Potentiometry
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![Potentiometry (Chapter 14)
Potentiometry
Ecell w/o current flow info abt. a chemical system
• endpoint in a titration
• Measure [ion]
Rapid; Simple; Inexpensive
Need
Reference electrode
Indicator electrode
Potential measuring device](https://image.slidesharecdn.com/potentiometry-140702115517-phpapp01/85/Potentiometry-1-320.jpg)
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1 Potentiometry
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.
potentiometry
Potentiometry is a method of analysis that determines the concentration of an ion or substance by measuring the potential developed at a sensitive indicator electrode immersed in the solution. There are two main types of indicator electrodes: metallic electrodes where redox reactions occur on the surface, and membrane electrodes where charge exchange occurs across a selective surface. Reference electrodes such as silver/silver chloride are used along with indicator electrodes to complete the circuit and allow measurement of potential. Potentiometry can be used for direct concentration measurements or titration applications such as acid-base, precipitation, complexation, and redox reactions.
Potentiometry ppt
it is about the description of Potentiometry, EMF, Types of Electrodes, Measurement of Electrode potential and applications of Potentiometry.
refernce electrodes
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.
Potentiometry
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 new
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.
2 potentiometry
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
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.
Recommended
1 Potentiometry
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.
potentiometry
Potentiometry is a method of analysis that determines the concentration of an ion or substance by measuring the potential developed at a sensitive indicator electrode immersed in the solution. There are two main types of indicator electrodes: metallic electrodes where redox reactions occur on the surface, and membrane electrodes where charge exchange occurs across a selective surface. Reference electrodes such as silver/silver chloride are used along with indicator electrodes to complete the circuit and allow measurement of potential. Potentiometry can be used for direct concentration measurements or titration applications such as acid-base, precipitation, complexation, and redox reactions.
Potentiometry ppt
it is about the description of Potentiometry, EMF, Types of Electrodes, Measurement of Electrode potential and applications of Potentiometry.
refernce electrodes
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.
Potentiometry
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 new
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.
2 potentiometry
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
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.
Potentiometry titration
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.
Electroanalytical Methods of analysis
The document provides information about electroanalytical methods of analysis. It defines electroanalytical methods as techniques that study analytes by measuring potentials or currents in an electrochemical cell containing the analyte. It discusses various types of electroanalytical techniques including potentiometry, voltammetry, and Karl Fischer titration. It provides details on the principles, instrumentation, applications, and advantages of these analytical methods.
Conductometry titration
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.
Polarography
This document discusses polarography, which is a technique for analyzing solutions using two electrodes - a dropping mercury working electrode and a reference electrode. It provides details on:
1. How polarography works by applying a voltage to induce a redox reaction and measuring the resulting current.
2. The components needed, including the dropping mercury electrode, reference electrode, and a supporting electrolyte.
3. How polarograms are generated by plotting current vs. applied voltage and the different regions that can be seen on a polarogram.
4. Factors that influence the diffusion current measured, such as concentration of the analyte, diffusion coefficient, and drop lifetime. Equations for calculating diffusion current are also presented.
potentiometry
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
Electroanalytical chemistry
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.
INDICATOR ELECTRODE
A helpful and knowledgeable presentation on Indicator electrodes from the subject of Pharmaceutical Analysis (department of B.pharm).
Voltammetry
This document discusses the principles and methods of voltammetry and polarography. Some key points:
- Voltammetry measures the current-potential curve during electrolysis using a small amount of sample. Polarography uses a dropping mercury electrode as the working electrode.
- In polarographic analysis, a polarized working electrode and depolarized reference electrode are used. No stirring is used. Only a small amount of analyte undergoes electrolysis.
- The limiting diffusion current is proportional to analyte concentration and can be used for quantitative analysis. The half-wave potential is used for qualitative analysis.
- Factors like temperature, supporting electrolyte composition, and mercury electrode potential affect the limiting diffusion current.
Conductometry
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.
Potentiometry
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
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This slide contains fragmentation of important functional groups i.e. Alkane and Carbonyl compounds in mass spectrometry.
Coulometry.pptx presentation assignment copy
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.
Polarography
Polarography is an electroanalytical technique invented in 1922 by Jaroslav Heyrovsky for which he won the Nobel Prize. It involves measuring the current in a solution under an applied potential using a dropping mercury electrode and a reference electrode such as SCE. Mercury is used as the working electrode due to its wide negative potential range and ability to regenerate its surface. A polarogram is generated by plotting current versus applied potential, showing residual, diffusion, and limiting currents. Polarography can be used for qualitative and quantitative analysis of metals, drugs, and other compounds.
Basics of Electrochemistry and Electrochemical Measurements
A potentiostat is an electronic instrument that controls the voltage difference between a working electrode and a reference electrode by injecting current through an auxiliary electrode. It is used to apply a potential to an electrochemical cell and measure the resulting current. A potentiostat requires a three-electrode cell with a working electrode, reference electrode, and counter electrode. The working electrode is where the potential is controlled and current is measured. Common reference electrodes include the saturated calomel electrode and silver/silver chloride electrode, which maintain a constant potential. The counter electrode completes the circuit by allowing current to flow out of the cell. Potentiostats are used to study electrochemical reactions and processes.
Potentiometry
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 ppt By Chand.pptx
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Potentiometry
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This document discusses amperometric titration, which is an electrochemical titration method that measures current under a constant applied voltage. It explains the principle that the current passing through an indicator electrode is measured during titration as the concentration of electroreducible ions changes. The document outlines the conditions, apparatus used including dropping mercury and rotating platinum microelectrodes, types of amperometric titrations, advantages such as ability to analyze reducible and non-reducible ions, applications including HPLC detection, and disadvantages like inaccurate results from foreign substances.
Potentiometry
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.
Polarography Principle, instrumentation, Applications.pptx
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.
Potentiometry
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.
potentiometry
This document discusses the principles of potentiometric measurement. Potentiometry involves measuring the potential of an electrochemical cell under conditions of zero current flow, allowing the cell composition to remain unchanged. The potential is related to analyte concentration by the Nernst equation. Potentiometric cells consist of a sensing electrode and a reference electrode separated by a salt bridge. The potential difference between the electrodes corresponds to analyte levels. Common sensing electrodes include ion-selective electrodes and metallic electrodes like silver or copper that respond to specific ions.
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Potentiometry titration
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.
Electroanalytical Methods of analysis
The document provides information about electroanalytical methods of analysis. It defines electroanalytical methods as techniques that study analytes by measuring potentials or currents in an electrochemical cell containing the analyte. It discusses various types of electroanalytical techniques including potentiometry, voltammetry, and Karl Fischer titration. It provides details on the principles, instrumentation, applications, and advantages of these analytical methods.
Conductometry titration
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.
Polarography
This document discusses polarography, which is a technique for analyzing solutions using two electrodes - a dropping mercury working electrode and a reference electrode. It provides details on:
1. How polarography works by applying a voltage to induce a redox reaction and measuring the resulting current.
2. The components needed, including the dropping mercury electrode, reference electrode, and a supporting electrolyte.
3. How polarograms are generated by plotting current vs. applied voltage and the different regions that can be seen on a polarogram.
4. Factors that influence the diffusion current measured, such as concentration of the analyte, diffusion coefficient, and drop lifetime. Equations for calculating diffusion current are also presented.
potentiometry
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
Electroanalytical chemistry
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.
INDICATOR ELECTRODE
A helpful and knowledgeable presentation on Indicator electrodes from the subject of Pharmaceutical Analysis (department of B.pharm).
Voltammetry
This document discusses the principles and methods of voltammetry and polarography. Some key points:
- Voltammetry measures the current-potential curve during electrolysis using a small amount of sample. Polarography uses a dropping mercury electrode as the working electrode.
- In polarographic analysis, a polarized working electrode and depolarized reference electrode are used. No stirring is used. Only a small amount of analyte undergoes electrolysis.
- The limiting diffusion current is proportional to analyte concentration and can be used for quantitative analysis. The half-wave potential is used for qualitative analysis.
- Factors like temperature, supporting electrolyte composition, and mercury electrode potential affect the limiting diffusion current.
Conductometry
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.
Potentiometry
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
Fragmentation of important functional group- Alkane and corbonyl compounds
This slide contains fragmentation of important functional groups i.e. Alkane and Carbonyl compounds in mass spectrometry.
Coulometry.pptx presentation assignment copy
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.
Polarography
Polarography is an electroanalytical technique invented in 1922 by Jaroslav Heyrovsky for which he won the Nobel Prize. It involves measuring the current in a solution under an applied potential using a dropping mercury electrode and a reference electrode such as SCE. Mercury is used as the working electrode due to its wide negative potential range and ability to regenerate its surface. A polarogram is generated by plotting current versus applied potential, showing residual, diffusion, and limiting currents. Polarography can be used for qualitative and quantitative analysis of metals, drugs, and other compounds.
Basics of Electrochemistry and Electrochemical Measurements
A potentiostat is an electronic instrument that controls the voltage difference between a working electrode and a reference electrode by injecting current through an auxiliary electrode. It is used to apply a potential to an electrochemical cell and measure the resulting current. A potentiostat requires a three-electrode cell with a working electrode, reference electrode, and counter electrode. The working electrode is where the potential is controlled and current is measured. Common reference electrodes include the saturated calomel electrode and silver/silver chloride electrode, which maintain a constant potential. The counter electrode completes the circuit by allowing current to flow out of the cell. Potentiostats are used to study electrochemical reactions and processes.
Potentiometry
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.
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This document discusses amperometric titration, which is an electrochemical titration method that measures current under a constant applied voltage. It explains the principle that the current passing through an indicator electrode is measured during titration as the concentration of electroreducible ions changes. The document outlines the conditions, apparatus used including dropping mercury and rotating platinum microelectrodes, types of amperometric titrations, advantages such as ability to analyze reducible and non-reducible ions, applications including HPLC detection, and disadvantages like inaccurate results from foreign substances.
Potentiometry
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.
Polarography Principle, instrumentation, Applications.pptx
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.
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Potentiometry
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.
potentiometry
This document discusses the principles of potentiometric measurement. Potentiometry involves measuring the potential of an electrochemical cell under conditions of zero current flow, allowing the cell composition to remain unchanged. The potential is related to analyte concentration by the Nernst equation. Potentiometric cells consist of a sensing electrode and a reference electrode separated by a salt bridge. The potential difference between the electrodes corresponds to analyte levels. Common sensing electrodes include ion-selective electrodes and metallic electrodes like silver or copper that respond to specific ions.
Potentiometry
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.
Potentiometry
Potentiometry involves measuring the potential of electrochemical cells using ion selective electrodes. It requires a reference electrode with a known constant potential and an indicator electrode that responds to the ion of interest. The potential difference between the electrodes is measured and related to ion concentration or activity. Common types of ion selective electrodes include glass membrane electrodes, crystalline membrane electrodes, and liquid membrane electrodes which incorporate different materials like glasses, crystals, or liquid membranes to selectively bind target ions. Calibration allows the electrode potential measurements to be converted to analytical results.
Analytical class potetiometry conductomtry, P K MANI
This document discusses potentiometric and conductometric titrations. It provides details on reference electrodes like the saturated calomel electrode and silver-silver chloride electrode. It describes indicator electrodes including metallic electrodes of the first and second type that respond directly or indirectly to analyte concentration. Membrane electrodes like glass pH electrodes are also discussed. The principles of potentiometry are explained through diagrams of electrode systems and the Nernst equation. Liquid junction potentials and factors influencing reference electrode potentials are summarized.
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This document provides an overview of electrochemistry techniques used in clinical chemistry, including potentiometry, voltammetry, coulometry, and conductometry. It describes the basic concepts such as electrochemical cells and electrodes. Potentiometry techniques like ion-selective electrodes and their applications in measuring electrolytes are discussed in detail. Other techniques like amperometry and different types of voltammetry and coulometry are also summarized along with their uses and advantages.
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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.
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This document provides an overview of voltammetry and potentiometry techniques. It discusses the history and development of voltammetry, which involves measuring current as a function of applied potential. Common types of voltammetry include linear sweep, cyclic, and stripping voltammetry. The document also describes the basic components of a voltammetry system, including the working, reference, and counter electrodes. Finally, it provides a brief introduction to potentiometry and its applications in titration and measuring concentration, activity, and pH.
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Electrochemical methods are analytical techniques that use measurements of potential, charge, or current to determine an analyte's concentration or characterize its reactivity. There are several types of electrochemical methods including potentiometry, voltammetry, coulometry, conductometry, and dielectrometry. Potentiometry measures the potential of a solution between two electrodes and relates the potential to analyte concentrations. Voltammetry applies a constant or varying potential at an electrode and measures the resulting current. Coulometry completely converts an analyte from one oxidation state to another by applying current or potential and measuring the total current passed. Potentiometric titration uses two electrodes to measure the potential across a solution during a titration rather than using
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Ion selective methods
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Ion specific electrodes
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potentiometry-180713090143.pdf
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.
Lec 3 4-electroanalytical methods part 1
The document discusses various electroanalytical methods, focusing on potentiometry. It describes potentiometry as a static method that involves measuring the potential of electrochemical cells in the absence of current. Key aspects of potentiometry include the reference electrode which maintains a known potential, and indicator electrodes such as ion-selective electrodes that respond to specific ions. Membrane electrodes are also discussed, including their ion selectivity properties and Nernstian response to changes in ion concentration.
Potentiometry, voltamemtry and conductometry
This document discusses various electroanalytical techniques used in clinical laboratories including potentiometry, voltammetry, conductometry, and coulometry. Potentiometry measures electrical potential differences using ion-selective electrodes or redox electrodes. Voltammetry and amperometry are sensitive techniques that apply a voltage to induce an electrochemical reaction and measure the resulting current. Conductometry measures how well ions conduct electricity. Coulometry determines the amount of an electroactive substance by measuring the charge required for its oxidation or reduction reaction. The NOVA-8 analyzer is highlighted as an example that can test for electrolytes, pH, hematocrit, and other clinical analytes using these electroanalytical methods.
electrochemistry.pptx
This document discusses electrochemistry and the Nernst equation. It begins by defining electrochemistry and describing the basic components of an electrochemical cell including electrodes, salt bridge, and cell potential. It then explains the Nernst equation and how it can be used to calculate cell potential based on concentrations. Different types of electrodes are described such as metal-metal ion, gas, redox, and ion selective electrodes. Applications of the Nernst equation include calculating electrode potentials, equilibrium constants, and determining pH. Finally, Frost diagrams are introduced as a graphical way to represent redox potentials and stability.
Dr. Amare ayalew abebe
This document provides an overview of ion selective electrodes (ISEs), including their definition, classification, properties, and applications. ISEs are indicator electrodes that respond selectively to specific ions. They are classified as either membrane or metallic electrodes. Membrane ISEs contain a thin selective membrane and include glass, solid-state, liquid, and molecular electrodes. The document discusses the chemical composition and working principles of common ISEs like glass pH electrodes and fluoride electrodes. It also notes potential applications of ISEs in areas like agriculture, food analysis, industry, and clinical chemistry.
Electrochem - Copy.pptx
To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.To develop a premier world class education centre, for creating global project management professionals, thereby making Larsen & Toubro (L&T) a centre of excellence in project management.
Ver1-Potentiometry (3rd +4th Lects).ppt
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 of fixed potential. Common indicator electrodes are metallic, membrane-based like glass pH electrodes, liquid membrane electrodes, crystalline membrane electrodes, and gas sensing probes. Potentiometric measurements involve calibrating the electrode potential against standards of known analyte activity to determine unknown concentrations via the Nernst equation. Special applications include micro-scale potentiometry for in vivo or real-time measurements.
Instrumental methods ii and basics of electrochemistry
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.
Second lect Potentiometry.ppt
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.
Ch17 z5e electrochem
This document discusses electrochemistry and galvanic cells. It defines oxidation and reduction, and explains how galvanic cells work by using half-reactions and a salt bridge or porous disk to allow ions to flow while preventing the electrons from mixing. It discusses how cell potential is calculated from standard reduction potentials of the half-reactions, and how the direction of electron flow determines the anode and cathode. Standard conditions and notation for describing complete galvanic cells are also covered.
Potentiometery BP 1st year.pptx
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.
Pharmaceutical Analysis Potentiometery BP
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.
Electrodes and Potentiometry.ppt
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.
ppt uit 2 link -final - (1.1.23) - Copy.pptx
Electrochemistry deals with the transformation of chemical energy into electrical energy and vice versa. An electrochemical cell converts this energy and can be classified as either galvanic/voltaic, which converts chemical to electrical, or electrolytic, which converts electrical to chemical. The Nernst equation describes the relationship between cell potential and reaction conditions. Electrodes can be reference electrodes, which have a stable and reproducible potential, or indicator electrodes, which respond to specific ions. Common reference electrodes include calomel and silver-silver chloride, while common indicator electrodes include glass and ion-selective electrodes.
Section 11 potentiometric electrodes and potentiometry
This document summarizes different types of potentiometric electrodes used to measure ion activity. It discusses electrodes of the first kind like silver/silver chloride electrodes and electrodes of the second kind like calomel electrodes. Redox electrodes and the hydrogen electrode are also covered. The document explains how to write the Nernst equation for different half-cells and full electrode systems. It provides examples of liquid junction cells and discusses sources of potential and factors that affect potentiometric measurements.
Chapter - 6 (Electrochemistry).ppt
Electroanalytical methods provide several advantages for quantitative analytical chemistry. They involve measuring the electrical properties of analyte solutions in electrochemical cells. Some key points:
- Electroanalytical methods allow easy automation through electrical signal measurements. They can also determine low analyte concentrations without difficulty.
- Electrochemical processes involve the transfer of electrons between substances during redox reactions. This occurs at the interface between electrodes and solutions in electrochemical cells.
- Advantages include low cost compared to spectroscopy and the ability to easily automate measurements and detect low analyte concentrations through electrical signals.
23sec2
This document discusses half-cells, cell potentials, and how to calculate cell potentials using standard reduction potentials of half-reactions. The key points are:
- Standard reduction potentials allow prediction of spontaneous reactions and equilibria.
- Cell potentials (Ecell) are calculated as the potential of the reduction half-reaction minus the potential of the oxidation half-reaction.
- A positive Ecell indicates a spontaneous reaction with the half-reaction with the larger (least negative) potential proceeding as the reduction.
Soil pH and EC, P K MANI
1) A pH meter works by measuring the potential difference between a glass electrode that responds to hydrogen ion concentration and a reference electrode with a known potential. The glass electrode selectively binds hydrogen ions, generating a potential based on the H+ concentration difference across the membrane.
2) The Nernst equation relates the measured potential to pH. At room temperature, pH equals the measured potential minus the reference electrode potential, divided by 0.05916 volts per pH unit.
3) Combination pH electrodes contain both the glass and reference electrodes in one probe for convenient measurement of the solution's pH based on its hydrogen ion concentration.
Vii.electrochemistry
This document provides an overview of electrochemistry concepts including:
- Basic definitions of oxidation, reduction, and redox reactions
- How galvanic cells generate electricity through spontaneous redox reactions separated into half-cells
- How the standard reduction potential (E°) and Nernst equation can be used to calculate cell potential (Ecell)
- Key aspects of potentiometry including using reference electrodes to measure analyte concentrations based on cell voltage
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Instrumental methods ii and basics of electrochemistry
Instrumental methods ii and basics of electrochemistry
Section 11 potentiometric electrodes and potentiometry
Section 11 potentiometric electrodes and potentiometry
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Astute Business Solutions | Oracle Cloud Partner |
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Potentiometry
- 1. Potentiometry (Chapter 14) Potentiometry Ecell w/o current flow info abt. a chemical system • endpoint in a titration • Measure [ion] Rapid; Simple; Inexpensive Need Reference electrode Indicator electrode Potential measuring device
- 2. Potentiometry Typical Cell Reference electrode / salt bridge / analyte soln / Indicator electrode Eref Ej Eind Reference electrode: Anode by convention Ecell = Ecath - Eanode = Eind - Eref + Ej
- 4. Potentiometry A. Junction Potential (Ej) – Potential that develops across the boundary between 2 electrolyte solns of different composition – Fundamental problem in Potentiometry – Limits accuracy – Small unk. value A junction potential of ~ 3 mV produces an error of ~ 0.05 pH units (12% error in [H+])
- 5. 0.01 M HCL - + 1 M HCl examples Skoog etal
- 6. Caused differences in mobility of the ions
- 7. Potentiometry B. Reference Electrodes Why is the SHE not useful as a reference in potentiometry a. Limited practical use b. Difficult to prepare electrode surfaces c. Difficult to control the activity of H+ d. All of the above Which one of the following is a arbitrary reference electrode for measuring electrode potentials a. Ag/AgCl b. Saturated Calomel Electrode c. Normal Hydrogen electrode d. All of the above
- 8. 1. Ag/AgCl Ag / AgCl, KCl (x M) // AgCls + 1e- Ags + Cl- E0 = 0.222 V Potential determined by [Cl- ] Sat’d, E = 0.197 V Two common Reference Electrodes Ag/AgCl SCE
- 9. 2. calomel electrode Hg / Hg2Cl2 (sat’d), KCl (x M) // Hg2Cl2(s) + 2e- 2Hgl + 2Cl- Potential determined by [Cl- ] Standard conditions: E0 = 0.268 V Sat’d calomel electrode (SCE) E = 0.241 V Why are sat’d solutions used?
- 10. Voltage Conversions Between Different Reference Scales p. 331 SCE to SHE; SHE to SCE SHE to AgCl; AgCl to SHE
- 11. C. Indicator Electrodes Electrode that responds directly to the analyte Ideal: Responds rapidly, reproducibly Selective Two main types 1- metallic 2- membrane
- 12. Potentiometry 1. Metallic Electrodes Example, Pt in a solution of Fe2+ /Fe3+ Potential determined by the Nernst Equation Eind = E0 – 0.0592 log [Fe2+ ]/[Fe3+ ] Ecell = Eind – E AgCl + Ej Not selective
- 13. Potentiometry 2. Membrane Indicator Electrodes – Ion selective electrodes (pIon electrodes) – Respond “selectively” to one species in solution Inside: soln containing the ion of interest, const. A Outside: soln containing the ion of interest, var. A Measure potential difference across the membrane Thin membrane that separates the sample from the inside of the electrode
- 15. pH measurement with a glass electrode Glass combination electrode
- 16. pH electrode Cell schematic Ag l AgCl l Cl- (x M) ll H+ (outside) l H+ (inside), Cl- (x M) l AgCl l Ag Cations (Na+ ) bind oxygen in SiO4 structure
- 17. pH Electrode Membrane must be hydrated
- 18. Functions by exchange of ions at the surface H+ Gls = H+ aq + Gl- s Glass 1 Soln 1 H+ Gls = H+ aq + Gl- s Glass 2 Soln 2 Eb = E1 – E2 = 0.05916 log Ain / Aout Eb = L – 0.0592pH Position of these two equil. are determined by aH+ in soln on the two sides of the membrane
- 19. Glass Electrode Potential Three components 1- boundary potential 2- potential of internal Ag/AgCl reference electrode 3- small asymmetry potential Eind = Eb + Eref2 + Easy Eind = L’ + 0.0592 Log A1 + Eref2 + Easy Eind = K + 0.0592 Log [H+] Eind = K + β0.0592 Log [H+] Electromotive efficiency
- 20. Activity becomes important when a. Ions have divalent or trivalent charges b. Ionic strength of the solution is high c. All of the above d. None of the above Activity vs Concentration
- 21. Calibrating a glass electrode Eind = K + 0.0592 Log [H+] For every 10 fold change in activity, the potential should change by 59.2 mV Slope = ?
- 22. Potentiometry Errors (limitations) in pH measurements 1- must calibrate electrode 2- junction potential and drift 3- alkaline (sodium) error 4- acid error 5- allow membrane to equilibrate 6- membrane must be hydrated 7- Temperature
- 23. Other examples of ISE Eind = K + (0.0592 / 2)Log [Ca2+ ] Liquid-based ISE
- 24. E = K – 0.0592 Log [F-] Slope = ? Solid State ISE Linear range = ?
- 26. Potentiometry Equation written from the point of view that the membrane electrode responds to only one ion, maybe more Full expression E = const. + 2.303RT / zF log (Ai + Ki,jAj zi/zj ) K ranges from 0 to values greater than 1 Selectivity coefficient KA,X = response of X / response of A The smaller, the less interference by X
- 27. Potentiometry Monovalent cations (assume k= 0) E = const + 0.0592 log Ax+ Monovalent anions (assume k = 0) E = const – 0.0592 log Aa-
- 28. Constant made up of several constants Determine experimentally 1- meas. Ecell for std sol of known conc. 2- meas Ecell for unknown conc. make assumption that K is unchanged
- 29. Advantages (Figures of Merit) and other characteristics a.Linear response over a wide range b.Non destructive c.Non contaminating d.Short response time (min) e.Unaffected by color and turbidity f.Precision: OK (1% at best) g.Sensitivity/Detection limits: (10-6 to 10-9*** M) h.Standard addition method often used (Why ?)
- 30. Problems: Questions to ask: Membrane or Metal ISE?? If membrane, Ecell = Emem – Eref Ememb = const +/− 0.0592 log a If metal, Ecell = Ecathode – Eref Ecathode Nernst Eq
- 31. Calculate the potential of the following cell when the aqueous solution is 7.40 x 10-3 M Hg2+ SCE // aq soln / Hg SCE is the saturated Calomel electrode, E0’ = 0.244 V
- 32. Example A pH glass/calomel electrode was found to develop a potential of –0.0412 V when used with a buffer of pH 6.00. With an unk soln, the potential was –0.2004 V. Calculate the pH of the solution.