Electrochemistry deals with oxidation-reduction reactions where chemical energy is converted to electrical energy and vice versa. It involves the transfer of electrons between oxidizing and reducing agents. An electrochemical cell allows a redox reaction to occur by transferring electrons through an external connector. The potential difference between the anode and cathode is called the electromotive force (emf). Various electroanalytical techniques like potentiometry, voltammetry, conductometry, and coulometry are used for clinical applications such as measuring blood gases, electrolytes, and analytes. Optical chemical sensors called optodes are also used as they offer advantages over traditional electrodes.
Potentiometry, voltamemtry and conductometryapeksha40
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.
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.
This document provides an overview of the key concepts in electrochemistry including oxidation-reduction reactions, galvanic cells, standard reduction potentials, the Nernst equation, electrolysis, batteries, corrosion, and commercial electrolytic processes. It defines important terms, describes experimental set ups and calculations for electrochemical cells, and summarizes fundamental electrochemical principles and laws such as Faraday's laws of electrolysis.
Electrochemistry deals with chemical reactions caused by electric currents or electric currents produced by chemical reactions. Galvanic cells convert chemical energy to electrical energy through redox reactions. Reversible cells like Daniel cells can undergo reactions in both directions while irreversible cells like zinc-silver cells cannot. Protective metal coatings through electroplating or electroless plating prevent corrosion by depositing a noble metal layer on a substrate.
This document provides a summary of a presentation on conductometry. It discusses electrochemical cells, types of electrodes including reference and indicator electrodes. It also describes the Nernst equation and its applications in determining solubility products and for analytical chemistry purposes such as measuring ion concentrations using cell potentials. Electrode types including electrodes of the first, second and third kind are explained along with examples like the silver/silver chloride electrode.
Potentiometry is an electroanalytical technique that uses potentiometers to measure electrochemical potential. It involves using reference and indicator electrodes immersed in analyte solutions. The potential difference between the electrodes depends on ion activity/concentration based on the Nernst equation, allowing for quantitative analysis. A salt bridge containing a neutral salt maintains electrical neutrality between electrode half-cells. Common reference electrodes include silver/silver chloride and saturated calomel electrodes. Potentiometry is used for pH measurements and potentiometric titrations.
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.
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.
Potentiometry, voltamemtry and conductometryapeksha40
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.
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.
This document provides an overview of the key concepts in electrochemistry including oxidation-reduction reactions, galvanic cells, standard reduction potentials, the Nernst equation, electrolysis, batteries, corrosion, and commercial electrolytic processes. It defines important terms, describes experimental set ups and calculations for electrochemical cells, and summarizes fundamental electrochemical principles and laws such as Faraday's laws of electrolysis.
Electrochemistry deals with chemical reactions caused by electric currents or electric currents produced by chemical reactions. Galvanic cells convert chemical energy to electrical energy through redox reactions. Reversible cells like Daniel cells can undergo reactions in both directions while irreversible cells like zinc-silver cells cannot. Protective metal coatings through electroplating or electroless plating prevent corrosion by depositing a noble metal layer on a substrate.
This document provides a summary of a presentation on conductometry. It discusses electrochemical cells, types of electrodes including reference and indicator electrodes. It also describes the Nernst equation and its applications in determining solubility products and for analytical chemistry purposes such as measuring ion concentrations using cell potentials. Electrode types including electrodes of the first, second and third kind are explained along with examples like the silver/silver chloride electrode.
Potentiometry is an electroanalytical technique that uses potentiometers to measure electrochemical potential. It involves using reference and indicator electrodes immersed in analyte solutions. The potential difference between the electrodes depends on ion activity/concentration based on the Nernst equation, allowing for quantitative analysis. A salt bridge containing a neutral salt maintains electrical neutrality between electrode half-cells. Common reference electrodes include silver/silver chloride and saturated calomel electrodes. Potentiometry is used for pH measurements and potentiometric titrations.
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.
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.
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.
potentiometry and ion selective electrodesAnimikh Ray
This document discusses potentiometry and ion selective electrodes. It provides information on:
- Potentiometry measures the potential of an electrochemical cell under static conditions without drawing current. This allows the cell composition to remain unchanged.
- Ion selective electrodes are used to measure specific ion concentrations in solution based on the potential difference between an indicator electrode immersed in the solution and a reference electrode.
- Common clinical applications of potentiometry and ion selective electrodes include measuring electrolyte levels like sodium, potassium, calcium and pH in samples like blood and urine to evaluate conditions like hypo- or hypernatremia.
potentiometry and ion selective electrodeAnimikh Ray
This document discusses potentiometry and ion selective electrodes. It provides information on:
- Potentiometry measures the potential of an electrochemical cell under static conditions without drawing current. This allows the cell composition to remain unchanged.
- Ion selective electrodes are used to measure specific ion concentrations in solution based on the potential difference between an indicator electrode immersed in the solution and a reference electrode.
- Common applications of potentiometry and ion selective electrodes include measuring electrolyte levels like sodium, potassium, calcium, and pH in clinical samples and environmental samples. This provides useful quantitative analysis in various fields like healthcare, agriculture, and food processing.
Class XII Electrochemistry - Nernst equation.Arunesh Gupta
This document provides an overview of electrochemistry and some key concepts. It begins by defining electrochemistry as the study of how spontaneous chemical reactions can produce electricity and how electrical energy can drive non-spontaneous reactions. It then discusses several applications of electrochemistry including metal production, electroplating, and batteries. The document goes on to define conductors and the differences between metallic and electrolytic conduction. It also introduces concepts like galvanic cells, salt bridges, standard electrode potentials, and the electrochemical series. In summary, the document provides a broad introduction to fundamental electrochemistry topics and concepts.
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.
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.
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.
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.
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.
ppt uit 2 link -final - (1.1.23) - Copy.pptxKundanBhatkar
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.
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.
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 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.
Module 2_S7 and S8_Electrochemical Cells.pptxAdittyaSenGupta
An electrochemical cell consists of two electrodes separated by an electrolyte. There are two types: galvanic cells and electrolytic cells. A galvanic cell converts the chemical energy of a spontaneous redox reaction directly into electrical energy. The Nernst equation relates the cell potential (E) of a galvanic cell to the standard potential (E0), temperature, and reaction quotient through the concentrations of reactants and products. It allows calculation of cell potential under non-standard conditions.
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 provides an overview of electrochemistry. It begins by defining electrochemistry as the study of chemical reactions at the interface of an electrode and electrolyte involving the interaction of electrical and chemical changes. The document then discusses the history and founders of electrochemistry, including Faraday's two laws of electrolysis. It explains key concepts such as oxidation-reduction reactions, balancing redox equations, and the Nernst equation. The document also covers applications including batteries, corrosion, electrolysis, and branches of electrochemistry like bioelectrochemistry and nanoelectrochemistry.
This document discusses various topics in electrochemistry including redox reactions, balancing redox equations, galvanic cells, standard reduction potentials, and applications such as corrosion and electrolysis. It defines key terms like oxidation, reduction, and half-reactions. Methods for balancing redox equations under acidic and basic conditions are explained. Components of galvanic cells like anodes, cathodes, and salt bridges are defined. Standard reduction potentials are used to determine cell potentials. Examples of galvanic cells and their notations are provided. Corrosion prevention methods and commercial electrolysis processes are briefly described.
The document provides information about electrochemistry. It discusses oxidation-reduction reactions and how they involve the transfer of electrons between species. It explains how to assign oxidation numbers to keep track of electrons gained and lost. Balancing oxidation-reduction reactions using the half-reaction method is also covered. Finally, the document discusses voltaic cells, electrolytic cells, and applications of electrochemistry such as electroplating.
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.
role of physician AT MEDICAL COLLEGE AND SOCIETY.pptxRAJNKIT
This document discusses the roles and responsibilities of physicians. It outlines that physicians should uphold professional qualities like compassion, ethics, and lifelong learning. Their key roles are to treat patients, participate in public health programs, educate communities, and ensure affordable healthcare. Physicians must continually learn and adapt to evolving standards and treatments to provide the best possible care.
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.
potentiometry and ion selective electrodesAnimikh Ray
This document discusses potentiometry and ion selective electrodes. It provides information on:
- Potentiometry measures the potential of an electrochemical cell under static conditions without drawing current. This allows the cell composition to remain unchanged.
- Ion selective electrodes are used to measure specific ion concentrations in solution based on the potential difference between an indicator electrode immersed in the solution and a reference electrode.
- Common clinical applications of potentiometry and ion selective electrodes include measuring electrolyte levels like sodium, potassium, calcium and pH in samples like blood and urine to evaluate conditions like hypo- or hypernatremia.
potentiometry and ion selective electrodeAnimikh Ray
This document discusses potentiometry and ion selective electrodes. It provides information on:
- Potentiometry measures the potential of an electrochemical cell under static conditions without drawing current. This allows the cell composition to remain unchanged.
- Ion selective electrodes are used to measure specific ion concentrations in solution based on the potential difference between an indicator electrode immersed in the solution and a reference electrode.
- Common applications of potentiometry and ion selective electrodes include measuring electrolyte levels like sodium, potassium, calcium, and pH in clinical samples and environmental samples. This provides useful quantitative analysis in various fields like healthcare, agriculture, and food processing.
Class XII Electrochemistry - Nernst equation.Arunesh Gupta
This document provides an overview of electrochemistry and some key concepts. It begins by defining electrochemistry as the study of how spontaneous chemical reactions can produce electricity and how electrical energy can drive non-spontaneous reactions. It then discusses several applications of electrochemistry including metal production, electroplating, and batteries. The document goes on to define conductors and the differences between metallic and electrolytic conduction. It also introduces concepts like galvanic cells, salt bridges, standard electrode potentials, and the electrochemical series. In summary, the document provides a broad introduction to fundamental electrochemistry topics and concepts.
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.
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.
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.
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.
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.
ppt uit 2 link -final - (1.1.23) - Copy.pptxKundanBhatkar
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.
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.
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 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.
Module 2_S7 and S8_Electrochemical Cells.pptxAdittyaSenGupta
An electrochemical cell consists of two electrodes separated by an electrolyte. There are two types: galvanic cells and electrolytic cells. A galvanic cell converts the chemical energy of a spontaneous redox reaction directly into electrical energy. The Nernst equation relates the cell potential (E) of a galvanic cell to the standard potential (E0), temperature, and reaction quotient through the concentrations of reactants and products. It allows calculation of cell potential under non-standard conditions.
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 provides an overview of electrochemistry. It begins by defining electrochemistry as the study of chemical reactions at the interface of an electrode and electrolyte involving the interaction of electrical and chemical changes. The document then discusses the history and founders of electrochemistry, including Faraday's two laws of electrolysis. It explains key concepts such as oxidation-reduction reactions, balancing redox equations, and the Nernst equation. The document also covers applications including batteries, corrosion, electrolysis, and branches of electrochemistry like bioelectrochemistry and nanoelectrochemistry.
This document discusses various topics in electrochemistry including redox reactions, balancing redox equations, galvanic cells, standard reduction potentials, and applications such as corrosion and electrolysis. It defines key terms like oxidation, reduction, and half-reactions. Methods for balancing redox equations under acidic and basic conditions are explained. Components of galvanic cells like anodes, cathodes, and salt bridges are defined. Standard reduction potentials are used to determine cell potentials. Examples of galvanic cells and their notations are provided. Corrosion prevention methods and commercial electrolysis processes are briefly described.
The document provides information about electrochemistry. It discusses oxidation-reduction reactions and how they involve the transfer of electrons between species. It explains how to assign oxidation numbers to keep track of electrons gained and lost. Balancing oxidation-reduction reactions using the half-reaction method is also covered. Finally, the document discusses voltaic cells, electrolytic cells, and applications of electrochemistry such as electroplating.
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.
role of physician AT MEDICAL COLLEGE AND SOCIETY.pptxRAJNKIT
This document discusses the roles and responsibilities of physicians. It outlines that physicians should uphold professional qualities like compassion, ethics, and lifelong learning. Their key roles are to treat patients, participate in public health programs, educate communities, and ensure affordable healthcare. Physicians must continually learn and adapt to evolving standards and treatments to provide the best possible care.
RENAL FUNCTION TESTS FOR PARAMEDICAL AND MEDICAL STUDENTSRAJNKIT
This document discusses renal function tests (RFTs). It begins by describing the functions of the kidney including formation of urine, excretion of waste products, and regulation of water and electrolytes. It then outlines the purposes of RFTs which are to assess renal damage, monitor disease progression, and adjust medication doses. RFTs measure glomerular function through tests of renal clearance and blood analytes like creatinine and urea. They also study tubular function using urine concentration, dilution, and other specialized tests. Common RFTs and their clinical significance are described in detail.
The document discusses liver function tests and their use in evaluating liver health and disease. It covers the metabolic, excretory, synthetic, detoxification and storage functions of the liver. Liver function tests are classified based on the liver's excretory, detoxification, and synthetic functions. Enzymes like ALT, AST, GGT, ALP, and bilirubin are discussed in the context of diagnosing different types of liver disease and jaundice. The document also discusses pancreatic function tests and enzymes like amylase and lipase that are indicators of pancreatic health and diseases like pancreatitis.
The document discusses the chemistry, digestion, and absorption of proteins and amino acids. It covers the structure and properties of proteins and the 20 standard amino acids. Key points include:
- Proteins are polymers of amino acids linked by peptide bonds. They serve structural, enzymatic, transport, storage, and other functions in the body.
- Amino acids vary in their side chains, determining properties like charge, solubility, and metabolism. They are classified by properties like polarity, acid/base characteristics, and essential/non-essential status.
- Protein structure is determined by amino acid sequence and interactions between R groups. Secondary structures like alpha helices influence 3D shape.
Iron is an essential trace element required for oxygen transport and many enzymatic processes. Women and children have higher iron requirements. Dietary sources like jaggery are rich in iron while milk is poor. Factors like calcium, phytates and oxalates inhibit iron absorption in the duodenum and jejunum, while vitamin C and cysteine enhance absorption. Iron is important for carrying oxygen via hemoglobin, acting as an enzyme cofactor, and supporting brain and cell functions. Iron deficiency anemia results from low intake or increased losses and is characterized by low hemoglobin and red blood cell changes. It is commonly seen in pregnant women and treated with oral or parenteral iron supplements.
This document discusses the estimation of serum amylase levels. It describes amylase as the main enzyme for carbohydrate digestion produced by the salivary glands and pancreas. It then outlines two main methods for estimating serum amylase - the iodometric method and saccharogenic method. The iodometric method measures the decrease in color intensity of a starch-iodine solution after hydrolysis by serum amylase. Normal serum amylase levels are 25-125 U/L, and increased levels can indicate conditions like acute pancreatitis while decreased levels may be seen in necrotic pancreatitis or hepatitis.
Automation in clinical chemistry involves using laboratory instruments and equipment to perform clinical assays with minimal technologist involvement. Automation replaces human effort with mechanical devices regulated by feedback to be self-monitoring. The IUPAC defines automation as the replacement of human manipulation with instrumental devices regulated by feedback for self-adjustment. Colorimetry uses Beer's Law and Lambert's Law, where the amount of light transmitted through colored solutions decreases exponentially with increasing concentration or thickness according to the laws.
Optical techniques like photometry, spectrophotometry, and colorimetry are used in clinical laboratories. They are based on Beer's law and Lambert's law. Spectrophotometry measures light intensity at selected wavelengths using a light source, monochromator, sample cuvettes, detector, and display. It provides more sensitivity than colorimetry which determines color intensity based on light absorption. Both techniques rely on the principle that absorbed light is inversely proportional to concentration according to Beer-Lambert's law.
This document discusses bioenergetics and the role of ATP in living systems. It explains that ATP stores and transports chemical energy within cells, which is released through its hydrolysis into ADP and phosphate. The hydrolysis of ATP is highly exergonic, with a large negative standard free energy change of -30.5 kJ/mol. This energy from ATP hydrolysis drives endergonic biochemical reactions and processes, such as the synthesis of glucose-6-phosphate from glucose and phosphate. The energy from ATP hydrolysis is efficiently coupled to these endergonic reactions through a cyclic process of ATP synthesis and breakdown.
This document discusses radioactivity and atomic structure. It begins by explaining the need to study radioactivity for diagnosis, therapy, and medical research. It then defines atoms and their structure, including atomic number and mass number. The document discusses isotopes and radioactive decay, including different types of decay and half-life. It also covers radiation properties, detection and measurement of radioactivity, and radiation safety quantities and units.
Travel Clinic Cardiff: Health Advice for International TravelersNX Healthcare
Travel Clinic Cardiff offers comprehensive travel health services, including vaccinations, travel advice, and preventive care for international travelers. Our expert team ensures you are well-prepared and protected for your journey, providing personalized consultations tailored to your destination. Conveniently located in Cardiff, we help you travel with confidence and peace of mind. Visit us: www.nxhealthcare.co.uk
Histololgy of Female Reproductive System.pptxAyeshaZaid1
Dive into an in-depth exploration of the histological structure of female reproductive system with this comprehensive lecture. Presented by Dr. Ayesha Irfan, Assistant Professor of Anatomy, this presentation covers the Gross anatomy and functional histology of the female reproductive organs. Ideal for students, educators, and anyone interested in medical science, this lecture provides clear explanations, detailed diagrams, and valuable insights into female reproductive system. Enhance your knowledge and understanding of this essential aspect of human biology.
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Kosmoderma Academy, a leading institution in the field of dermatology and aesthetics, offers comprehensive courses in cosmetology and trichology. Our specialized courses on PRP (Hair), DR+Growth Factor, GFC, and Qr678 are designed to equip practitioners with advanced skills and knowledge to excel in hair restoration and growth treatments.
The skin is the largest organ and its health plays a vital role among the other sense organs. The skin concerns like acne breakout, psoriasis, or anything similar along the lines, finding a qualified and experienced dermatologist becomes paramount.
5-hydroxytryptamine or 5-HT or Serotonin is a neurotransmitter that serves a range of roles in the human body. It is sometimes referred to as the happy chemical since it promotes overall well-being and happiness.
It is mostly found in the brain, intestines, and blood platelets.
5-HT is utilised to transport messages between nerve cells, is known to be involved in smooth muscle contraction, and adds to overall well-being and pleasure, among other benefits. 5-HT regulates the body's sleep-wake cycles and internal clock by acting as a precursor to melatonin.
It is hypothesised to regulate hunger, emotions, motor, cognitive, and autonomic processes.
Mercurius is named after the roman god mercurius, the god of trade and science. The planet mercurius is named after the same god. Mercurius is sometimes called hydrargyrum, means ‘watery silver’. Its shine and colour are very similar to silver, but mercury is a fluid at room temperatures. The name quick silver is a translation of hydrargyrum, where the word quick describes its tendency to scatter away in all directions.
The droplets have a tendency to conglomerate to one big mass, but on being shaken they fall apart into countless little droplets again. It is used to ignite explosives, like mercury fulminate, the explosive character is one of its general themes.
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2. ELECTROCHEMISTRY
It is a speciality of classical physics
&chemistry which deals with oxidation &
reduction reactions with transfer of
chemical energy into electrical energy &
vice versa
3. BASIC TERMS
OXIDATION—loss of electron(s) by a species;
increase in oxidation number; increase in
oxygen.
REDUCTION—gain of electron(s); decrease in
oxidation number; decrease in oxygen;
increase in hydrogen.
OXIDIZING AGENT—electron acceptor;
species is reduced.
REDUCING AGENT—electron donor; species
is oxidized.
4. Electrochemical Cells
An apparatus that allows a
redox reaction to occur by
transferring electrons through
an external connector.
Product favored reaction --->
voltaic or galvanic cell ---->
electric current
Reactant favored reaction ---
> electrolytic cell ---> electric
current used to cause
chemical change.
Batteries are voltaic cells
6. •Electrons travel thru external wire.
Salt bridge allows anions and cations to
move between electrode compartments.
Zn --> Zn2+ + 2e- Cu2+ + 2e- --> Cu
<--Anions
Cations-->
Oxidation
Anode
Negative
Reduction
Cathode
Positive
RED CAT
7. Electromotive Force (emf)
The potential difference between the
anode and cathode in a cell is called the
electromotive force (emf).
It is also called the cell potential, and is
designated Ecell.
8. Zn/Cu Electrochemical Cell
Zn(s) ---> Zn2+(aq) + 2e- Eo = +0.76 V
Cu2+(aq) + 2e- ---> Cu(s) Eo = +0.34 V
---------------------------------------------------------------
Cu2+(aq) + Zn(s) ---> Zn2+(aq) + Cu(s)
Eo = +1.10 V
Cathode,
positive,
sink for
electrons
Anode,
negative,
source of
electrons
+
9. H2 input
1.00 atm
inert
metal
We need a standard electrode to
make measurements against!
The Standard Hydrogen Electrode (SHE)
Pt
1.00 M H+
25oC
1.00 M H+
1.00 atm H2
Half-cell
2H+ + 2e- H2
Eo
SHE = 0.0 volts
10. H2 1.00 atm
Pt
1.0 M H+
Cu
1.0 M CuSO4
0.34 v
cathode half-cell
Cu+2 + 2e- Cu
anode half-cell
H2 2H+ + 2e-
KCl in agar
+
Now let’s combine the copper half-cell with the SHE
Eo = + 0.34 v
11. H2 1.00 atm
Pt
1.0 M H+
1.0 M ZnSO4
0.76 v
cathode half-cell
2H+ + 2e- H2
anode half-cell
Zn Zn+2 + 2e-
KCl in agar
Zn
-
Now let’s combine the zinc half-cell with the SHE
Eo = - 0.76 v
12. Assigning the Eo
Al+3 + 3e- Al Eo = - 1.66 v
Zn+2 + 2e- Zn Eo = - 0.76 v
2H+ + 2e- H2 Eo = 0.00 v
Cu+2 + 2e- Cu Eo = + 0.34
Ag+ + e- Ag Eo = + 0.80 v
Write a reduction half-cell, assign the voltage
measured, and the sign of the electrode to the
voltage.
Increasing
activity
13. TABLE OF STANDARD
REDUCTION POTENTIALS
2
Eo (V)
Cu2+ + 2e- Cu +0.34
2 H+ + 2e- H 0.00
Zn2+ + 2e- Zn -0.76
oxidizing
ability of ion
reducing ability
of element
To determine an oxidation from a
reduction table, just take the opposite
sign of the reduction!
14.
15. +
-
battery
Na (l)
electrode half-
cell
electrode half-
cell
Molten NaCl
Na+
Cl-
Cl- Na+
Na+
Na+ + e- Na 2Cl- Cl2 + 2e-
Cl2 (g) escapes
Observe the reactions at the electrodes
NaCl (l)
(-)
Cl-
(+)
23. POTENTIOMETRY
Measurement of an electrical potential
difference between two half cells in an
electrochemical cell when the cell
current is zero .
Galvanic cell
Left side – reference electrode
Right side – Indicator (measuring )
electrode
24. Characteristics of Ideal Reference Electrode:
1) Reversible and follow Nernst equation
2) Potential should be constant with time
3) Should return to original potential after being subjected to
small currents
4) Little hysteresis with temperature cycling
5) Should behave as ideal nonpolarized electrode
25. CELL POTENTIAL – Sum of all potential
gradients existing between different phases
of cell
VARIOUS POTENTIAL GRADIENTS
Redox potential
Membrane potentials
Diffusion potentials
26.
27. ELECTRODES FOR
POTENTIOMMETRIC
APPLICATIONS
REDOX ELECTRODES
Inert metal electrodes
Metal electrodes participating in redox
reaction
ION SELECTIVE ELECTRODES
Glass electrode
polymer membrane electrode
Pco2 electrodes
28. REDOX ELECTRODES
Redox potential – result of chemical equilibrium
involving electron transfer reactions
Oxidised form + ne ↔ Reduced form
redox couple
with respect to SHE
NERNST EQUATION –
E = E0 – N/n x log ared /aox = Eo- .0592v/n xlog ared/ao
N= RT xIn Log 10 /F
29. INERT METAL ELECTRODES
PLATINUM ELECTRODES
GOLD ELECTRODES
HYDROGEN ELECTRODES – pH
measurement
Platinum & gold electrodes r coated with
highly porous platinum( platinum black ) to
catalyze the reaction
ELECTRODE POTENTIAL –
E = E0 – N x log ( f H2)1/2 / aH
34. ION SELECTIVE ELECTRODES
MEMBRANE POTENTIAL
Caused by the permeability of certain types of
membranes to selected anions and cations
Interact with a single ion species
Potential is propotional to the logarithm of the
ionic activity or concentration of the ion
TYPES
GLASS ELECTRODE
POLYMER MEMBRANE ELECTRODE
35. GLASS ELECTRODE
Formulated from
Melts of silicon and aluminium oxide mixed with oxides
of earth or alkali metal cations
- By varying composition , electrodes with selectivity
of various cations can be demonstrated
- Formula for H+ selective glass
72% SiO2, 22% Na2O, 6% CaO
SELECTIVITY ORDER
H+ >>> Na+ > K+ Ph range 7.0 – 8.0
if 71% SiO2, 11% Na2O, 18% Al2O3
H+ >Na+> K+
39. POLYMER MEMBRANE ELECTRODE
WORKING MECHANISM – 3 CATEGORIES
a) CHARGE DISSOCIATED ION EXCHANG
It employs quarternary ammonium(NH4+) salts as
membrane component
Uses
Determinatin of chloride ion in blood & serum
LIMITATIONS –
Anions more lipophilic than chloride in sample may
interfere
Loss of chloride sensitivity with repeated heparin
exposure
40. b) CHARGED ASSOCIATED CARRIER –
Used for Ca+ ion – based on Ca+ selective ion
exchange property of 2-ETHYLHEXYL
PHOSPHORIC ACID dissolved in DIOCTYL
PHENYL PHOSPHONATE .
Reffered as LIQUID MEMBRANE ISE
LATER ON INGREDIENTS WERE INCORPORATED
INTO PVC MEMBRANE
FORMULATION OF PVC MEMBRANE
1 To 3% ionophore - ex TRIFLUROACETONE Gp
64% plasticizer – controls polarity of membrane
30 wt % PVC
< 1wt% additives – ex large lipophilic anions like
TETRAPHENYL BORATE derivatives for cation
selective ISE
41. NEUTRAL ION CARRIER (
IONOPHORE)
INCORPORATION OF NEUTRAL
ANTIBIOTIC VALINOMYCIN – highly
selective for K+ ions
INCORPORATION OF
TRIFLOROACETOPHENONE GROUPS –
Highly selective for carbonate ion
Forms negatively charged adducts
Used for determining total CO2 in
serum/plasma
42. ADVANTAGES OF ISE
Simple
Rapid
Nondestructive
Applicable to a wide range of concentratio
DISADVANTAGES
Interference with other ions
45. VOLTAMMETRY & AMPEROMETRY
VOLTAMETRY – Measurement of current
when an external potential is applied while the
potential varies under potentiostatic control.
Based on the principle of electrolytic cell
Current is directly propotional to the
concentration of the analyte
AMPEROMETRY – Measurement of
current when a constant external
potential is applied
Current is inversely proportional to the
resistance of the the electrolyte
52. ANODIC STRIPPINB VOLTAMMETRY
Used for detecting trace level of toxic
substance in clinical sample
- Carbon working electrode is used
- E app first kept highly negative
- Then scanned more positive
- Reduced metals reoxidize
- Give large anodic current proportional to
ion conc.
- Potential at which peak obs.indicate which
metal is present
53. RAPID SSAN CYCLIC VOLTAMMETRIC
TECHNIQUE
Quantify dopamine in brain tissue in freely
moving animals
Oxidation of dopamine to a quinone sp.at
an implanted microcarbon electrode yields
peak cuffents prop. To concentration of
dopamine levels
54. CONDUCTOMETRY
Measure of ability of ions in solution to carry
current under the influence of potential
diiference
Potential with frequency between 100 to 3000 hZ
IS USED ( PREVENTS ELECTRODE
POLARISATION)
Current is directly propotional to solution
conductance, where conductance is inverse of
resistance
UNIT – SIEMENS ( Ohm-1 )
Depends on-
ionic charge
viscosity
potential applied
55. CLINICAL APPLICATIONS
- Measurement of volume fraction of
erythrocytes
- Electronic counting of blood cells in
suspension ( COULTER PRINCIPLE )
-Titrations ( acid-base , precipitations )
-Tranducer mechanism for some biosensors
56. COULOMETRY
Measures the electrical charge between two
electrodes in a electrochemical cell
Charge is directly proportional to oxidation or
reduction of the substance at one of the electrode
Q =nNF
Q = Charge
n = no of electrons
N = Amount of substance reduced or oxidized
F = Faradays constant (96,487 coulambs/mole)
CLINICAL APPLICATIONS
Cl- ions in serum
Coulometric titrations
Mode of transduction in biosensors
57. OPTICAL CHEMICAL SENSORS
OPTODES
USE – In analytical instruments to measure blood
gases and electrolytes
ADVANTAGES OVER ELECTRODES
- Ease of miniaturization
- Less noise
- Potential long term stability
- No need for reference electrode
BASIC CONCEPT
Optodes used for PO2 Measurement based on
immobilisation of organic dyes ( pyrene
phenantherene, fluoranthrene)
58. METAL LIGAND COMPLEX ( Ruthenium [11]
tris [di pyridine],Pt & Pb metalloporphyrins)
in hydrophobic polymer films ( silicon rubber)
in which O2 is soluble
Decreased intensity of fluorescence is
proportional to PO2
APPLICATIONS
- Used for pCO2 determination
- Optically sense the electrolyte ions eg.
lipophilic ionophore for polymer memb.ISE with
lipophilic Ph indicator ( valinomycin for k+)
change in optical absorption or flourescence
spectrum of polymer layer
59.
60.
61.
62.
63.
64.
65.
66.
67. TECHQNIQUES OF IMMOBILISATION
ENTRAPMENT METHOD
CROSS LINKING OF ENZYME WITH AN
INERT PROTEIN ex- bovine serum albumin
SIMPLE ADSORPTION OF THE ENZYME
TO ELECTRODE SURFACE
COVALENT BINDING OF ENZYME TO
INSOLUBLE CARRIER ex- nylon or glass
BULK MODIFICATION OF ELECTRODE
MATERIAL, mixing enzyme with carbon
paste.which serves as enzyme immobilisation
matrix & electroactive surface
68.
69.
70.
71. ENZYME BASED BIOSENSORS WITH
POTENTIOMETRIC METHOD
UREA ------- 2NH3 + CO2
Urease
LIMITATIONS
High substrate concentration
Local alkaline pH due to hydrolysis of urea
IT IS REDUCED BY
Placing a semipermeable membrane between
enzyme and sample to limit diffusion of urea
72.
73. ENZYME BASED BIOSENSORS WITH
OPTICAL DETECTION
EXAMPLE-
Optical detection for pH & oxygen
Glucose & cholesterol optical sensor
BASED ON
Flourescence
Absorbance
Reflectance
as mode of detectio
74. AFFINITY BASED BIOSENSORS
Immobilised biological recognition element is
a binding protien ,antibody ,(immunosensor)
or oligonucleotide ( eg DNA , aptamers etc
)with high binding specificity & affinity
towards a clinically imp analyte.
Typically single use devices
BASED ON
Electrochemical, optical, thermal,mass,
acoustic detection methods
75. EXAMPLE
ALPHA FETOPROTIEN detected via a quartz
crystal microbalance type mass detector ,
possesing immobilized antialpha-fetoprotien
antibodies
DNA SENSORS – A complementry DNA segment
to the target DNA is immobilized on a suitable
transducer eg.
Genosensor for detecting V Leiden mutations
using capture probeswith inosine substituted
for guanosine nucleic acid
76. ELECTROCHEMICAL O2 SNSORS- carry
out heterogenous enzyme immunoassay
using catalase as labeling enzyme &
immobilizing capture antibodies on the
outer surface of gas permeable membrane.
H2O2 ------ 2H+ + O2
77.
78.
79.
80.
81. IN VIVO & MINIMALY INVASIVE
SENSORS
MINIATURED VERSION OF ELECTROCHEMICAL &
OPTICAL SENSOR DEVICES EMPLOYED IN VIVO
ADVANTAGES
Real time monitoring
Critically ill patients ( Ph /PCO2/PO2 )
LIMITATIONS
Biological response of living system towards sensors
(CLOTTING)
Once inserted no reliable caliberation
82. APPLICATIONS
Measurement of O2 saturation
Measurement of Ph /PCO2 /Po2 based on clark
style design sensor
Glucose sensors – Fully automated
Feed back control of subcutaneos insulin
delivery