm’s law.
Conductometric measurements.
Factor affecting conductivity.
Application of conductometry.
2.Conductometric titration-:
Introduction.
Types of conductometric tiration.
Advantages of conductometric tiration.
3.Recent devlopement
Conductometry:
is the simplest of the electroanalytical techniques; by Kolthoff in 1929.
Conductors are:
either metallic (flow of electrons) or electrolytic (movemenmt of ions).
Conductance of electricity:
migration of positively charged ions towards the cathode and negatively charged ones towards the anode
(i.e.) current is carried by all ions present in solution.
Conductance depends on the number of ions in solun.
Factors affecting conductance:
1- Temperature:
(1C increase in temperature causes 2 % increase in conductance).
2- Nature of ions
Size, molecular weight and number of charges.
3- Concentration of ions:
As the number of ions increases, the conductance increases.
4- Size of electrodes
Conductance is directly proportional to the cross sectional area (A).
1. Electrochemistry deals with the production of electricity from chemical reactions and use of electricity to cause non-spontaneous reactions.
2. Conductors are classified as metallic conductors which allow current by electron movement and electrolytic conductors which allow current through dissolved or molten state with chemical decomposition.
3. Electrolytes are classified as strong which completely dissociate and weak which partially dissociate. Conductivity is directly proportional to concentration and inversely proportional to length.
This document provides an introduction to conductometric titrations. It explains that conductometric titrations measure the change in conductivity at the endpoint of a titration reaction. The document discusses the principles behind conductivity changes during titrations and the apparatus used. It then describes the procedure for conductometric titrations and plots the results. Finally, it provides examples of different types of conductometric titrations including neutralization, redox, and precipitation titrations.
Coulometry is an electrochemical method that measures the current needed to completely oxidize or reduce an analyte. There are two forms: controlled potential and controlled current. Controlled potential coulometry applies a constant potential to ensure 100% current efficiency and quantitative reaction of the analyte without interfering species. The decreasing current over time corresponds to decreasing analyte concentration. Controlled current coulometry passes a constant current, allowing more rapid analysis since current does not decrease over time. The total charge simply equals current multiplied by time. Coulometry provides precise, sensitive, and selective analysis of inorganic and organic compounds and can be adapted to automatic titration methods.
Aquas solution electrical conductivity (k) calculation د. shaltout
- Conductivity is a measure of a solution's ability to conduct electricity, which depends on the presence, concentration, mobility, and charge of ions in the solution.
- Conductivity is measured between two electrodes and reported in units of micromhos per centimeter or millisiemens per meter.
- A solution's conductivity is directly proportional to the electrode surface area and inversely proportional to the distance between electrodes.
Conductivity measurement involves measuring how well a solution conducts electricity. There are two main types of conductivity sensors:
1. Contacting sensors which use electrodes in contact with the solution and can measure low conductivities. They are susceptible to fouling.
2. Inductive (toroidal) sensors which do not contact the solution and can be used in dirty applications. They require a minimum conductivity of 15 μS/cm.
Proper calibration and temperature compensation are important for accuracy. Contacting sensors are calibrated using standard solutions while inductive sensors require in-situ calibration accounting for installation effects. Temperature compensation considers the nonlinear increase in water conductivity and solute type.
Conductometry / conductometric titrationRabia Aziz
more chemistry contents are available
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conductometric titration
Barium sulfate, for example, is insoluble and remains as BaSO4 (s) when added to water, and thus cannot affect the concentration of the water. Magnesium hydroxide is only slightly soluble, so even though the ions conduct well, their concentration is low and there is little conductance in a solution above solid Mg(OH)2.
Conductometry is a technique that measures the electrical conductivity of a solution during a chemical reaction or titration. It works on the principle that conductivity changes as ions are replaced by other ions. The instrumentation includes a conductivity cell with electrodes, a current source, and a conductivity meter. Conductometry has applications in determining water quality, solubility of salts, and as an analytical technique for titrations. It provides accurate results but is limited for some redox titrations where hydronium ion concentration masks conductivity changes.
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9
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2. INTRODUCTION OF CONDUCTOMETRY
2
conductometry is a measurement of electrolytic conductivity to monitor a
progress of chemical reaction. Conductometry has notable application in analytical
chemistry, where conductometric titration is a standard technique. In usual
analytical chemistry practice, the term conductometry is used as a synonym
of conductometric titration, while the term conductimetry is used to describe non-
Titrative applications. Conductometry is often applied to determine the total
conductance of a solution or to analyze the end point of titrations that include ions.
In this type of titration, upon the continuous addition of the titrant (and the
continuous recording of the corresponding change in electrolytic conductivity), a
sudden change in the conductivity implies that the stoichiometric point has been
reached. The increase or decrease in the electrolytic conductivity in the
conductometric titration process is linked to the change in the concentration of the
hydroxyl and hydrogen ions (which are the two most conducting ions).
The strength of an acid can be determined via conductometric titration with a
standard solution of a base. An example of a curve plotted for such a titration process
is given below.
3. 3h
The method of conductometric titration is very useful in the titration of homogeneous
suspensions or coloured solutions as these titrations cannot be done with the use of
normal chemical indicators.
4. 4
Conductometry means measuring the conductivity of ionic solutions caused by
mobility of ions towards respective electrodes in presence of an electric field.
Conductivity is measured by using conductometer.
Units of conductivity is mhos(Ω-1).
Conductivity is generally measured by using a Wheatstone bridge circuit and a
conductivity cell made of platinum.
𝑅 = 𝑉/𝑖 V-potential difference in volts
i-current in amperes
𝐶 = 1/𝑅
Total conductance of the solution is directly proportional to the sum of the n individual ion
contributions .
G = cim,i
5. 5
Ohm’s Law
The magnitude of conductometric titration is based on ohm’s law.
𝒊 = 𝒆/R
where,
i = current in amperes
e = potential difference
R = resistance in ohm’s
Conductivity Measurements
1.Electrodes
Two parallel platinized Pt. foil electrodes or Pt. black with
electrodeposited a porous Pt. film which increases the surface
area of the electrodes and further reduces faradaic polarization.
6. 6
2.Primary standard solutions
Primary standard KCl solution ,at 25℃, 7.419g of KCl in 1000g of solution has a specific
conductivity of 0.01286Ω-1/cm.
3. Conductivity Cell :
Avoid the change of temperature during determination.
4.Wheat stone bridge :
7. 7
Factors Affecting Conductivity
Size of ions
Temperature
Number of ions
Charge of ions
Specific conductivity:-It is conductivity offered by a substance of 1cm length and
1sq.cm surface area. units are mhos/cm.
Equivalent conductivity:-it is conductivity offered by a solution containing
equivalent weight of solute in it.
8. 8
Analytical chemistry studies and uses
instruments and methods used to separate, identify,
and quantify matter. In practice, separation,
identification or quantification may constitute the entire
analysis or be combined with another method. Separation
isolates analytes. Qualitative analysis identifies analytes,
while quantitative analysis determines the numerical
amount or concentration.
Classical qualitative methods use separations such
as precipitation, extraction, and distillation.
Identification may be based on differences in color, odor,
melting point, boiling point, radioactivity or reactivity.
Classical quantitative analysis uses mass or volume
changes to quantify amount. Instrumental methods may
be used to separate samples
using chromatography, electrophoresis or field flow
fractionation. Then qualitative and quantitative analysis
can be performed, often with the same instrument and
may use light interaction, heat interaction, electric
fields or magnetic fields.
Analytical Chemical
Laboratory
9. 9
Principle
The principle of the conductometric titration process can be stated as follows –
During a titration process, one ion is replaced with another and the difference
in the ionic conductivities of these ions directly impacts the overall electrolytic
conductivity of the solution.
It can also be observed that the ionic conductance values vary between cations and
anions. Finally, the conductivity is also dependent upon the occurrence of a chemical
reaction in the electrolytic solution.
Theory
The theory behind this type of titration states that the end-point corresponding to the
titration process can be determined by means of conductivity measurement. For a
neutralization reaction between an acid and a base, the addition of the base would
lower conductivity of the solution initially. This is because the H+ ions would be
replaced by the cationic part of the base.
After the equivalence point is reached, the concentration of the ionic entities will
increase. This, in turn, increases the conductance of the solution. Therefore, two
straight lines with opposite slopes will be obtained when the conductance values are
plotted graphically. The point where these two lines intersect is the equivalence point.
10. 10
Process
For the conductometric titration of an acid with a base, the general process is as follows:
10 ml of the acid must be diluted with approximately 100 ml of distilled water (so that the
changes in the conductance brought on by the addition of the base become small).
A burette must now be filled with the base and the initial volume must be noted.
In this step, a conductivity cell must be inserted into the diluted acid solution in a way
that both the electrodes are completely immersed.
Now, the conductivity cell can be connected to a digital conductometer in order to obtain
an initial reading.
The base must now be added drop wise into the acid solution. The volume of base added
must be noted along with the corresponding change in the conductance.
A sharp increase in the conductance of the solution implies that the endpoint has been
reached. However, a few more readings must be taken after the endpoint of the titration.
These observed values must now be plotted graphically. The equivalence point can be
obtained from the point of intersection between the two lines.
The strength of the acid can now be calculated via the formula S2 = (V1S1)/10; where S2 is
the strength of the acid, V1 is the volume of base added (as per the equivalence point on
the conductometric titration graph), and S1 is the strength of the base (already known).
Here, the volume of the acid (V2) is equal to 10 ml.
11. 11
Advantages and Disadvantages of Conductometric
Titration
Some advantages of the conductometric titration process are listed below.
This process is very useful in the titrations of very dilute solutions and weak acids.
The end-point of this method of titration is very sharp and accurate when compared to a
few other titration processes.
This type of titration is applicable for solutions that are coloured or turbid, and for which
the endpoint of the titration with normal indicators cannot be observed easily by the
human eye.
Conductometric titration has numerous applications in acid-base titrations, redox
titrations, precipitation titrations, and complex titrations.
The two major disadvantages of this type of titration include:
Only a few specific redox titrations can be done with the help of this process. This is
because the conductivity of the solution is masked by relatively high hydronium ion
concentration.
The accuracy of conductometric titration is low when the concentrations of the
electrolyte are high, making the titration process unsatisfactory.
12. APPLICATIONS OF CONDUCTOMETRY
It can be used for the determination of:-
Solubility of sparingly soluble salts
Ionic product of water
Basicity of organic acids
Salinity of sea water (oceanographic work)
Chemical equilibrium in ionic reactions
Conductometric titration
12
Conductometric Titration-:
Introduction.
Types of conductometric tiration.
Advantages of conductometric tiration.
13. CONDUCTOMETRIC TITRATIONS:
The determination of end point of a titration by
means of conductivity measurements are known
as conductometric titrations.
13
14. ACID-BASE TITRATIONS
• Titration of strong acid
(a) with strong base e.g. HCl with NaOH
(b) with weak base e.g. HCl with NH4OH
14
Types of conductometric titrations:
15. • Titration of weak acid
(c) with strong base e.g. CH3COOH with NaOH
(d) with weak base e.g. CH3COOH with NH4OH
15
17. REPLACEMENT TITRATIONS
Salt of strong acid and weak base vs.
strong base
Ex: ammonium chloride vs. sodium
hydroxide
Salt of strong base and weak acid vs.
strong acid
Eg: sodium acetate vs. hydrochloric acid
17
21. COMPLEXOMETRIC TITRATION
Ex.:-KCl vs. Hg(ClO4)2
Non-aqueous titrations can also be measured
using conductometry.
Ex:-
a)titration of weak bases vs. perchloric acid in
dioxan-formic acid.
b)Titration of weak organic acids in methanol vs.
tetra methyl ammonium hydroxide in methanol-
benzene.
21
22. 22
RECENT DEVLOPEMNTS
In refinary industries.
Estimation of polyelectrolytic solution.
Biotechnology.
Microbiosensors for enviromental monitoring.