Focuses on measurement of pH, ORP (Redox), and Conductivity and aspects related to inline measurement of these critical analytical parameters. Discussion topics include scientific theory, measurement challenges, proper troubleshooting, installation, key applications, and the future of analytical measurements
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.
Reference electrodes are used to maintain a constant potential against which the potential of an indicator or working electrode can be measured. An ideal reference electrode has a reproducible and stable potential that is not affected by small currents or changes in temperature or solution composition. Common reference electrodes include the standard hydrogen electrode, which defines zero potential, and silver/silver chloride electrodes. Reference electrodes are used along with indicator or working electrodes in electrochemical cells to measure the potential difference between the electrodes, which depends on the analyte concentration.
Conductivity measurement techniques include 2-electrode, 4-electrode, and inductive methods. Conductivity is a measure of a solution's ability to conduct electricity and is calculated using conductance, resistance, voltage, current, and cell constant. Factors like temperature, polarization, and contamination can affect conductivity readings so calibration is important. Conductivity is used in various applications like water treatment, leakage detection, and interface detection.
The document discusses pH control solutions and key considerations for pH measurement and control. It notes that pH control presents extraordinary challenges due to the extreme sensitivity and nonlinearity of pH measurements. Proper configuration of measurement equipment and control strategies are required to account for factors like temperature effects, sensor drift, and nonlinear titration curves. The document also highlights important valve requirements and process considerations for achieving tight pH control.
The document discusses pH measurement using a Yokogawa Model PH8EHP pH sensor. Key points:
- The sensor uses a glass electrode method to measure pH in water from 0-50°C at flows from 30-600 ml/min.
- Two-point calibration is standard, using either automatic or manual calibration. Automatic calibration avoids errors.
- Calibration involves measuring the sensor response in pH buffer solutions and adjusting the readings to match the buffer values. The sensor slope can also be directly entered.
- Troubleshooting focuses on checking for broken sensor glass or aging membranes if impedance readings are too high or low. Verifying proper submersion and response in buffers can diagnose
Potentiometry involves measuring the potential of electrochemical cells under conditions of no current flow. There are two types - direct potentiometry measures the potential of indicator electrodes related to analyte concentration, while indirect potentiometry involves measuring potential changes during titrations. A potentiometric cell consists of a reference electrode that maintains a constant potential, an indicator electrode whose potential varies with analyte concentration, and a salt bridge. The Nernst equation describes the relationship between electrode potential and analyte concentration or activity.
Potentiometry is an electroanalytical technique where the potential difference between two electrodes is measured under conditions of no current flow. It was invented in 1841 by Johann Christian Poggendorff using a slide-wire potentiometer. A potentiometric cell consists of a reference electrode with a known potential and an indicator electrode, whose potential changes depending on the analyte concentration. The potential difference between the electrodes is measured to determine the analyte concentration. Common applications of potentiometry include titrations, analysis of pollutants, drugs, foods, and more.
This document discusses potentiometry, which 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.
Reference electrodes are used to maintain a constant potential against which the potential of an indicator or working electrode can be measured. An ideal reference electrode has a reproducible and stable potential that is not affected by small currents or changes in temperature or solution composition. Common reference electrodes include the standard hydrogen electrode, which defines zero potential, and silver/silver chloride electrodes. Reference electrodes are used along with indicator or working electrodes in electrochemical cells to measure the potential difference between the electrodes, which depends on the analyte concentration.
Conductivity measurement techniques include 2-electrode, 4-electrode, and inductive methods. Conductivity is a measure of a solution's ability to conduct electricity and is calculated using conductance, resistance, voltage, current, and cell constant. Factors like temperature, polarization, and contamination can affect conductivity readings so calibration is important. Conductivity is used in various applications like water treatment, leakage detection, and interface detection.
The document discusses pH control solutions and key considerations for pH measurement and control. It notes that pH control presents extraordinary challenges due to the extreme sensitivity and nonlinearity of pH measurements. Proper configuration of measurement equipment and control strategies are required to account for factors like temperature effects, sensor drift, and nonlinear titration curves. The document also highlights important valve requirements and process considerations for achieving tight pH control.
The document discusses pH measurement using a Yokogawa Model PH8EHP pH sensor. Key points:
- The sensor uses a glass electrode method to measure pH in water from 0-50°C at flows from 30-600 ml/min.
- Two-point calibration is standard, using either automatic or manual calibration. Automatic calibration avoids errors.
- Calibration involves measuring the sensor response in pH buffer solutions and adjusting the readings to match the buffer values. The sensor slope can also be directly entered.
- Troubleshooting focuses on checking for broken sensor glass or aging membranes if impedance readings are too high or low. Verifying proper submersion and response in buffers can diagnose
Potentiometry involves measuring the potential of electrochemical cells under conditions of no current flow. There are two types - direct potentiometry measures the potential of indicator electrodes related to analyte concentration, while indirect potentiometry involves measuring potential changes during titrations. A potentiometric cell consists of a reference electrode that maintains a constant potential, an indicator electrode whose potential varies with analyte concentration, and a salt bridge. The Nernst equation describes the relationship between electrode potential and analyte concentration or activity.
Potentiometry is an 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.
The document discusses pH control and measurement. It provides an overview of pH concepts including:
- The definition of pH and how it relates to hydrogen and hydroxyl ion concentrations
- Details of how a pH sensor works including the glass electrode, reference electrode, and liquid junction
- Benefits of smart pH sensors which store calibration data to enable sensor diagnostics and trending
- Examples of sensor diagnostics provided by smart sensors such as detecting broken glass, coated sensors, and non-immersed sensors
- How sensor parameters change over time and smart sensor trending can identify sensors needing replacement before measurements are compromised
The document summarizes the pH glass electrode, which is used to measure pH through the detection of hydrogen ion activity. It functions as a fast responding, hydrogen ion selective electrode. The electrode contains a lithium silicate glass membrane that forms a hydrated gel layer, allowing only hydrogen ions to penetrate and alter the electrochemical potential between the glass and reference electrode. It is able to measure pH based on the Nernst equation, with the potential changing approximately 60mV for every unit change in pH.
Inductively coupled plasma mass spectrometry (ICPMS) is a sensitive analytical technique used for elemental analysis. It involves generating gaseous atoms of elements from liquid samples using an argon plasma at temperatures of 7000-10000°C, then using a quadrupole mass analyzer to separate and detect ions based on their mass-to-charge ratio. ICPMS provides very low detection limits down to parts-per-trillion levels, multi-element capabilities, and a wide linear dynamic range of 9 orders of magnitude. However, it can be subject to spectral interferences from polyatomic ions, isobaric ions, and doubly charged ions that must be overcome through methods like collision or reaction cells. Advances in
Polarography is an electroanalytical technique that uses a dropping mercury electrode to determine the concentration of electroactive species in a solution. It works by measuring the current flowing between the indicator electrode and reference electrode as the voltage is increased. Polarography provides a polarogram graph of current vs voltage that shows diffusion currents and limiting currents to identify species present. It has advantages like simple sample handling, speed, sensitivity and limited use of organic solvents. Polarography is used in pharmaceutical analysis to determine concentrations of drugs, vitamins, hormones and other compounds.
There is no redox chemistry at the membrane; potential is
determined by the relative concentrations of the analyte on each side of
the membrane. By convention, the indicator electrode is considered to
be the cathode in a potentiometric device
Amperometric titration involves measuring the electric current produced by a titration reaction while keeping the voltage constant between electrodes. It can determine the endpoint of titrations involving an electroreducible ion being titrated with a counter ion. The diffusion current is measured and plotted against the titrant volume added. At the endpoint, there is a sharp change in current. Amperometric titration offers advantages like rapid analysis, ability to work with dilute solutions, and determination of insoluble substances. It finds applications in areas like determining water content and quantification of ions.
Slides giving an overview on pH and its measurement.
Contains information about pH meters, its calibration, maintenance , types of ph electrode and modern definition of pH
This document discusses conductivity meters, which measure the electrical conductivity of solutions. It describes two main types - contacting meters with electrodes, and inductive meters with wire coils. Conductivity depends on temperature and ion concentration, and is calibrated using standard solutions. Conductivity meters are used to monitor water quality, detect leaks, and ensure cleaning procedures in industries like pharmaceuticals.
Polarography and voltammetry are electroanalytical techniques that involve applying a potential to a working electrode and measuring the resulting current. Jaroslav Heyrovsky discovered polarography in 1922 and was awarded the Nobel Prize for it in 1959. Polarography uses a dropping mercury electrode as the working electrode, while voltammetry can use other electrodes like platinum. Both techniques involve varying the applied potential over time and analyzing the current-potential relationship known as a polarogram or voltammogram. Key parameters that can be determined include peak potentials, diffusion coefficients, and formal reduction potentials which provide qualitative and quantitative analysis of electroactive species in solution.
Conductivity measurement involves measuring how well a solution conducts electricity. There are two main types of conductivity sensors:
1. Contacting sensors which use electrodes in contact with the solution and can measure low conductivities. They are susceptible to fouling.
2. Inductive (toroidal) sensors which do not contact the solution and can be used in dirty applications. They require a minimum conductivity of 15 μS/cm.
Proper calibration and temperature compensation are important for accuracy. Contacting sensors are calibrated using standard solutions while inductive sensors require in-situ calibration accounting for installation effects. Temperature compensation considers the nonlinear increase in water conductivity and solute type.
We provide you Project Temperature Sensors – Types.You can choose the best of your choice and interest from the list of topics we suggested. All new project ideas that are appearing focuses to improve the knowledge of Engineering students.
https://www.elprocus.com
Visit our page to get more ideas on Project Report Format for Final Year Engineering Students these ideas developed by professionals.
Elprocus provides free verified electronic projects kits around the world with abstracts, circuit diagrams, and free electronic software. We provide guidance manual for Do It Yourself Kits (DIY) with the modules at best price along with free shipping.
This document describes amperometric titration techniques using polarography. It discusses three types of titration curves that can occur depending on whether the titrand, titrant, or both are reducible species. The titration procedure involves placing a sample solution in a polarographic cell, adding a supporting electrolyte, and measuring the diffusion current as a titrant is added. The shape of the resulting titration curve - decreasing, steady then increasing, or V-shaped - indicates which species are reducible. The method provides accurate end point determination from the titration curve graph with benefits such as a continuously renewed electrode surface and ability to measure diluted solutions. Disadvantages include time needed to remove dissolved oxygen and limitations of more negative potentials
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 involves measuring electrode potentials using a reference electrode and indicator electrode. The reference electrode maintains a constant potential while the indicator electrode's potential varies with analyte concentration. Common reference electrodes include the saturated calomel electrode and silver-silver chloride electrode. Indicator electrodes include pH electrodes, ion-selective electrodes, and redox electrodes. Potentiometric measurements are used in clinical chemistry, environmental monitoring, titrations, and various industrial applications like food processing.
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.
It is a well known fact that metal ions have a profound effect on cellular processes
The importance or the role that ions play in cellular activity can be gauged by the fact that most cells maintain a very critical Na+ & k+ balance between the extracellular and the intracellular spaces.
Any distribution in this critical balance is to the cellular metabolism through a drastic change in the osmotic pressure resulting in cellular swelling.
Amperometric titration is a technique where the potential between a polarizable working electrode and a non-polarizable reference electrode is kept constant. During titration, the diffusion current is measured, which changes as the concentration of the electroreducible ion changes. At the endpoint, there is a sharp change in the diffusion current. Amperometric titrations can be performed between an electroreducible ion and a non-electroreducible ion, or between two electroreducible ions. The titration conditions require that the titrant, titrate, or both be electroreducible, and the applied potential corresponds to the limiting current.
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.
This document discusses an electrical conductivity meter. It begins by defining electrical conductivity and its units of measurement. It then describes the working principle of conductivity meters, which use a potentiometric method with four electrodes to apply a current and measure potential. Conductivity meters are used to measure the conductivity of various materials, including metals, liquids, and solutions, for applications like quality control and monitoring purity in industries like manufacturing, aerospace, and agriculture.
A pH meter measures the concentration of hydrogen ions in a solution to determine if it is acidic or alkaline. It works by measuring the potential difference between a glass electrode that senses the hydrogen ions and a reference electrode in contact with a reference solution. The glass electrode contains a special glass bulb that allows hydrogen ions to interact with it, changing the electrochemical potential. This potential difference is measured by the pH meter and converted to a pH value. A silver chloride electrode is commonly used as the reference electrode due to its stable and reproducible reaction.
The document discusses pH control and measurement. It provides an overview of pH concepts including:
- The definition of pH and how it relates to hydrogen and hydroxyl ion concentrations
- Details of how a pH sensor works including the glass electrode, reference electrode, and liquid junction
- Benefits of smart pH sensors which store calibration data to enable sensor diagnostics and trending
- Examples of sensor diagnostics provided by smart sensors such as detecting broken glass, coated sensors, and non-immersed sensors
- How sensor parameters change over time and smart sensor trending can identify sensors needing replacement before measurements are compromised
The document summarizes the pH glass electrode, which is used to measure pH through the detection of hydrogen ion activity. It functions as a fast responding, hydrogen ion selective electrode. The electrode contains a lithium silicate glass membrane that forms a hydrated gel layer, allowing only hydrogen ions to penetrate and alter the electrochemical potential between the glass and reference electrode. It is able to measure pH based on the Nernst equation, with the potential changing approximately 60mV for every unit change in pH.
Inductively coupled plasma mass spectrometry (ICPMS) is a sensitive analytical technique used for elemental analysis. It involves generating gaseous atoms of elements from liquid samples using an argon plasma at temperatures of 7000-10000°C, then using a quadrupole mass analyzer to separate and detect ions based on their mass-to-charge ratio. ICPMS provides very low detection limits down to parts-per-trillion levels, multi-element capabilities, and a wide linear dynamic range of 9 orders of magnitude. However, it can be subject to spectral interferences from polyatomic ions, isobaric ions, and doubly charged ions that must be overcome through methods like collision or reaction cells. Advances in
Polarography is an electroanalytical technique that uses a dropping mercury electrode to determine the concentration of electroactive species in a solution. It works by measuring the current flowing between the indicator electrode and reference electrode as the voltage is increased. Polarography provides a polarogram graph of current vs voltage that shows diffusion currents and limiting currents to identify species present. It has advantages like simple sample handling, speed, sensitivity and limited use of organic solvents. Polarography is used in pharmaceutical analysis to determine concentrations of drugs, vitamins, hormones and other compounds.
There is no redox chemistry at the membrane; potential is
determined by the relative concentrations of the analyte on each side of
the membrane. By convention, the indicator electrode is considered to
be the cathode in a potentiometric device
Amperometric titration involves measuring the electric current produced by a titration reaction while keeping the voltage constant between electrodes. It can determine the endpoint of titrations involving an electroreducible ion being titrated with a counter ion. The diffusion current is measured and plotted against the titrant volume added. At the endpoint, there is a sharp change in current. Amperometric titration offers advantages like rapid analysis, ability to work with dilute solutions, and determination of insoluble substances. It finds applications in areas like determining water content and quantification of ions.
Slides giving an overview on pH and its measurement.
Contains information about pH meters, its calibration, maintenance , types of ph electrode and modern definition of pH
This document discusses conductivity meters, which measure the electrical conductivity of solutions. It describes two main types - contacting meters with electrodes, and inductive meters with wire coils. Conductivity depends on temperature and ion concentration, and is calibrated using standard solutions. Conductivity meters are used to monitor water quality, detect leaks, and ensure cleaning procedures in industries like pharmaceuticals.
Polarography and voltammetry are electroanalytical techniques that involve applying a potential to a working electrode and measuring the resulting current. Jaroslav Heyrovsky discovered polarography in 1922 and was awarded the Nobel Prize for it in 1959. Polarography uses a dropping mercury electrode as the working electrode, while voltammetry can use other electrodes like platinum. Both techniques involve varying the applied potential over time and analyzing the current-potential relationship known as a polarogram or voltammogram. Key parameters that can be determined include peak potentials, diffusion coefficients, and formal reduction potentials which provide qualitative and quantitative analysis of electroactive species in solution.
Conductivity measurement involves measuring how well a solution conducts electricity. There are two main types of conductivity sensors:
1. Contacting sensors which use electrodes in contact with the solution and can measure low conductivities. They are susceptible to fouling.
2. Inductive (toroidal) sensors which do not contact the solution and can be used in dirty applications. They require a minimum conductivity of 15 μS/cm.
Proper calibration and temperature compensation are important for accuracy. Contacting sensors are calibrated using standard solutions while inductive sensors require in-situ calibration accounting for installation effects. Temperature compensation considers the nonlinear increase in water conductivity and solute type.
We provide you Project Temperature Sensors – Types.You can choose the best of your choice and interest from the list of topics we suggested. All new project ideas that are appearing focuses to improve the knowledge of Engineering students.
https://www.elprocus.com
Visit our page to get more ideas on Project Report Format for Final Year Engineering Students these ideas developed by professionals.
Elprocus provides free verified electronic projects kits around the world with abstracts, circuit diagrams, and free electronic software. We provide guidance manual for Do It Yourself Kits (DIY) with the modules at best price along with free shipping.
This document describes amperometric titration techniques using polarography. It discusses three types of titration curves that can occur depending on whether the titrand, titrant, or both are reducible species. The titration procedure involves placing a sample solution in a polarographic cell, adding a supporting electrolyte, and measuring the diffusion current as a titrant is added. The shape of the resulting titration curve - decreasing, steady then increasing, or V-shaped - indicates which species are reducible. The method provides accurate end point determination from the titration curve graph with benefits such as a continuously renewed electrode surface and ability to measure diluted solutions. Disadvantages include time needed to remove dissolved oxygen and limitations of more negative potentials
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 involves measuring electrode potentials using a reference electrode and indicator electrode. The reference electrode maintains a constant potential while the indicator electrode's potential varies with analyte concentration. Common reference electrodes include the saturated calomel electrode and silver-silver chloride electrode. Indicator electrodes include pH electrodes, ion-selective electrodes, and redox electrodes. Potentiometric measurements are used in clinical chemistry, environmental monitoring, titrations, and various industrial applications like food processing.
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.
It is a well known fact that metal ions have a profound effect on cellular processes
The importance or the role that ions play in cellular activity can be gauged by the fact that most cells maintain a very critical Na+ & k+ balance between the extracellular and the intracellular spaces.
Any distribution in this critical balance is to the cellular metabolism through a drastic change in the osmotic pressure resulting in cellular swelling.
Amperometric titration is a technique where the potential between a polarizable working electrode and a non-polarizable reference electrode is kept constant. During titration, the diffusion current is measured, which changes as the concentration of the electroreducible ion changes. At the endpoint, there is a sharp change in the diffusion current. Amperometric titrations can be performed between an electroreducible ion and a non-electroreducible ion, or between two electroreducible ions. The titration conditions require that the titrant, titrate, or both be electroreducible, and the applied potential corresponds to the limiting current.
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.
This document discusses an electrical conductivity meter. It begins by defining electrical conductivity and its units of measurement. It then describes the working principle of conductivity meters, which use a potentiometric method with four electrodes to apply a current and measure potential. Conductivity meters are used to measure the conductivity of various materials, including metals, liquids, and solutions, for applications like quality control and monitoring purity in industries like manufacturing, aerospace, and agriculture.
A pH meter measures the concentration of hydrogen ions in a solution to determine if it is acidic or alkaline. It works by measuring the potential difference between a glass electrode that senses the hydrogen ions and a reference electrode in contact with a reference solution. The glass electrode contains a special glass bulb that allows hydrogen ions to interact with it, changing the electrochemical potential. This potential difference is measured by the pH meter and converted to a pH value. A silver chloride electrode is commonly used as the reference electrode due to its stable and reproducible reaction.
Electrical conductivity is a material's ability to conduct electric current. It is measured in siemens per meter. Materials with many movable charged particles like electrons or ions are good conductors of electricity, while insulators contain few mobile charges. An experiment was described to test conductivity using a battery, lamp, wire, and pencil lead. As the lamp was moved farther from the pencil lead, its brightness dimmed, showing that the pencil lead is a poor conductor over long distances due to few mobile charges.
Introduction to Functional Safety and SIL CertificationISA Boston Section
This overview session will acquaint attendees with the key concepts in the IEC 61508 standard for functional safety of electrical/electronic and programmable electronic systems. An introduction is provided to safety integrity levels (SIL), the safety lifecycle and the requirements needed to achieve a functional safety certificate. Information will be provided on documentation requirements and an introduction to the basic objectives of product design for functional safety.
In this day and age of automated computer control valve sizing, the logic and theories behind it are invisible. In his presentation, Al Holton of Allagash Valve & Controls will look at the basic principles that apply and how they affect the application and installation of a wide range of control valve types. He will also review the reasoning behind valve type selection.
This document discusses maintaining accuracy of tunable diode laser (TDL) measurements in high temperature applications. It outlines sources of temperature error for TDLs, including external temperature sensors being too far from the measurement path and temperature gradients over long path lengths. Experimental results show up to 30% error in oxygen concentration measurements due to a 40°C temperature difference. The document recommends using spectral temperature measurements to account for temperature effects and achieve fully accurate TDL measurements.
The document discusses various oxygen measurement applications across different industries including storage and environment, upstream and processing, recovery and waste, downstream and purification. It provides examples of successful oxygen measurement applications in pharmaceutical API manufacturing, blanketing in mixing stirrers, centrifuge inertization, general manufacturing tank storage, and chemical manufacturing such as oxidation in extruders and waste-gas reclaiming.
- The document reports on an experiment investigating the limitations of electrical measurement devices like analog and digital multimeters.
- It was determined that the internal resistance of an analog ammeter was 0.504 ± 0.024 Ω. The voltage readings of a digital multimeter were found to be most accurate for measuring sinusoidal electrical quantities.
- The experiment analyzed the accuracy of different devices in measuring values like voltage, current, resistance, and more under various circuit conditions.
(Efc 4) european federation of corrosion guidelines on electrochemical corros...Muhammad Awais
This document provides guidelines for electrochemical corrosion measurements. It is published by the European Federation of Corrosion Working Party on Physicochemical Methods of Corrosion Testing. The document contains 8 chapters that cover topics such as instrumentation and calibration, electrochemical cell design, electrode design, reference electrodes, sample preparation, evaluation of ohmic drop, automatic measurement systems, and field testing. The overall aim is to provide practical guidance on how to properly perform various electrochemical corrosion experiments and measurements in both laboratory and field settings.
Chapter 4: Corrosion testing
(shared using VisualBee)Nima_s70
This chapter discusses corrosion testing methods and considerations. It describes 4 types of corrosion tests: 1) laboratory tests using small specimens, 2) pilot-plant tests that duplicate full-scale operations, 3) actual service tests in operating plants, and 4) field tests using exposed specimens. Key factors discussed include the materials tested, specimen size and shape, surface preparation, measurement techniques, exposure methods, and types of tests like boiling tests and sea water tests. The goal of corrosion testing is to evaluate materials, mechanisms, and environments in a controlled and reproducible manner.
The document provides an overview of oxygen measurement solutions from Mettler-Toledo for process analytics. It discusses key drivers for oxygen measurement, amperometric measurement techniques, sensor design features, system offerings including transmitters and housings, and applications and case studies. The presentation aims to demonstrate how Mettler-Toledo's oxygen measurement solutions can help customers improve process control, product quality, and operational efficiency.
external & internal corrosion monitoringsair ali khan
Cathodic protection and corrosion control monitoring techniques are used to protect buried metallic structures from corrosion. Cathodic protection involves making the structure more negatively charged than its environment to prevent corrosion. Close interval potential surveys, pipe-to-soil potential tests, and pipeline current mapping are used to monitor cathodic protection effectiveness. Corrosion coupons, electrical resistance probes, and residual inhibitor analysis also monitor corrosion by measuring factors like metal loss and inhibitor concentration over time. Together, these techniques provide continuous monitoring to ensure corrosion control and protect critical pipeline infrastructure.
The Utility of Zeta Potential Measurements in the Characterization of CMP Slu...HORIBA Particle
This document discusses the utility of zeta potential measurements in characterizing CMP slurries. It explains that the zeta potential and interfacial chemistry of particles in slurries are fundamental parameters that control dispersion stability and system properties. The zeta potential depends on factors like pH, electrolyte concentration, and particle surface chemistry. Maintaining the proper zeta potential is important for optimizing the polishing efficiency and surface smoothness of CMP slurries.
Diploma_I_Applied science(chemistry)U-III Acid & bases Rai University
1) Acids cause substances like lemons and food to be sour and can damage materials like teeth and sculptures. Acids have positively charged hydrogen ions and turn litmus red.
2) Bases have negatively charged hydroxide ions, feel slippery, and turn litmus blue. Common bases include hand soaps and drain cleaners.
3) The Brønsted-Lowry concept defines acids as proton donors and bases as proton acceptors in reversible acid-base reactions. Both acids and bases can act as conjugates of each other by gaining or losing protons.
The document discusses body fluids and electrolytes. It covers the functions of fluids, components of body fluids, fluid compartments, factors affecting fluid balance, and disturbances in fluid balance like edema and dehydration. It also discusses electrolytes like sodium, potassium, chloride, their functions, and electrolyte imbalances including hyponatremia, hypernatremia, hyperkalemia, and hypokalemia.
This document is about a certificate program called SAChE (Safety and Chemical Engineering) that focuses on Inherently Safer Design. The document was written by Hema Madaka and appears to be related to a course called ELA905. It provides limited context in just the title and metadata, so a 3 sentence summary can only state the high level topics covered rather than analyze or explain the document's contents or purpose.
This document discusses the concepts of usability and principles of usable design. It defines usability as the effectiveness, efficiency and satisfaction with which users can achieve goals in particular environments according to ISO standards. There are 10 principles of usable design including consistency, compatibility, feedback, and error prevention. The document also outlines 6 steps for designing a usable product which are to identify goals, establish characteristics and their effects, test prototypes, review compliance, and ensure correct design.
The document introduces Functional Integrity Certification, which is described as the first combined certification for functional safety and functional security. It provides contact information for exida, the company offering this certification. exida aims to help customers comply with industry standards for functional safety, cyber security, and alarm management through independent services and tools. The document lists some of exida's major customers and gives an overview of the company's scope, services, industries served, and what it does to provide functional safety and cyber security consultancy and certification.
Safety Lifecycle Management - Emerson Exchange 2010 - Meet the Experts Mike Boudreaux
The document discusses process safety and functional safety. It covers many topics related to ensuring safety in industrial processes, including safety lifecycles, risk assessments, safety instrumented systems, standards like IEC 61511, and maintaining safety through proper design, installation, operation and modification of systems.
What story are you telling about your products?Mike Boudreaux
This document discusses effective storytelling techniques for presentations. It outlines the key elements of a compelling story, including getting the audience's attention, stimulating desire, and reinforcing the message with reasons. The document explores different story archetypes like the hero's journey and provides examples of how to construct stories around products or services. It also distinguishes stories from lectures and highlights aspects that make stories more engaging and persuasive.
Isa saint-louis-advanced-p h-short-course-day-1Jim Cahill
- The document summarizes key points from a presentation on advanced pH measurement and control. It discusses challenges in pH control and new technologies for high temperature glass electrodes, wireless transmitters, and online diagnostics.
- Titration curves are essential for pH system design but can be deceptive due to nonlinearity. Factors like temperature, solvent concentration, and CO2 levels can also impact measured pH.
- Accurate pH measurement requires selecting the proper glass and reference electrodes for the process and using techniques like middle signal selection and online diagnostics to detect errors.
A pH meter measures the acidity or alkalinity of solutions by measuring hydrogen ion concentration using an ion-sensitive electrode. It operates similarly to a galvanic cell and has different modes including standby, pH measurement, millivolt reading, and automatic temperature control. Calibration involves one-point or two-point procedures using buffer solutions to standardize the meter's readings. Proper maintenance of the electrode and regular calibration of the pH meter are important to ensure accurate measurements. Common issues like unstable readings, slow response times, or calibration errors can usually be addressed by cleaning the electrode and recalibrating the instrument.
The document discusses pH and how it is measured using a pH electrode. It defines pH as the negative logarithm of hydrogen ion concentration on a scale of 0-14. It then explains that a pH electrode consists of a sensing glass bulb electrode and a reference electrode connected by an internal electrolyte solution. The sensing electrode develops a potential based on the hydrogen ion activity of the sample solution. The reference electrode provides a stable reference potential for comparison. The document outlines factors that can affect pH measurement accuracy such as temperature, ion interference, and conductivity. It also discusses electrode calibration using buffer solutions of known pH values.
pH is a measure of acidity or alkalinity on a scale of 0 to 14. A pH below 7 is acidic, above 7 is alkaline, and 7 is neutral. pH is defined as the negative logarithm of hydrogen ion concentration and represents the ratio of hydrogen and hydroxide ions in solution. pH is measured using a pH meter which consists of electrodes, a meter, and buffers for calibration and provides a quantitative measurement of acidity or alkalinity. Temperature affects pH measurements so compensation is required for accurate readings.
This document describes procedures for potentiometric titration experiments involving aspirin, vinegar, and sodium carbonate samples. Potentiometric titration uses a pH electrode and reference electrode connected to a pH meter to monitor pH changes during titration. For the aspirin experiment, an aspirin tablet is dissolved and titrated with sodium hydroxide while pH is recorded. The vinegar experiment involves titrating a vinegar sample with hydrochloric acid. For sodium carbonate, the sample produces two equivalence points when titrated with hydrochloric acid due to its carbonate ions. Data analysis involves calculating percent composition and errors from the titration curves and derivative plots.
This document discusses pH measurement and provides details on:
- The definition and scale of pH as a measure of acidity or alkalinity.
- Why pH is measured in various industries and applications.
- The principles of pH measurement using a glass electrode and pH meter.
- Factors that affect pH measurement accuracy such as temperature, ionic strength, and electrode calibration.
- The process of calibrating pH electrodes using buffer solutions and adjusting for the Nernstian slope.
The document describes an experiment involving potentiometric titration and determination of acid dissociation constants. Key steps included:
1) Calibrating a pH meter in buffer solutions and measuring the pH of hair conditioners.
2) Titrating acetic acid with sodium hydroxide while monitoring pH.
3) Constructing a titration curve and identifying the endpoint using the first derivative.
4) Calculating the acid dissociation constant of acetic acid and obtaining 11.43% relative error.
The document discusses pH and conductivity measurement and control. It begins by explaining that pH control presents problems for many industries. It then outlines three steps to minimize pH control problems: 1) applying pH process knowledge, 2) proper instrument design and selection, and 3) regular calibration and maintenance. The document goes on to explain pH concepts like the scale and how pH meters work. It also covers conductivity measurement and provides examples of conductivity levels in different solutions. Finally, it discusses calibration techniques and practical applications of pH and conductivity measurement.
This document describes a steam and water analysis system (SWAS) for a power plant. It discusses the need for online monitoring of critical water parameters to prevent equipment damage from scaling and corrosion. The SWAS conditions samples through cooling, pressure regulation, and filtering before analyzing parameters like pH, conductivity, dissolved oxygen, silica, and phosphate. It provides details on sample inlet schematics, equipment, analyzer specifications and calibration procedures. Maintaining water purity is important for protecting steam turbines and other apparatus.
This document summarizes an experiment to calibrate a pH meter and measure the pH of hair conditioners. The pH meter was calibrated using pH 4, 7, and 10 buffer solutions. The pH and electrode potential of three hair conditioner brands dissolved in water were then measured. The measured pH values were close to the calculated pH values based on electrode potential, with less than 1.3% error. The calibration process and measurements of hair conditioner pH provided an example of using a pH meter for analysis and quality control in various industries.
This document discusses analytical instrumentation used to measure pH and conductivity. It begins by stating that maintaining analytical instruments is a major challenge for industries. It then provides details on pH, including its scale from 0-14 and how pH meters work by measuring the voltage difference between reference and measuring electrodes. The document also covers conductivity measurement and its applications in determining salt content and water quality. It concludes by listing some common water quality and air quality parameters that are monitored along with other types of analytical instruments.
Measurement of Hydrogen Ion Concentration (pH)ECRD IN
This document discusses pH and methods of measuring pH. It begins with an overview of pH and what it measures. It then describes the pH scale and how pH values are calculated from hydrogen ion concentration. Various pH indicators and their color changes in different pH ranges are presented in a table. The document mainly focuses on using a pH meter with glass electrodes to accurately measure pH. It provides details on operating, calibrating, and storing measurements with a pH meter. Buffer solutions used for calibration are also described.
This document discusses pH and methods of measuring pH. It begins with an overview of pH and what it measures. It then describes the pH scale and how pH values are calculated from hydrogen ion concentration. Various pH indicators and their color changes in different pH ranges are presented in a table. The document mainly focuses on using a pH meter with glass electrodes to accurately measure pH. It provides details on operating, calibrating, and storing measurements with a pH meter. Buffer solutions used for calibration are also described.
Measurement of hydrogen ion concentration (p h)ECRD2015
This document discusses pH and methods of measuring pH. It begins with an overview of pH and what it measures. It then describes the pH scale and how pH values are calculated from hydrogen ion concentration. Various pH indicators and their color changes in different pH ranges are presented in a table. The document mainly focuses on using a pH meter with glass electrodes to accurately measure pH. It provides details on operating, calibrating, and storing measurements with a pH meter. Buffer solutions used for calibration are also described.
The document discusses pH electrodes and how pH meters work. It contains the following key points:
1. pH meters measure the voltage generated by a solution, which indicates the concentration of hydrogen ions and allows the measurement of pH.
2. A pH meter contains a glass electrode that interacts with hydrogen ions in the solution and a reference electrode to provide a baseline measurement.
3. The voltage measured corresponds to pH - a higher voltage means more hydrogen ions and lower pH, while a lower voltage means fewer hydrogen ions and higher pH.
4. Factors like the calibration standards used, junction potentials, temperature, and contaminants on the probe can introduce errors in pH measurements. Regular calibration and cleaning of electrodes
pH meters measure the hydrogen-ion concentration in solutions by determining the voltage difference between a pH electrode and a reference electrode immersed in the solution. The pH electrode, usually made of glass, detects the hydrogen-ion concentration in the solution, while the reference electrode provides a point of reference for the electrical potential. pH meters are calibrated using standard buffer solutions and can then be used to precisely measure pH levels, with applications across industries like chemistry, agriculture, food production, and healthcare.
Magical Mystery Tour of High Purity pH Measurements Yokogawa1
The measurement of high purity pH samples in power applications presents significant challenges to understand, apply and maintain analysis instrumentation. The source of the additional “magic” is the fact that high purity samples by their very nature have a very low conductivity, which presents its own set of issues and challenges in comparison to routine pH measurements. The presentation will explore the theory of pH and how it can be successfully applied in high purity applications, discuss both standard and solution temperature compensation, review installation requirements, and illustrate good calibration and maintenance procedures to facilitate satisfactory measurements.
In this webinar we will:
Review the theory behind the measurement of pH
Discuss the issues surrounding high purity pH measurements
Illustrate the difference between standard and solution temperature compensation
Assess installation requirements for successful measurements
Clarify good calibration and maintenance procedures
The aim of this book is to give a representative description of pH measurement in the process industries. The actual sensor, the pH electrode, is therefore the main focus of the text. Correct sensor use is fundamental for a meaningful pH measurement. Accordingly, both practical and theoretical requirements are discussed in depth so that the measuring principle is understood and an accurate measurement made possible.
The first section (practical considerations) of the book describes the sensor, and the other elements that constitute a pH measurement system. Together with a troubleshooting diagram, this section gives the information needed in order to ensure the correct working of the pH electrodes for long periods of time. The second, application orientated section gives solutions to different measuring tasks, giving examples from the lab and from industry. The last, theoretical part explains the basis of the pH measurement and completes, by further explanation, the information given in the first section. In addition, this book is outlined to be a useful tool in solving different measuring tasks. Thereby it can be read either in its totality or in parts.
This document provides an introduction to pH measurement, including:
1) It defines pH and explains that pH measures the concentration of hydronium ions in a solution, classifying solutions as acidic or alkaline.
2) It discusses why pH is measured, including for production quality control, cost control, safety, regulatory compliance, equipment protection, and research.
3) It describes the tools used for pH measurement, including pH electrodes made of glass sensitive to hydrogen ions, and reference electrodes, which are used together to determine the pH value of a sample solution.
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Analytical Measurements: Troubleshooting, Maintenance and the Future
1. pH & Conductivity Parameter Training Measurement, Maintenance & the Future ISA Boston Section March 15, 2011 U E 2 E 3 E 1 Reference- electrolyte E 6 E 5 E 4 Inner Buffer
4. Some examples of pH values 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 lemon juice orange juice beer cheese milk pure water egg white borax Milk of Magnesia H 2 SO 4 (1N) 4.9% HCl (0.1N) 0.37% acetic acid (0.1N) 0.6% HCN (0.1N) 0.27% sodium bicarbonate 0.84% (0.1N) potassium ac. 0.98% (0.1N) NH 4 OH 0.017% (0.01N) NH 4 OH 1.7% 1.0N NaOH 4%
5. How does pH measurement work? pH is a potentiometric measurement via an electrochemical sensor/electrode/probe U= E pH -E ref (mV) This potential difference is a function of the solution being measured E pH glass electrode E ref reference electrode high impedance pH Meter
7. What is special about pH glass? H + H + + + + + + + - - - - - - Acidic Alkaline Glass membrane Glass membrane (0.2 - 0.5mm) Gel layer ca. 1 µm (outer and inner) positive charge negative charge internal buffer The surface layer of the glass membrane is the “key performer” in each pH measurement! pH is a measurement of the potential difference between inner and outer layer of glass membrane! This is one reason why pH sensors need to be stored in salt solution when not in use!
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10. The Nernst Equation E = E 0 + 2.303 R T log n F 1. Internal Reference Potential 2. Inner Glass/Solution Potential 3. External Reference Potential 4. LIQUID JUNCTION POTENTIAL
11. The Nernst Equation E = E 0 + 2.303 R T log n F 2.303 R T is known as “The Electrode Slope” n F IDEAL SLOPE = 59.16 mV/pH unit at 25 °C Slope is temperature dependent
12. The Nernst Response Curve mV = 59.16 pH mV E = E o + 2.3 RT/F log a H + where 2.3 RT/F = 0.198T K = 59.16 mV @ 25 o C
36. Conductivity Measurement A conductivity “cell”, sensor, or electrode is an “electro-mechanical” measurement 1 cm 1 cm d = 1 cm Cond Solution Electrode plate VAC
45. Cell Geometry The measured resistance will be dependent on the spacing of the electrode – cell geometry “cell constant” Therefore, units measurement has dimension component, ex. mS/cm 1 cm 1 cm d = 1 cm Cond Solution Electrode plate VAC
52. Sensor Cell Constant 0.1 cm 0.1 cm -1 0.1 cm 1 cm Conductivity Cell Constant = Length Area 1 cm 1 cm 2 = = 1 cm -1 INSULATOR ELECTRODE ELECTRODE INNER OUTER 1 cm 1 cm
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57. Four-Electrode Conductivity Measurement AC Current Source AC Voltage Measurement Drive Electrodes Measuring Electrodes Four Electrode Sensor Four-Electrode Measuring Instrument
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63. Cell Installation -2 electrode NOT Recommended Cell Installation... INLET OUTLET OUTLET AIR INLET Avoid dead legs and air traps
64. Cell Installation -4 electrode Recommended OUTLET INLET Maintain a minimum clearance between sensor and pipe
65. Cell Installation -4 electrode NOT Recommended Maintain a minimum clearance between sensor and pipe
66. Conductivity, Resistivity, TDS Ranges Conductivity 100M 10M 1M 100K 10K 1K 100 10 1 Ultrapure water Deionized water Distilled water Condensate Drinking water Cooling tower water Percentage of acids, bases and salt Waste water Brackish water, Sea water Water for Industrial Process 5% Salinity 2% NaOH 20% HCl 0.01 .1 1 10 100 1000 10k 100k 1000k 0.021 0.4 4.6 46 460 4.6k 46k TDS ppm Conductivity and resistivity are measured at 25 C; TDS is expressed as Sodium Chloride (NaCl) Resistivity ohm-cm µS-cm
67. Main Applications and Measuring Range Inductive 4 Elec 2 Elec 0.01 0.1 1.0 10 100 1000 10k 100k 1000k Conductivity ( µ S/cm) 100 M 10M 1M 100k 10k 1000 100 10 1 Resistivity (Ohm-cm) Ultra pure water Pure water Make up water Drinking water Diluted acids, bases, salts Waste water Brackish water Industrial process water Acids, bases Water Processes Biotech/Food and Beverage Chemical Processes
70. Welcome to the Digital World! Same electrochemical end of the sensor converted to digital signal which is more robust and gives more information
71. Analog Sensor Technology Most analog sensors provide the user with one piece of information to determine the health of the sensor: Slope Limited information for troubleshooting
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77. Applications and Measurement Range Expanded range with enhanced accuracy! 0.01 0.1 1.0 10 100 1000 10k 100k 1000k Conductivity ( µ S/cm) 100 M 10M 1M 100k 10k 1000 100 10 1 Resistivity (Ohm-cm) Ultra pure water Pure water Make up water Drinking water Diluted acids, bases, salts Waste water Brackish water Industrial process water Acids, bases CURRENT 4E RANGE CURRENT 2E RANGE UniCond ® extends the range of measurement to cover UPW to seawater with a single sensor! UPW to seawater with a single UniCond ® sensor !
Some examples are: Beer 4,5 pH Milk 6,2 pH lemon juice 2,2 pH HCl 0,1 M 1 pH Activity a= concentration* activity factor. This activity factor is often estimated to be close to 1, and means activity~concentration
Describe reference system. Calomel reference (Hg/Hg 2 Cl 2 ) is the general electrochemical standard in place of the standard hydrogen electrode (describe!). Not suitable for industrial use: unstable above 60 o C toxic Preferred system is Ag/AgCl, essentially as good as the Calomel system but high temperature stable.
Walther Nernst developed the equation that bears his name in 1880’s (published 1889) Eo ‘standard’ potential for the electrode R universal gas constant T temperature (absolute, degrees Kelvin) F Faraday constant Valence number of ion not shown since it is 1
Walther Nernst developed the equation that bears his name in 1880’s (published 1889) Eo ‘standard’ potential for the electrode R universal gas constant T temperature (absolute, degrees Kelvin) F Faraday constant Valence number of ion not shown since it is 1
Walther Nernst developed the equation that bears his name in 1880’s (published 1889) Eo ‘standard’ potential for the electrode R universal gas constant T temperature (absolute, degrees Kelvin) F Faraday constant Valence number of ion not shown since it is 1
Some solutions aggressive towards the sensor and cause loss of calibration quicker than others pH 7 + 2.5 needs less calibration than pH 5.2 + 0.2 Quality - who makes it!
Walther Nernst developed the equation that bears his name in 1880’s (published 1889) Eo ‘standard’ potential for the electrode R universal gas constant T temperature (absolute, degrees Kelvin) F Faraday constant Valence number of ion not shown since it is 1
Walther Nernst developed the equation that bears his name in 1880’s (published 1889) Eo ‘standard’ potential for the electrode R universal gas constant T temperature (absolute, degrees Kelvin) F Faraday constant Valence number of ion not shown since it is 1
Walther Nernst developed the equation that bears his name in 1880’s (published 1889) Eo ‘standard’ potential for the electrode R universal gas constant T temperature (absolute, degrees Kelvin) F Faraday constant Valence number of ion not shown since it is 1
Conductivity is affected by temperature since water becomes less viscous at higher temperatures and ions can move more easily—they have greater mobility. Typical mineral ions increase in conductivity by about 2% of value per °C. Temperature as well as water purity can change the conductivity. For this reason, it has become an industry standard to compensate measurements to 25°C. That is, the conductivity value is reported as if the sample were at 25°C. General purpose temperature compensation provides the typical 2% per °C correction.
Conductivity is affected by temperature since water becomes less viscous at higher temperatures and ions can move more easily—they have greater mobility. Typical mineral ions increase in conductivity by about 2% of value per °C. Temperature as well as water purity can change the conductivity. For this reason, it has become an industry standard to compensate measurements to 25°C. That is, the conductivity value is reported as if the sample were at 25°C. General purpose temperature compensation provides the typical 2% per °C correction.
To minimize the problems of the two electrode design, a different method has been developed.
Four-electrode measurement refers to a conductivity sensor incorporating four electrodes into its probe body instead of the usual two. The four-electrode measuring technique is used for highly conductive and/or dirty water samples which would foul the surfaces and/or plug the narrow passages of conventional two-electrode conductivity sensors. Suspended solids, turbidity, silt and oils tend to coat electrode surfaces and accumulate in passages and produce negative conductivity errors with two-electrode conductivity systems. Four-electrode measurement applies an AC current through the sample via two outer drive electrodes. These electrodes may become fouled and the circuit will compensate to maintain the AC current level. Two inner measuring electrodes are used to sense the voltage drop through the portion of solution between them. The circuit makes a high impedance AC voltage measurement, drawing negligible current and making it much less affected by additional resistance due to fouling of the measuring electrode surfaces.
1. Electrode surface condition for high conductivity measurements with two-electrode systems is critical. The surface must be rough on a microscopic scale in order to provide very intimate contact with the sample. Otherwise a high resistance at the interface would cause low conductivity readings. 2. Coatings which insulate the electrodes of a two-electrode sensor have a direct impact on the accuracy, especially when the conductivity of the sample is high. Moderate insulation of the electrodes of four-electrode sensors has no effect since the voltage measurement is made with virtually no current flow. 3. The flat surface of four-electrode sensors is largely self-cleaning in high flow applications.
Inductive conductivity provides the best tolerance for fouling conditions, with no electrodes in contact with the sample. It can also be used for high purity chemical concentration measurements with its excellent chemical resistance and no wetted metal parts. Insertion and submersion mounting are available.
Conductivity cell installation must assure that the cell is completely immersed in water. No bubbles can be within the annular space between electrodes or erroneously low conductivity (high resistivity) readings will result. Upward flow is desirable so air can easily escape.
When installing in large pipe, do not use a series of reducing bushings that would create a “dead leg” of stagnant water around the cell. Tap directly into the pipe or into a pipe plug in a Tee. Deionization resin beads, if they escape from a column, can become lodged between the electrodes of a conductivity cell and short them, causing erroneously high conductivity (low resistivity) readings.
When installing in large pipe, do not use a series of reducing bushings that would create a “dead leg” of stagnant water around the cell. Tap directly into the pipe or into a pipe plug in a Tee. Deionization resin beads, if they escape from a column, can become lodged between the electrodes of a conductivity cell and short them, causing erroneously high conductivity (low resistivity) readings.
When installing in large pipe, do not use a series of reducing bushings that would create a “dead leg” of stagnant water around the cell. Tap directly into the pipe or into a pipe plug in a Tee. Deionization resin beads, if they escape from a column, can become lodged between the electrodes of a conductivity cell and short them, causing erroneously high conductivity (low resistivity) readings.
Typical ranges of applications are shown in resistivity, conductivity and Total dissolved solids (ppm TDS) units. The TDS scale here is based on the concentration of sodium chloride that would have the identified conductivity and resistivity. Other substances such as calcium carbonate may be use as the basis.
As we all know, In the sensor a small microprocessor has been integrated, that stores and process all relevant data. All this information is then digitally transferred to the instrument without any risk of interferences. The microprocessor is also able to store information like calibration values, identity and timestamp the maximum process temperature. What is even more interesting with ISM is the connection possibilities and how the sensors can perform there own diagnostics in real-time.
With the ISM we have transferred the technology experience and know how that we have collected over the years into the sensor and the sensor head. In the sensor a small microprocessor has been integrated, that stores and process all relevant data. All this information is then digitally transferred to the instrument. With this new technology, the ISM sensors are able to perform its own diagnostics in real-time. All our new transmitters are ready to handle the ISM technology and together with the ISM sensors they can perform true predictive maintenance.
SLIDE CAN BE SKIPPED IN CASE OF TIME PRESSURE There is an overlap in measuring range for inductive and 4E cond. Sensors We position the 4E sensors mainly for chemical, pharma-, and F&B application where the conditions are not to harsh. The inductive sensors are designed for chemical and P&P industrie where you have harsh conditions. Nevertheless, if the customer insist on either a 4E or inductive solution we now can offer both sensor types with best performance. SLIDE CAN BE SKIPPED IN CASE OF TIME PRESSURE