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- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Instrumental_Analysis_(LibreTexts)/23%3A_PotentiometryIn potentiometry we measure the potential of an electrochemical cell under static conditions. Because no current—or only a negligible current—flows through the electrochemical cell, its composition re...In potentiometry we measure the potential of an electrochemical cell under static conditions. Because no current—or only a negligible current—flows through the electrochemical cell, its composition remains unchanged. For this reason, potentiometry is a useful quantitative method of analysis.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/11%3A_Electrochemical_Methods/11.06%3A_Additional_ResourcesThe page outlines various experiments designed to introduce students to electrochemistry applications. The experiments are organized into categories including general electrochemistry, electrode prepa...The page outlines various experiments designed to introduce students to electrochemistry applications. The experiments are organized into categories including general electrochemistry, electrode preparation, potentiometry, coulometry, voltammetry, and amperometry.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/11%3A_Electrochemical_Methods/11.07%3A_Chapter_Summary_and_Key_TermsThis chapter covers three electrochemical analysis methods: potentiometry, coulometry, and voltammetry. Potentiometry involves measuring potential without significant current and using the Nernst equa...This chapter covers three electrochemical analysis methods: potentiometry, coulometry, and voltammetry. Potentiometry involves measuring potential without significant current and using the Nernst equation to calculate analyte activity. Coulometry is based on Faraday???s law to determine analyte quantity through electrical charge or current.
- https://chem.libretexts.org/Ancillary_Materials/Worksheets/Worksheets%3A_Analytical_Chemistry_II/PotentiometryTo take advantage of the analyte's electroactivity for analytical purposes, we need to be able to conduct electrons in and out of the solution. What else do you need in your system to measure the pote...To take advantage of the analyte's electroactivity for analytical purposes, we need to be able to conduct electrons in and out of the solution. What else do you need in your system to measure the potential of the complete cell? What do you want the potential of the reference electrode to be, changing or constant? After stopping the reaction and removing the enzyme, you put the Pt electrode back in.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Instrumental_Analysis_(LibreTexts)/22%3A_An_Introduction_to_Electroanalytical_Chemistry/22.06%3A_Types_of_Electroanalytical_MethodsWe divide electrochemical techniques into static techniques and dynamic techniques. In a static technique we do not allow current to pass through the electrochemical cell and, as a result, the concent...We divide electrochemical techniques into static techniques and dynamic techniques. In a static technique we do not allow current to pass through the electrochemical cell and, as a result, the concentrations of all species remain constant. Dynamic techniques, in which we allow current to flow and force a change in the concentration of species in the electrochemical cell, comprise the largest group of interfacial electrochemical techniques.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Analytical_Chemistry/2%3A_Analytical_Chemistry_2.0_(Harvey)/12%3A_Electrochemical_Methods/12.2%3A_Potentiometric_MethodsIn potentiometry we measure the potential of an electrochemical cell under static conditions. Because no current—or only a negligible current—flows through the electrochemical cell, its composition re...In potentiometry we measure the potential of an electrochemical cell under static conditions. Because no current—or only a negligible current—flows through the electrochemical cell, its composition remains unchanged. For this reason, potentiometry is a useful quantitative method. The first quantitative potentiometric applications appeared soon after the formulation of the Nernst equation, which relates an electrochemical cell’s potential to the concentration of electroactive species in the cell.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/12%3A_Chromatographic_and_Electrophoretic_Methods/12.06%3A_Other_Forms_of_ChromatographyThe text covers various liquid chromatography techniques, focusing on liquid-solid adsorption, ion-exchange, and size-exclusion chromatography. Liquid-solid chromatography involves polar stationary ph...The text covers various liquid chromatography techniques, focusing on liquid-solid adsorption, ion-exchange, and size-exclusion chromatography. Liquid-solid chromatography involves polar stationary phases and nonpolar solvents for separating compounds, excelling in analyzing isomers. Ion-exchange chromatography uses resin beads with ionic functional groups to separate ions based on their affinity for the exchange sites, utilizing gradient elutions to affect solute retention.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Instrumental_Analysis_(LibreTexts)/23%3A_Potentiometry/23.03%3A_Membrane_Indicator_ElectrodesIf metals were the only useful materials for constructing indicator electrodes, then there would be few useful applications of potentiometry. In 1906, Cremer discovered that the potential difference a...If metals were the only useful materials for constructing indicator electrodes, then there would be few useful applications of potentiometry. In 1906, Cremer discovered that the potential difference across a thin glass membrane is a function of pH when opposite sides of the membrane are in contact with solutions that have different concentrations of H+. The existence of this membrane potential led to the development of a new class of indicator electrodes, which we call ion-selective electrodes.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/09%3A_Titrimetric_Methods/9.05%3A_Precipitation_TitrationsThe document discusses precipitation titrimetry, a type of titration where the analyte and titrant form an insoluble precipitate. It covers historical applications, calculation of titration curves, an...The document discusses precipitation titrimetry, a type of titration where the analyte and titrant form an insoluble precipitate. It covers historical applications, calculation of titration curves, and methods for identifying the end point using indicators or potentiometric titrations. The document also provides quantitative applications and calculations for estimating analyte concentrations in mixtures.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Instrumental_Analysis_(LibreTexts)/23%3A_Potentiometry/23.02%3A_Metallic_Indicator_ElectrodesIn potentiometry, the potential of the indicator electrode is proportional to the analyte’s activity. Two classes of indicator electrodes are used to make potentiometric measurements: metallic electro...In potentiometry, the potential of the indicator electrode is proportional to the analyte’s activity. Two classes of indicator electrodes are used to make potentiometric measurements: metallic electrodes, which are the subject of this section, and ion-selective electrodes, which are covered in the next section.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/11%3A_Electrochemical_Methods/11.01%3A_Overview_of_ElectrochemistryThis chapter focuses on analytical electrochemistry, which uses measurements of potential, current, or charge to determine analyte concentration or chemical reactivity. Key concepts include the relati...This chapter focuses on analytical electrochemistry, which uses measurements of potential, current, or charge to determine analyte concentration or chemical reactivity. Key concepts include the relationship between electrode potential and analyte form, differences in surface and bulk concentrations, current's role in measuring redox rates, and the balance between controlling current and potential.
