Potentiometric titration uses a potentiometer to determine the concentration of an analyte in solution. A potentiometer consists of an indicator electrode and a reference electrode placed in the solution. The potential difference between the electrodes is measured as titrant is added. When the endpoint of the titration is reached, there is an abrupt change in the measured potential that can be used to calculate the concentration of analyte. Potentiometric titration is a common volumetric technique used in electroanalytical chemistry.
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.
ESTIMATION OF THE RATE OF REACTION WILL BE DONE BASED ON THE POTENTIAL DIFFERENCE BETWEEN REFERENCE AND INDICATOR ELECTRODE. THE POTENTIAL OF THE REFERENCE ELECTRODE IS STABLE WHERE AS THE POTENTIAL OF THE INDICATOR ELECTRODE VARIES WITH THE POTENTIAL OF THE SOLUTION IN WHICH IT IS PLACED
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.
Potentiometry involves measuring the potential difference between two electrodes under equilibrium conditions. There are two main types of electrodes - reference electrodes that maintain a constant potential, and indicator or working electrodes whose potential varies with ion concentration. Common reference electrodes include the standard hydrogen electrode, saturated calomel electrode, and silver/silver chloride electrode. Indicator electrodes include glass membrane electrodes for measuring pH and ion-selective electrodes that respond selectively to specific ions. Potentiometry is used for pH measurements, ion-selective measurements, and potentiometric titrations.
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
Potentiometry is an analytical technique that measures the potential of electrochemical cells without drawing current. It involves using a reference electrode with a known potential and an indicator electrode whose potential varies with analyte concentration. The cell potential is measured and related to concentration using the Nernst equation. Common reference electrodes include the standard hydrogen electrode and saturated calomel electrode. Glass membrane and ion-selective electrodes are often used as indicator electrodes to detect specific ions like hydrogen or fluoride ions. Potentiometry finds applications in clinical analysis, environmental monitoring, and titration experiments.
Potentiometry is an electroanalytical technique where the potential difference between two electrodes is measured under conditions of no current flow. It was invented in 1841 by Johann Christian Poggendorff using a slide-wire potentiometer. A potentiometric cell consists of a reference electrode with a known potential and an indicator electrode, whose potential changes depending on the analyte concentration. The potential difference between the electrodes is measured to determine the analyte concentration. Common applications of potentiometry include titrations, analysis of pollutants, drugs, foods, and more.
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.
ESTIMATION OF THE RATE OF REACTION WILL BE DONE BASED ON THE POTENTIAL DIFFERENCE BETWEEN REFERENCE AND INDICATOR ELECTRODE. THE POTENTIAL OF THE REFERENCE ELECTRODE IS STABLE WHERE AS THE POTENTIAL OF THE INDICATOR ELECTRODE VARIES WITH THE POTENTIAL OF THE SOLUTION IN WHICH IT IS PLACED
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.
Potentiometry involves measuring the potential difference between two electrodes under equilibrium conditions. There are two main types of electrodes - reference electrodes that maintain a constant potential, and indicator or working electrodes whose potential varies with ion concentration. Common reference electrodes include the standard hydrogen electrode, saturated calomel electrode, and silver/silver chloride electrode. Indicator electrodes include glass membrane electrodes for measuring pH and ion-selective electrodes that respond selectively to specific ions. Potentiometry is used for pH measurements, ion-selective measurements, and potentiometric titrations.
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
Potentiometry is an analytical technique that measures the potential of electrochemical cells without drawing current. It involves using a reference electrode with a known potential and an indicator electrode whose potential varies with analyte concentration. The cell potential is measured and related to concentration using the Nernst equation. Common reference electrodes include the standard hydrogen electrode and saturated calomel electrode. Glass membrane and ion-selective electrodes are often used as indicator electrodes to detect specific ions like hydrogen or fluoride ions. Potentiometry finds applications in clinical analysis, environmental monitoring, and titration experiments.
Potentiometry is an electroanalytical technique where the potential difference between two electrodes is measured under conditions of no current flow. It was invented in 1841 by Johann Christian Poggendorff using a slide-wire potentiometer. A potentiometric cell consists of a reference electrode with a known potential and an indicator electrode, whose potential changes depending on the analyte concentration. The potential difference between the electrodes is measured to determine the analyte concentration. Common applications of potentiometry include titrations, analysis of pollutants, drugs, foods, and more.
This document discusses potentiometry, which is a method of measuring electrical potential or electromotive force (emf) of a solution using indicator and reference electrodes. It describes the components of a potentiometric cell including the reference electrode, salt bridge, analyte solution, and indicator electrode. Various types of reference electrodes like standard hydrogen, saturated calomel, and silver/silver chloride electrodes are explained. The document also covers different types of indicator electrodes like metallic electrodes, membrane electrodes, and gas sensing probes. Direct potentiometry and potentiometric titration techniques are briefly mentioned.
This document provides an overview of potentiometry and related electroanalytical techniques. It defines key concepts like reference electrodes, indicator electrodes, and salt bridges used in potentiometric cells. Equations for electrode potentials are described for various metal-metal ion systems. Membrane electrodes like glass pH electrodes are also summarized. The document concludes with brief discussions of potentiometric titration techniques and voltammetry methods.
Electrogravimetric analysis involves the quantitative deposition of an analyte onto an electrode through electrolysis. There are two main types: constant current electrolysis, where the current is kept constant and the potential varies, and controlled potential electrolysis, where the potential is kept constant to selectively deposit analytes. Electrogravimetric analysis can be used for quantitative analysis, separation, preconcentration of analytes, and electrosynthesis.
Voltammetry is a technique where a time-dependent potential is applied to an electrochemical cell and the current is measured as a function of the applied potential. This results in a voltammogram which provides qualitative and quantitative information about redox reactions. The earliest technique was polarography developed in the 1920s. Modern voltammetry uses a three-electrode system with various excitation signals applied. Common techniques include normal pulse polarography, differential pulse polarography, staircase polarography and square wave polarography which have better sensitivity than normal polarography. The shape of the voltammetric wave depends on factors like the reversibility of the redox reaction. The diffusion current occurs at very negative potentials where the reaction rate is controlled by diffusion
This document discusses reference electrodes, which maintain a constant potential regardless of current. It describes how reference electrodes establish a reference point for measuring potential in voltammetric methods. An ideal reference electrode uses stable, well-defined half-cell components. The standard hydrogen electrode (SHE) is described as the reference, but it is impractical, so saturated calomel electrodes (SCE) and silver/silver chloride electrodes are commonly used instead as they offer stable, reproducible potentials. The SCE consists of mercury coated with mercurous chloride paste and immersed in saturated potassium chloride solution, while the Ag/AgCl electrode uses silver wire coated with solid silver chloride in saturated potassium chloride solution.
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.
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.
Potentiometry is an electrochemical method of Analysis deals with the measurement of electric potential or emf of an electrolyte solution under the condition of constant current.
Potentiometry is the measurement of electrical potential of an electrolyte solution to determine its concentration.
The principle is based on the fact that the potential of the given sample is directly proportional to the concentration of its electro active ions or its activity (pH)
When the pair of electrodes is placed in the sample solution it shows the potential difference by the addition of the titrant or by the change in the concentration of the ions.
The theory of potentiometry is based on the nernst equation.It gives the basic relationship between the potential generated by an electrochemical cell and the concentration of the ions.
The potential E ( Half cell potential) of any electrode is given by nernst equation
This document discusses potentiometry, which is an electroanalytical technique that measures the potential (voltage) of electrochemical cells containing indicator and reference electrodes. It involves using electrodes to measure voltages generated from chemical reactions. Various types of electrodes are described including metal, ion-selective, glass membrane, liquid membrane, and crystalline membrane electrodes. Applications of potentiometry include ion concentration measurements, pH measurements, and potentiometric titrations.
This document provides an overview of coulometry, which is an electroanalytical technique used for quantitative analysis. There are two forms of coulometry: controlled-potential coulometry and controlled-current coulometry. Both techniques involve completely oxidizing or reducing an analyte and measuring the total charge passed to determine the amount of analyte. Controlled-potential coulometry applies a constant potential while controlled-current coulometry applies a constant current. Factors like electrolysis time, electrode area, and stirring rate affect the analysis. Coulometry is used to quantify both inorganic and organic analytes.
This document discusses different types of electrodes used in electroanalytical chemistry. It describes inert electrodes like platinum, gold and graphite that do not participate in reactions, and reactive electrodes like zinc, copper and lead that actively participate in reactions. The document discusses various types of electrodes in detail, including glass electrodes, liquid ion exchanger membranes, solid state membranes, neutral carrier membranes, coated wire electrodes, and ion selective field effect transistors. It also outlines the principle, advantages, limitations and applications of ion selective electrodes.
Polarographic analysis is a voltammetry technique that uses a dropping mercury electrode (DME) or static mercury drop electrode (SMDE) to measure the current resulting from the electrolysis of electroactive species at controlled potentials. It involves applying a potential between a mercury working electrode and a reference electrode, like a saturated calomel electrode, while measuring the current. The current-voltage curve, or polarogram, reveals information about the species present in solution, including qualitative and quantitative analysis through measurements of diffusion current and half-wave potential. Polarography takes advantage of mercury's wide cathodic potential range and its ability to renew its surface between drops.
Potentiometry involves measuring electrode potentials using a reference electrode and indicator electrode. The reference electrode maintains a constant potential while the indicator electrode's potential varies with analyte concentration. Common reference electrodes include the saturated calomel electrode and silver-silver chloride electrode. Indicator electrodes include pH electrodes, ion-selective electrodes, and redox electrodes. Potentiometric measurements are used in clinical chemistry, environmental monitoring, titrations, and various industrial applications like food processing.
Polarography is an electrochemical technique used to analyze reducible or oxidizable substances in solution. It involves varying the electric potential between a dropping mercury electrode and a reference electrode while monitoring the current. A polarogram is generated by plotting the current readings against the applied voltage. Key features of polarography include applied voltages between 0-2.5V and current values between 0.12-100 microamperes. Polarography finds applications in pharmaceutical analysis such as determining dissolved oxygen, trace metals in drugs, vitamins, hormones, antibiotics, and diagnosing cancer from blood serum.
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
It contains what is amperometry and where it will be derived and what is the principle behind the amperometry. Instrumentation of amperometry and the purpose of dipping mercury electrode and rotating platinum electrode. The advantage over rotating platinum electrodes. Amperometric titration curves for reducible ions and non-reducible ions. What tells the Ilkovic equation and how it relates to the amperometry is also included. Applications, advantages, and disadvantages of amperometric titration are also included. Questions related to amperometry and amperometric titration are given for practice. The contents taken from the websites are also given.
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.
Potentiometry is an electroanalytical technique that measures the electric potential of electrochemical cells under zero-current conditions. It involves measuring the potential difference between a reference electrode with a known potential and an indicator electrode whose potential varies with the concentration of the analyte ion. The potential difference is used to determine analyte concentration based on the Nernst equation. Common applications of potentiometry include clinical analysis of electrolytes, environmental analysis of ions in water, and titration measurements.
This document provides information on potentiometry and potentiometric titration. It discusses the basic principles of potentiometry including electrode potentials and how a potential difference is established between an electrode and solution. It describes the instrumentation used including reference electrodes like calomel and silver-silver chloride electrodes and indicator electrodes like metal, glass membrane, and quinhydrone electrodes. It also discusses different types of potentiometric titrations and provides examples of applications for potentiometry in various industries.
This document discusses potentiometry, which is a method of analysis that determines concentration by measuring potential difference between two electrodes without current flow. It describes the principle, reference electrodes like standard hydrogen electrode and saturated calomel electrode, indicator electrodes like glass electrode, and how potentiometric titration can determine the endpoint using methods like the normal titration curve, first derivative curve, and second derivative curve. Potentiometry provides advantages over visual indicator methods by not requiring indicators and allowing the same instrument to be used for different titrations.
This document discusses potentiometry, which is a method of measuring electrical potential or electromotive force (emf) of a solution using indicator and reference electrodes. It describes the components of a potentiometric cell including the reference electrode, salt bridge, analyte solution, and indicator electrode. Various types of reference electrodes like standard hydrogen, saturated calomel, and silver/silver chloride electrodes are explained. The document also covers different types of indicator electrodes like metallic electrodes, membrane electrodes, and gas sensing probes. Direct potentiometry and potentiometric titration techniques are briefly mentioned.
This document provides an overview of potentiometry and related electroanalytical techniques. It defines key concepts like reference electrodes, indicator electrodes, and salt bridges used in potentiometric cells. Equations for electrode potentials are described for various metal-metal ion systems. Membrane electrodes like glass pH electrodes are also summarized. The document concludes with brief discussions of potentiometric titration techniques and voltammetry methods.
Electrogravimetric analysis involves the quantitative deposition of an analyte onto an electrode through electrolysis. There are two main types: constant current electrolysis, where the current is kept constant and the potential varies, and controlled potential electrolysis, where the potential is kept constant to selectively deposit analytes. Electrogravimetric analysis can be used for quantitative analysis, separation, preconcentration of analytes, and electrosynthesis.
Voltammetry is a technique where a time-dependent potential is applied to an electrochemical cell and the current is measured as a function of the applied potential. This results in a voltammogram which provides qualitative and quantitative information about redox reactions. The earliest technique was polarography developed in the 1920s. Modern voltammetry uses a three-electrode system with various excitation signals applied. Common techniques include normal pulse polarography, differential pulse polarography, staircase polarography and square wave polarography which have better sensitivity than normal polarography. The shape of the voltammetric wave depends on factors like the reversibility of the redox reaction. The diffusion current occurs at very negative potentials where the reaction rate is controlled by diffusion
This document discusses reference electrodes, which maintain a constant potential regardless of current. It describes how reference electrodes establish a reference point for measuring potential in voltammetric methods. An ideal reference electrode uses stable, well-defined half-cell components. The standard hydrogen electrode (SHE) is described as the reference, but it is impractical, so saturated calomel electrodes (SCE) and silver/silver chloride electrodes are commonly used instead as they offer stable, reproducible potentials. The SCE consists of mercury coated with mercurous chloride paste and immersed in saturated potassium chloride solution, while the Ag/AgCl electrode uses silver wire coated with solid silver chloride in saturated potassium chloride solution.
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.
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.
Potentiometry is an electrochemical method of Analysis deals with the measurement of electric potential or emf of an electrolyte solution under the condition of constant current.
Potentiometry is the measurement of electrical potential of an electrolyte solution to determine its concentration.
The principle is based on the fact that the potential of the given sample is directly proportional to the concentration of its electro active ions or its activity (pH)
When the pair of electrodes is placed in the sample solution it shows the potential difference by the addition of the titrant or by the change in the concentration of the ions.
The theory of potentiometry is based on the nernst equation.It gives the basic relationship between the potential generated by an electrochemical cell and the concentration of the ions.
The potential E ( Half cell potential) of any electrode is given by nernst equation
This document discusses potentiometry, which is an electroanalytical technique that measures the potential (voltage) of electrochemical cells containing indicator and reference electrodes. It involves using electrodes to measure voltages generated from chemical reactions. Various types of electrodes are described including metal, ion-selective, glass membrane, liquid membrane, and crystalline membrane electrodes. Applications of potentiometry include ion concentration measurements, pH measurements, and potentiometric titrations.
This document provides an overview of coulometry, which is an electroanalytical technique used for quantitative analysis. There are two forms of coulometry: controlled-potential coulometry and controlled-current coulometry. Both techniques involve completely oxidizing or reducing an analyte and measuring the total charge passed to determine the amount of analyte. Controlled-potential coulometry applies a constant potential while controlled-current coulometry applies a constant current. Factors like electrolysis time, electrode area, and stirring rate affect the analysis. Coulometry is used to quantify both inorganic and organic analytes.
This document discusses different types of electrodes used in electroanalytical chemistry. It describes inert electrodes like platinum, gold and graphite that do not participate in reactions, and reactive electrodes like zinc, copper and lead that actively participate in reactions. The document discusses various types of electrodes in detail, including glass electrodes, liquid ion exchanger membranes, solid state membranes, neutral carrier membranes, coated wire electrodes, and ion selective field effect transistors. It also outlines the principle, advantages, limitations and applications of ion selective electrodes.
Polarographic analysis is a voltammetry technique that uses a dropping mercury electrode (DME) or static mercury drop electrode (SMDE) to measure the current resulting from the electrolysis of electroactive species at controlled potentials. It involves applying a potential between a mercury working electrode and a reference electrode, like a saturated calomel electrode, while measuring the current. The current-voltage curve, or polarogram, reveals information about the species present in solution, including qualitative and quantitative analysis through measurements of diffusion current and half-wave potential. Polarography takes advantage of mercury's wide cathodic potential range and its ability to renew its surface between drops.
Potentiometry involves measuring electrode potentials using a reference electrode and indicator electrode. The reference electrode maintains a constant potential while the indicator electrode's potential varies with analyte concentration. Common reference electrodes include the saturated calomel electrode and silver-silver chloride electrode. Indicator electrodes include pH electrodes, ion-selective electrodes, and redox electrodes. Potentiometric measurements are used in clinical chemistry, environmental monitoring, titrations, and various industrial applications like food processing.
Polarography is an electrochemical technique used to analyze reducible or oxidizable substances in solution. It involves varying the electric potential between a dropping mercury electrode and a reference electrode while monitoring the current. A polarogram is generated by plotting the current readings against the applied voltage. Key features of polarography include applied voltages between 0-2.5V and current values between 0.12-100 microamperes. Polarography finds applications in pharmaceutical analysis such as determining dissolved oxygen, trace metals in drugs, vitamins, hormones, antibiotics, and diagnosing cancer from blood serum.
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
It contains what is amperometry and where it will be derived and what is the principle behind the amperometry. Instrumentation of amperometry and the purpose of dipping mercury electrode and rotating platinum electrode. The advantage over rotating platinum electrodes. Amperometric titration curves for reducible ions and non-reducible ions. What tells the Ilkovic equation and how it relates to the amperometry is also included. Applications, advantages, and disadvantages of amperometric titration are also included. Questions related to amperometry and amperometric titration are given for practice. The contents taken from the websites are also given.
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.
Potentiometry is an electroanalytical technique that measures the electric potential of electrochemical cells under zero-current conditions. It involves measuring the potential difference between a reference electrode with a known potential and an indicator electrode whose potential varies with the concentration of the analyte ion. The potential difference is used to determine analyte concentration based on the Nernst equation. Common applications of potentiometry include clinical analysis of electrolytes, environmental analysis of ions in water, and titration measurements.
This document provides information on potentiometry and potentiometric titration. It discusses the basic principles of potentiometry including electrode potentials and how a potential difference is established between an electrode and solution. It describes the instrumentation used including reference electrodes like calomel and silver-silver chloride electrodes and indicator electrodes like metal, glass membrane, and quinhydrone electrodes. It also discusses different types of potentiometric titrations and provides examples of applications for potentiometry in various industries.
This document discusses potentiometry, which is a method of analysis that determines concentration by measuring potential difference between two electrodes without current flow. It describes the principle, reference electrodes like standard hydrogen electrode and saturated calomel electrode, indicator electrodes like glass electrode, and how potentiometric titration can determine the endpoint using methods like the normal titration curve, first derivative curve, and second derivative curve. Potentiometry provides advantages over visual indicator methods by not requiring indicators and allowing the same instrument to be used for different titrations.
Potentiometry is the field of electro-analytical chemistry in which potential is measured without current flow.
It is a method of analysis in which we determine the concentration of solute in solution and the potential difference between two electrodes.
Potentiometry is a technique that measures the potential or electromotive force (emf) of a solution using an indicator electrode and a reference electrode. The potential difference between the two electrodes is dependent on factors like pH, gas concentration, or analyte ion activity in the solution. Common types of electrodes used include glass membrane pH electrodes, ion-selective electrodes with liquid or crystalline membranes, and gas-sensing electrodes. Potentiometric measurements can be carried out via direct measurement, standard addition, or titration to determine analyte concentration.
This document provides an overview of electrochemistry and electrochemical cells. It defines electrochemistry as the study of the relationship between chemical transformations and electrical energy. It describes the two main types of electrochemical cells - electrolytic cells, which convert electrical to chemical energy, and galvanic/voltaic cells, which convert chemical to electrical energy. Key aspects of electrochemical cells covered include the electrodes, electrode charges, redox reactions, cell notation, salt bridges, cell potential, and reference electrodes. The document also discusses indicator electrodes, such as glass pH electrodes and potentiometric titration methods.
This document discusses potentiometry, which is a method of measuring electrical potential or emf to determine the concentration of ions in solution. It describes the components of a potentiometric cell including reference, indicator and salt bridge electrodes. Various types of reference electrodes like hydrogen, calomel and silver/silver chloride electrodes are explained. Indicator electrodes can be metallic, glass membrane, liquid membrane, crystalline membrane or gas sensing probes. Direct potentiometry and potentiometric titration methods for cation/anion analysis are also summarized.
Potentiometry: Electrical potential, electrochemical cell, reference electrodes, indicator
electrodes, measurement of potential and Ph, construction and working of electrodes,
Potentiometric titrations, methods of detecting end point, Karl Fischer titration.
This document discusses electrodes and potentiometry. It introduces potentiometry as using electrodes to measure voltages that provide chemical information. A galvanic cell is used, with an indicator electrode that responds to the analyte and a reference electrode at a constant potential. The cell voltage is the difference between the electrodes. Common reference electrodes include silver-silver chloride and saturated calomel electrodes. Indicator electrodes can be metal electrodes that undergo redox reactions or ion-selective electrodes that selectively bind ions. Glass electrodes are commonly used for pH measurements. Sources of error in pH and other ion-selective electrode measurements are also discussed.
Introduction – cells – types - representation of galvanic cell - electrode potential - Nernst equation (derivation of cell EMF) - calculation of cell EMF from single electrode potential - reference electrode: construction, working and applications of standard hydrogen electrode, standard calomel electrode - glass electrode – EMF series and its applications - potentiometric titrations (redox) - conductometric titrations - mixture of weak and strong acid vs strong base.
This document discusses potentiometry and ion selective electrodes. It begins by explaining that potentiometry measures the potential of an electrochemical cell under static conditions without drawing current. An ion selective electrode uses a selective membrane to measure the concentration of specific ions based on the potential difference between an indicator and reference electrode. The document then describes different types of reference electrodes, indicator electrodes, and ion selective electrodes like glass membrane, solid state, liquid membrane and gas sensing electrodes. It concludes by discussing applications in clinical chemistry, environmental analysis and food processing and advantages like speed and low cost and limitations like precision and interference issues.
Instrumental methods ii and basics of electrochemistryJLoknathDora
1. The document discusses electrochemical cells and instrumentation based on electrochemical properties. It describes the basic components and reactions of galvanic and electrolytic cells.
2. Potentiometric titrations are discussed as a method to determine the equivalence point of a titration based on potential measurements using a reference and indicator electrode. Common indicator electrodes like quinhydrone and glass electrodes are described.
3. The principles of operation of quinhydrone and glass electrodes are summarized, including their Nernst equations and typical cell setups. Advantages and limitations of these indicator electrodes are also mentioned.
This document discusses potentiometry, which involves measuring the potential or emf of a solution using an indicator electrode that responds to changes in potential or pH and a reference electrode with a stable, known potential. It describes common reference electrodes like the hydrogen, saturated calomel, and silver-silver chloride electrodes. It also discusses indicator electrodes like the glass and antimony electrodes and ion-selective electrodes. Potentiometric titrations can be used to determine endpoints by measuring potential changes during titration.
This document discusses various devices used in electrochemical analysis and auxiliary laboratory devices. It describes devices for electrochemical analysis including galvanic cells, electrodes, potentiometry, conductometry, and voltammetry. It also describes auxiliary devices such as centrifuges, shakers, homogenizers, vacuum pumps, thermostats, and air conditioning used to support electrochemical analysis and biomedical research.
This document discusses devices used in electrochemical analysis and auxiliary laboratory devices. It describes galvanic cells, electrodes, and potentiometric devices used to determine ionic composition. It also discusses auxiliary devices like centrifuges and thermostats. Conductometers and coulometers are described which measure conductivity by applying a low voltage alternating current between electrodes to avoid electrolysis. pH meters and glass electrodes are summarized which can directly measure pH by relating the electrode voltage to hydrogen ion concentration.
There are several types of electrodes classified by their composition and function. Reference electrodes like the standard hydrogen electrode (SHE) and saturated calomel electrode (SCE) maintain a known and constant potential used for comparison. The SHE represents the standard reduction potential but is difficult to maintain at standard conditions. The SCE uses a mercury/mercury chloride mixture and is easier to construct and maintain compared to the SHE. Indicator electrodes like the glass electrode are used in titration analysis, with the glass electrode potential indicating pH. Electrodes can also be classified as anodes, which experience oxidation, or cathodes, which undergo reduction.
Potentiometry1 for mpharm ist sem notes prakash64742
The document summarizes potentiometry and potentiometric titrations. Potentiometry uses measurement of electrical potential to perform qualitative and quantitative analysis. The potential of a sample is directly proportional to the activity of electroactive ions present, such as pH. Potentiometric titrations involve direct measurement of electrode potential or changes in potential upon titrant addition to determine the endpoint. Common types include acid-base, redox, complexometric, and precipitation titrations. Choice of reference and indicator electrodes depends on the reaction taking place.
Potentiometry is an electrochemical method that measures potential without current flow. It uses indicator electrodes that generate a potential dependent on analyte concentration combined with a reference electrode that provides a fixed potential. Common reference electrodes include the saturated calomel electrode and silver/silver chloride electrode. Potentiometric methods allow for the rapid, direct determination of ion concentrations through calibration curves or standard addition methods. Special applications include potentiometric pH measurement in unusual samples and potentiometric titrations.
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2. 1. History
2. Definition
3. Principle
4. Potentiometer
5. Electrode potential
6. Construction
7. Working
8. Electrodes
9. Salt bridge
10. Potentiometric titration
11. Applications
Contents:
3.
United States Government, and (2) RUSSELL , citizens
of the United States of America, have invented certain
new and useful improvements like potentiometery.
…
History
CHARLES J.
PATRISSI,
employee of
the
4.
The slide-wire potentiometer was invented by
Johann Christian Poggendorff (1796-1877) in
1841. Leeds and Northrup Type K model was a
standard piece of apparatus in most college and
university electrical measurements laboratories for
the first half of the 20th century
5.
1) Potentiometric
2) Voltammetric, Polarographic, Amperometric
3) Electrolysis: electrogravimetric and coulometric
4) Conductiometric
Here, we will discuss potentiometery.
Four Basic Electroanalytical
Methods of Analysis
6.
Potentiometry is the field of electro analytical
chemistry in which potential is measured under the
condition of no current flow.
OR
Potentiometry is one of volumetric technique of
electro-analytical chemistry.
or
Potentiometrey is the method used in
electroanalytical chemistry usually to find the
concentration of solute in solution in potentiometric
measurement the potential between two electrode is
measured using the high impedance voltmeter
Definition :
7.
When a metal strip is placed in a solution of its
own ions there are two possibilities or tendencies:
Metal atoms may dissolve in the solution as positive
ions leaving electrons on the electrode.
Metal ions may take up electrons from electrode and
get deposited as neutral atoms
In this way A POTENTIAL DIFFERENCE is setup
b/w electrode and solution .
Principle
8.
It is instrument used to determine the potential
differences between a reference electrode and an
indicator electrode. These two electrodes form
electro chemical cell that are dipped in solution to be
analyzed.
Measured potential can be used to determine the
quantity of analyte in terms of concentration.
Potentiometer
10.
Tendency of electrode to lose or gain electrons
Standard Potential
Potential of pure metal when it is dipped in 1
Molar solution of its own ions at 25°C (298K) is
known as standard Electrode potential.
Electrode potential
11.
Oxidation Potential
The potential of substance to get oxidized is called
oxidation potential.
Reduction Potential
The potential of substance to get reduced is called
reduction potential.
15.
Working
At its most basic, a potentiometer consists of two
electrodes, whose reduction potentials differ,
inserted in a test solution. The voltmeter is attached
to the electrodes to measure the potential difference
between them.
One of the electrodes is a reference electrode,
whose electrode potential is known.
The other electrode is the test electrode.
The test electrode is usually either a metal
immersed in a solution of its own ions, whose
concentration you wish to discover, or a carbon rod
electrode sitting a solution which contains the ions
of interest in two different oxidation states.
16.
1. Oxidation take place at anode.
For example on zinc electrode
Zn → Zn2+ + 2e-
1. Reduction take place at cathode.
For example on copper electrode
Cu2+ + 2e−→ Cu
When redox reaction take place than potential is
develop which is measured by galvanometer.
17.
Electrode Potential is the potential of
electrochemical cell and can be
represented as :
E cell = E indicator - E
reference +E j
Ej= potential develops across the liquid
junction at each end of salt bridge it is
negligible .
21.
The standard H2 electrode potential is defined as the potential
that is developed between the H2 gas adsorbed on the pt metal
and H+ of the solution when the H2 gas at a pressure of 760 mm
of Hg is in equilibrium with H+ of unit concentration
Working:
Pt foil : coated with black pt
1 molar HCl solution
Pure H2 gas bubbled continuously at 1 atm.
Pt act as conductor, inert and facilitate in attaining
equilibrium
Electrode Potential is 0.00 volts
H2 (gas) ↔ 2H+ (ions) + 2e- (electrons)
SHE
23.
Limitations :
1. Can’t be used in solution containing strong
oxidizing agents.
2. Difficult and expensive to maintain.
3. Excess of H2 bubbling out carries little HCl with it
and hence the H+ concentration decreases. In such a
system, it is difficult to maintain the concentration
of HCl at 1M.
24. Most commonly used electrode in potentiometry
Tube 5-15cm long, 0.5-1 cm in diameter.
Slurry of mercury & mercurous chloride with saturated
soln of KCl
Connected by a small opening with saturated solution of
KCl.
Pt metal is placed inside the slurry
Ceramic fiber act as salt bridge
2Hg +2Cl¯ → Hg2Cl2 + 2e¯
E = 0.2444 at 25°C
Calomel electrode
26.
Advantages:
Concentration of chloride ions don’t change even
some of the solvent get evaporated.
Generates small junction potential so more accurate
Limitations :
Mostly saturated solution of KCl is used and that is
temperature dependent.
27.
It consist of silver wire coated with AgCl
Coating may be electroplating or Physical.
This coated wire is placed in 1M solution of AgCl.
Ag + Cl¯ ↔ AgCl + 1e¯
E= 0.199V
Advantages:
Easy handling, and cost effective
Limitation: sometimes show reactivity.
Silver-Silver chloride electrode
30.
Metal electrode develops electric potential as a
result of redox reaction at its surface.
1. First Order Electrode
A first order electrode involves the metal in contact
with its own ions, such as Ag, Ag+ or Zn, Zn.
Ag⁺ + e¯ ↔ Ag (s) E= 0.800
Limitation:
metallic indicator electrodes are not very selective
and
respond not only to their own cations but also to other
more easily reduced cations.
– Many metal electrodes can be used only in neutral
or basic solutions because they dissolve in the
presence of acids
Metal Indicator Electrodes
31.
A second-order electrode is one that responds
to the presence of precipitating or
complexing ions. For example, silver wire
could serve as the indicator electrode for
chloride.
Ag +Cl¯ ↔ AgCl + e¯ E= 0.199
2.Second order Electrode
32. The most commonly used indicator electrodes
are known as inert. These electrodes are not
involved in the half-cell reactions of the
electrochemical species. Typical inert
electrodes are platinum, gold, and carbon.
Inert electrodes are responsive to any
reversible redox system; these are widely
used in potentiometric work.
3. Inert Electrode
33.
Its most commonly used indicator
electrode
It involves Ion Exchange reaction
Membrane is made up of chemically
bonded Na2O, SiO2 and Al2O3
The Glass bulb is filled with solution of
HCl & KCl, silver acetate coated with
AgCl is inserted as Electrode.
Glass membrane
Electrode
36.
First glass absorb water
Then H ions can move in the direction of
lesser concentration and replace Na ions and
others in the glass membrane.
SiO2-Na⁺ + H⁺ → SiO- H⁺ + Na⁺
As a result of diffusion and exchange process
a potential develops on each side of glass
membrane
Working
37.
Its potential is not effected by the
presence of strong reducing and
oxidizing agents.
It operates over a wide pH range,
It respond fast and function well in
physiological systems
Used in pH meter.
Applications
39.
Used in acid base titration but very
limited application because many organic
substances directly react with hydrogen
gas.
Hydrogen Electrode
40.
Contain a solution of Quinones and Hydroquinones
prepared from Quinhydrone
2QH → Q+H2Q
Simple and easily attains equilibrium
employed in the presence of mild oxi and red agents
at pH8
Sensitive to high conc of salts and oxi & red agents.
Quinhydrone Electrode
41.
The electrode consists of an inert metal electrode
(usually a platinum wire) in contact with
quinhydrone crystals and a water-based solution.
Quinhydrone is slightly soluble in water, dissolving
to form a mixture of two substances, quinone and
hydroquinone, with the two substances present at
equal concentration. Each one of the two substances
can easily be oxidised or reduced to the other.
The potential at the inert electrode depends on the
ratio of the activity of two substances (quinone-
hydroquinone), and also the hydrogen ion
concentration. The electrode half-reaction is:
Hydroquinone ↔ Quinone + 2H+ +2e-
42.
For practical pH measurement, a second pH independent
reference electrode (such as a silver chloride electrode) is
also used. This reference electrode does not respond to
the pH. The difference between the potential of the two
electrodes depends (primarily) on the activity of H+ in the
solution. It is this potential difference which is measured
and converted to a pH value.
The quinhydrone electrode is not reliable above pH 8. It is
also unreliable in the presence of strong oxidising or
reducing agents, which would disturb the equilibrium
between hydroquinone and quinone. It is also subject to
errors in solutions containing proteins or high
concentrations of salts.
Other electrodes commonly used for measuring pH are
the glass electrode, the hydrogen electrode, the antimony
– antimony oxide electrode, and the ion-sensitive field
effect transistor ISFET electrode.
43.
U shaped tube filled with an inert electrolyte
1. Glass tube bridge (gel+ KI or Na2SO4)
2. Filter tube bridge (filter paper+KCl or NaCl)
Function:
1. Allow electrical contact b/w 2 solutions.
2. Prevent mixing of two solutions.
3. Maintain electrical neutrality.
Salt Bridge
45.
Quantitative measuring procedure in
which a liquid solution is added to a
mixture until some distinctive feature,
signal or end point is observed.
Titration :
46.
It’s a volumetric method in which
potential between two electrodes
(reference & indicator) is measured as a
function of added reagent volume.
Potentiometric Titration
50. Volumetric methods based upon the formation of
slightly soluble precipitate are called " precipitation
titration " .
Because of the precipitating titration based upon
utilizing silver nitrate
(AgNO3) as a precipitating agent, then it called "
argentimetric
processes " .
Precipitation titration is a very important , because it
is a perfect method
for determine halogens and some metal ions
Precipitation Titration
51.
Complex ions ( coordination compounds) are
produce from reaction of
many metal ions (electrons accepter) with electron
pair donors .
The donor species (or called ligands) must have at
least one pair of
unshared electrons for bond formation
Complex formation Titration
52.
Neutralization titrations are performed with
standard solutions of strong acids or
bases. While a single solution (of either acid or base)
is sufficient for the titration of
a given type of analyte, it is convenient to have
standard solutions of both acid and
base available in case back-titration is needed to
locate the end point more exactly.
The concentration of one solution is established by
titration against a primary standard;
the concentration of the other is then determined
from the acid/ base ratio
(that is, the volume of acid needed to neutralize 1.000
mL of the base).
Neutralization Titration
53.
A redox titration is a type of titration based on a
redox reaction between the analyte and titrant.
Redox titration may involve the use of a redox
indicator and/or a potentiometer. Common
examples of a redox titration is treating a
solution of iodine with a reducing agent and
using starch as an indicator. Iodine forms an
intensely blue complex with starch. Iodine (I2)
can be reduced to iodide(I−) by
e.g. thiosulphate (S2O3
2−), and when all iodine is
spent the blue colour disappears. This is called
an iodometric titration
Oxidation-Reduction titration
54.
Analysis of pollutants in water
Drug Analysis in Pharmaceutical industry
Food industry for analysis of quality
Biochemical and biological Assay or analysis
To check the quality of cosmetics
Also used as analytical tool in Textile, paper,
paints, explosive energy and more .
Applications of
Potentiometry