Name: using iodine to find unknown concentrations
Uploaded: 2024-12-05T18:31:57.000Z
Duration: 1 min 23 s
Channel: JoVE

قياس اليود وقياس اليود هما طريقتان يستخدمتان لتحليل كمية العوامل المؤكسدة أو المختزلة الموجودة في العينة ، على التوالي.
في المعايرة بالتحليل الحجمي باليودومتر ، عادة ما يتم تحمض محلول التحليل المؤكسد ومعالجته بفائض من أيونات اليوديد ، مما ينتج عنه كمية مكافئة من اليود في حالة توازن مع ثلاثي يوديد. ثم يتم معايرة اليود المحرر ضد عامل اختزال موحد.
يضاف محلول النشا المحضر حديثا بالقرب من نقطة النهاية ، مما يشكل مركبا من النشا واليود الأزرق الداكن. ثم تستمر المعايرة بالتحليل الحجمي حتى يختفي اللون الأزرق.
تتيح العلاقة المتكافئة عبر اليود بين المادة التحليلية المؤكسدة ومحلول المعايرة بالتحليل الكيميائي المختزل تحديد تركيز المادة المراد تحليلها.
في المقابل ، تتضمن معايرة اليود معايرة مباشرة لمادة تحليلية مختزلة في وجود النشا مقابل محلول اليود القياسي حتى يتحول المحلول إلى اللون الأزرق الداكن ، مما يدل على أن كل المواد المراد تحليلها تتأكسد وأن مركب النشا واليود يتشكل .
بمعرفة القياس المتكافئ للتفاعل وحجم محلول المعايرة بالتحليل الكيميائي المستهلك ، يمكن تحديد تركيز المادة التحليلية.

المعايرة بالأكسدة والاختزال: اليودومتري واليوديمتري

Redox Titration: Iodimetry and Iodometry

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اليودومتري واليوديمتري هما طريقتان تحليليتان تستخدمان لتحديد تركيز العوامل المؤكسدة أو المختزلة باستخدام اليود. في المعايرات باليودومتري، عادة ما يتم تحميض محلول المحلل المؤكسد ومعالجته بكمية زائدة من أيونات اليوديد، مما يولد كمية مكافئة من اليود في حالة توازن مع ثلاثي اليوديد. يتم بعد ذلك معايرة اليود المنطلق مباشرة باستخدام عامل اختزال موحد. عندما يصبح لون محلول اليود المخفف أصفر باهتًا، تتم إضافة بضع قطرات من محلول النشا المحضر حديثًا، مما يؤدي إلى تكوين مركب نشا-يود أزرق داكن مكثف. تستمر المعايرة حتى اختفاء اللون الأزرق، مما يسمح بتحديد تركيز المحلل من خلال العلاقة المتكافئة بين اليود والمحلل المؤكسد والمعاير المختزل. يجب إجراء المعايرة بسرعة مع التقليب بقوة للحصول على نتائج دقيقة.

في المعايرات اليوديمترية، يتم معايرة المحلل المختزل مباشرة باستخدام محلول اليود القياسي في وجود النشا. يعمل النشا كمؤشر، حيث يشكل مركب نشا-يود أزرق داكن عندما يكون اليود زائدًا. أثناء تقدم المعايرة، يتفاعل المحلل المختزل مع اليود، مما يتسبب في انخفاض تركيز اليود. عندما يتفاعل المحلل المختزل بالكامل ويتأكسد تمامًا، فإن أي كمية إضافية من اليود لن تُختزل، مما يؤدي إلى تكوين مركب نشا-يود أزرق داكن. يشير هذا التغيير في اللون إلى نقطة نهاية المعايرة.

لتحديد تركيز المحلل، يتم النظر في القياسات الكيميائية للتفاعل (الممثلة بالمعادلة الكيميائية المتوازنة) وحجم محلول اليود القياسي المستخدم أثناء المعايرة. ومن خلال معرفة كمية اليود التي تفاعلت مع المحلل والعلاقة المتكافئة بين اليود والمحلل، يمكن تحديد تركيز المحلل المختزل في العينة الأصلية بدقة.
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قياس اليود وقياس اليود هما طريقتان تحليليتان تستخدمان لتحديد تركيز العوامل المؤكسدة أو المختزلة باستخدام اليود. في المعايرة بالتحليل الحجمي باليود ، ...

Education

JoVE Core

Analytical Chemistry

الكيمياء التحليلية

Unit 1

الوحدة الأولى

Electrochemical Analyses and Redox Titration

التحليلات الكهروكيميائية والمعايرة بالأكسدة والاختزال

electrochemical-analyses-and-redox-titration

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

using iodine to find unknown concentrations

Iodometry and iodimetry use iodine to measure unknown concentrations in redox titrations. These methods help determine the amount of an oxidizing or reducing agent in a sample. The key idea is that iodine changes color and reacts in a known stoichiometric ratio with the analyte.

In iodometric titrations, the sample usually contains an oxidizing agent. The solution is acidified and then treated with an excess of iodide ions, which releases an equivalent amount of iodine in equilibrium with triiodide. The iodine is then titrated against a standardized reducing agent.

As the iodine solution becomes pale yellow, a few drops of freshly prepared starch solution are added. Starch forms a dark blue starch-iodine complex. The titration continues until the blue color disappears. The sample should be stirred vigorously and the titration should be done quickly for accurate results.

In iodimetric titrations, the process is reversed. A reducing analyte is titrated directly with a standard iodine solution in the presence of starch. As the reducing analyte reacts with iodine, the iodine level drops. When all of the reducing analyte has reacted, extra iodine remains and the dark blue starch-iodine complex appears. That color change marks the endpoint.

For both methods, the concentration of the analyte is calculated from the balanced chemical equation and the volume of iodine solution or titrant used. The stoichiometric relationship between iodine and the analyte shows how much of the sample reacted. This makes iodometry and iodimetry useful analytical tools for measuring unknown redox concentrations.

Using Iodine to Find Unknown Concentrations

using-iodine-to-find-unknown-concentrations

electrochemistry: overview

Electrochemistry and Redox Reactions

Electrochemistry connects electrical measurements with chemical reactions, especially oxidation and reduction. It focuses on how electron movement helps explain reaction behavior. Oxidation is the loss of electrons from a substance, and reduction is the gain of electrons. A species with strong electron affinity is an oxidizing agent, or oxidant. A species that donates electrons is a reducing agent, or reductant. These redox steps are often described with half-reactions. When electrons move...

electrodes: overview

Types of Electrodes in Electrochemistry

Electrodes are conductive materials in an electrochemical cell. They allow electron transfer reactions to happen at their surfaces. Electrochemical measurements use them to control and measure current and potential. The working electrode, also called the indicator electrode, is the main sensing electrode. Its potential changes with the analyte concentration and with the activity of the electroactive species. Common indicator electrodes include inert platinum electrodes, silver electrodes that...

interfacial electrochemical methods: overview

interfacial-electrochemical-methods-overview

Static and Dynamic Electrochemical Methods

Static and dynamic electrochemical methods study what happens at the boundary between an electrode and a solution. These interfacial methods focus on the electrode-solution interface rather than the overall properties of the liquid. They are useful in electroanalytical chemistry because they can detect very small changes in analyte concentration. These methods are grouped by whether a nonzero current flows through the cell. Static methods, such as potentiometry, measure the cell potential...

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Potentiometry and Electrochemical Cell Potential

Potentiometry measures the potential difference between two electrodes in an electrochemical cell. It does this without drawing significant current, so the solution’s composition is not altered. The method uses an indicator electrode, which exchanges electrons with the analyte solution, and a reference electrode, which keeps a constant potential. Each electrode is placed in a solution that makes up a half-cell. In a common setup, the reference electrode is the anode, or left-hand electrode,...

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Reference and Indicator Electrodes in Potentiometry

Potentiometric measurements use reference electrodes and indicator electrodes to track changes in a solution. A reference electrode gives a stable baseline, while indicator and working electrodes respond to changes in the solution’s composition. The Standard Hydrogen Electrode, or SHE, is a common reference electrode. It keeps a zero potential at all temperatures. However, it needs a continuous supply of hydrogen gas, so it is not practical for routine use. The Saturated Calomel Electrode, or...

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Membrane Electrodes in Ion Sensing

Membrane electrodes measure ions by using a selective membrane that creates a potential difference across it. This membrane potential is called the asymmetry potential, and it can remain nonzero even when analyte concentrations are the same on both sides of the membrane. The signal usually depends on all ions in the sample that can interact with the membrane, not just one analyte. Selectivity is described by a selectivity coefficient. This value compares the response to an interferent with the...

redox titration: overview

Redox Titration Endpoints and Indicators

Redox titration uses electron transfer in a redox, or reduction-oxidation, reaction to find the concentration of an unknown solution. The titrant has a known concentration, and it is added gradually to the analyte, which is the solution being tested. The endpoint shows when the reaction between the two substances is complete. Before a redox titration begins, the analyte should be in a single oxidation state. If needed, this is done by pre-oxidizing or pre-reducing the sample with an auxiliary...

redox titration: iodimetry and iodometry

Iodometry and iodimetry use iodine to measure unknown concentrations in redox titrations. These methods help determine the amount of an oxidizing or reducing agent in a sample. The key idea is that iodine changes color and reacts in a known stoichiometric ratio with the analyte. In iodometric titrations, the sample usually contains an oxidizing agent. The solution is acidified and then treated with an excess of iodide ions, which releases an equivalent amount of iodine in equilibrium with...

redox titration: other oxidizing and reducing agents

redox-titration-other-oxidizing-and-reducing-agents

Choosing Oxidizing Titrants in Redox Titration

Redox titrations can use oxidizing titrants other than iodine. Common choices include potassium permanganate (KMnO4), cerium(IV), and potassium dichromate (K2Cr2O7). The best titrant depends on stability, cost, analyte strength, and the reaction rate between the analyte and the titrant. Potassium permanganate is a strong oxidizing titrant in highly acidic solution. It reduces from Mn(VII) to Mn(II) while it oxidizes the analyte to a higher oxidation state. KMnO4 also works as a self-indicator,...

potentiometric titration: overview

Endpoint Detection in Potentiometric Titration

Potentiometric titration is a quantitative analytical method used to find the concentration of an analyte by measuring the potential difference between two electrodes in a solution. The endpoint is the point where this potential changes sharply. It usually appears when the stoichiometric reaction between the analyte and the titrant is complete. To find the endpoint, the measured potential difference is plotted against the volume of titrant added. This graph is called a titration curve. A...

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Gran Plot for Titration Endpoint Prediction

A Gran plot helps predict the endpoint of a potentiometric or acid-base titration before the endpoint is reached. It uses titration data collected only up to a point that is still below the equivalence volume. The data are then transformed into a straight-line format. To build the plot, the line is extended to the x-axis. That x-intercept shows the titrant volume needed to reach the equivalence point. In potentiometric titration, the Gran plot uses the volume-corrected base-10 antilogarithm of...

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Electrode Weighing in Electrogravimetric Analysis

Electrogravimetric analysis measures an analyte by weighing the material that deposits on an electrode. A pre-weighed working electrode is placed in solution, and a potential is applied. The target substance then deposits by reduction at the cathode or by oxidation at the anode. After electrolysis, the electrode is weighed again. The mass increase gives the weight of the analyte in the solution. To check that deposition is complete, the fresh electrode surface is exposed to the solution while...

coulometry: overview

Coulometry and Electrical Charge Analysis

Coulometry is an analytical method that finds the amount of an analyte by measuring the electrical charge needed for its complete electrolysis. It is known for being rapid, accurate, and precise. Unlike many other methods, it does not require analytical standards. The total charge passed during electrolysis is linked to the amount of analyte through Faraday's laws of electrolysis. For correct coulometric measurements, the charge supplied must match Faraday's constant multiplied by the number...

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Measuring Analyte Charge by Potentiostatic Coulometry

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Controlled-Current Coulometry in Redox Analysis

Controlled current coulometry is an electrochemical method used to measure the amount of a substance by passing a steady current through a cell. It is also called amperostatic coulometry. The analyte, or substance being analyzed, reacts at the electrode surface as charge moves through the system. The amount of analyte is found by measuring how long it takes for a known charge to pass. This calculation follows Faraday’s laws of electrolysis. A typical setup includes a galvanostat, a...

controlled-current coulometry: coulometric titration

controlled-current-coulometry-coulometric-titration

Electrically Generated Reagents in Titration

Coulometric titrations use an electrically generated reagent to measure the amount of a substance in a sample. The electron acts as the standard reagent, and the result depends on the current and the time used to generate it. The method follows the same basic idea as a regular titration, including endpoint detection. Two conditions are essential for this type of titration. First, the electrode reaction that makes the reagent must be 100% efficient. Second, the generated reagent must react...

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Voltammetry for Detecting Redox Species

Voltammetry measures current in an electrochemical cell as the applied potential changes. It is an electroanalytical method used to study redox-active species. The current response is shown on a graph called a voltammogram. A voltammetric cell uses three electrodes: a working electrode, a reference electrode, and an auxiliary electrode. Redox reactions happen at the working electrode, and a potentiostat controls its potential. The reference electrode, such as a saturated calomel electrode or a...

voltammetry: factors affecting measurements

voltammetry-factors-affecting-measurements

Voltammetry and Faradaic Current

Voltammetry measures faradaic current, which is the current created by redox reactions of an analyte at the working and auxiliary electrodes. The current from reduction is called cathodic current and carries a positive charge. The current from oxidation is called anodic current and has a negative charge. The applied potential at the working electrode controls the flow of faradaic current. The size of that current depends on how fast the oxidation or reduction reaction occurs at the electrode...

voltammograms: overview

Voltammogram Shapes and Redox Analysis

Voltammograms are current plots made against applied potential. They help show how an electrochemical system behaves during a redox reaction. The shape of the plot depends on how the current is measured and on whether convection, or fluid movement, is present. When convection is present, as in hydrodynamic voltammetry, the voltammogram usually has a sigmoid shape. In this case, the current rises from a residual current to a limiting current at the analyte’s oxidation or reduction potential.

voltammetric techniques: linear-scan (e vs time)

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Polarography and Voltammetry with Mercury Drops

Polarography and hydrodynamic voltammetry are voltammetric techniques used to study electrochemical reactions. They track the current that flows as the electrode potential changes. In polarography, the key working electrode is a dropping mercury electrode, or DME. A DME uses a capillary tube filled with mercury. A tiny mercury droplet forms at the tip and then drops away. This gives a fresh electrode surface for each measurement. During the test, the potential applied to the DME changes...

voltammetric techniques: pulse voltammetry

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Pulse Voltage Methods for Electrochemistry

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voltammetric techniques: cyclic voltammetry

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Reading Redox Peaks with Cyclic Voltammetry

Cyclic voltammetry measures how current changes as the potential at an electrode is varied. It is used to study the redox properties of a chemical species, meaning how easily it is oxidized or reduced. The setup uses three electrodes in an electrolyte solution. The working electrode is where the redox reaction of interest takes place. The reference electrode provides a stable potential, and the counter electrode completes the circuit for current flow. The process starts at a chosen initial...

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Trace Analysis by Stripping Voltammetry

Stripping voltammetry is an electrochemical method used to detect trace amounts of analytes in solution. It works by applying a potential to an electrode and measuring the current that results. The current is then used to estimate the analyte concentration. Anodic Stripping Voltammetry, or ASV, is used for metals and metalloids at very low levels. It has two main steps: deposition and stripping. First, a negative potential reduces analyte ions and deposits them on the working electrode surface.

amperometry: overview

Measuring Analytes with Amperometric Sensors

Amperometry measures specific analytes in a solution by tracking the electric current from an electrochemical reaction. A constant potential is applied between a working electrode and a reference electrode. The current that results is proportional to the analyte concentration. The Clark oxygen electrode is a common example of amperometry. It uses a cathode and an anode sealed inside a gas-permeable membrane. The cathode is typically platinum or gold, and the anode is silver. When a potential...

key terms and concepts

Learn how iodometry and iodimetry use iodine, iodide, and starch to measure unknown oxidizing or reducing agents in redox titrations.

Using Iodine to Find Unknown Concentrations | JoVE K12

analytical chemistry

JoVE Core Analytical Chemistry simplifies complex chemical principles by breaking them down into clear, engaging animations, making topics from SI Units to NMR spectroscopy more accessible and straightforward. Additionally, the scientist-in-action videos highlight the application of these concepts in real-world research conducted in laboratories globally.

Using Iodine to Find Unknown Concentrations

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