REDOX TITRATIONS with IODINE Introduction
Total Page:16
File Type:pdf, Size:1020Kb
Load more
Recommended publications
-
Elementary Iodine-Doped Activated Carbon As an Oxidizing Agent for the Treatment of Arsenic-Enriched Drinking Water
water Article Elementary Iodine-Doped Activated Carbon as an Oxidizing Agent for the Treatment of Arsenic-Enriched Drinking Water Fabio Spaziani 1,2,*, Yuli Natori 1, Yoshiaki Kinase 1, Tomohiko Kawakami 1 and Katsuyoshi Tatenuma 1 1 KAKEN Inc., Mito Institute 1044 Hori, Mito, Ibaraki 310-0903, Japan 2 ENEA Casaccia, Via Anguillarese 301, 00123 Roma, Italy * Correspondence: [email protected] Received: 18 July 2019; Accepted: 23 August 2019; Published: 27 August 2019 Abstract: An activated carbon impregnated with elementary iodine (I2), named IodAC, characterized by oxidation capability, was developed and applied to oxidize arsenite, As(III), to arsenate, As(V), in arsenic-rich waters. Batch and column experiments were conducted to test the oxidation ability of the material. Comparisons with the oxidizing agents usually used in arsenic treatment systems were also conducted. In addition, the material has been tested coupled with an iron-based arsenic sorbent, in order to verify its suitability for the dearsenication of drinking waters. IodAC exhibited a high and lasting oxidation potential, since the column tests executed on water spiked with 50 mg/L of arsenic (100% arsenite) showed that 1 cc of IodAC (30 wt% I2) can oxidize about 25 mg of As(III) (0.33 mmol) before showing a dwindling in the oxidation ability. Moreover, an improvement of the arsenic sorption capability of the tested sorbent was also proved. The results confirmed that IodAC is suitable for implementation in water dearsenication plants, in place of the commonly used oxidizing agents, such as sodium hypochlorite or potassium permanganate, and in association with arsenic sorbents. -
Comparative Study of Oxidants in Removal of Chemical Oxygen Demand from the Wastewater (IJIRST/ Volume 4 / Issue 1/ 011)
IJIRST –International Journal for Innovative Research in Science & Technology| Volume 4 | Issue 1 | June 2017 ISSN (online): 2349-6010 Comparative Study of Oxidants in Removal of Chemical Oxygen Demand from the Wastewater Prof Dr K N Sheth Kavita V Italia Director PG Student Geetanjali Institute of Technical Studies, Udaipur Department of Environmental Engineering Institute of Science & Technology for Advanced Studies & Research, Vallabh Vidyanagar Abstract Chemical Oxygen Demand (COD) test involves chemical oxidation using chromic acid as a strong oxidizer. COD of a wastewater sample is the amount of oxidant- potassium dichromate that reacts with the sample when it is heated for 2 hours under controlled environmental conditions and result is expressed as mg of oxidant consumed per liter of a given sample of wastewater. COD can be helpful in determining the quantity required for dilution needed for conducting Biochemical Oxygen Demand (BOD) five day test. In the present investigation attempts have been made to use other oxidants like hydrogen peroxide H2O2, sodium hypo-chlorite, calcium hypo-chlorite and potassium permanganate for measurement of COD by standard method and compare the results obtained using potassium dichromate as strong oxidant. Experiments were carried out for each oxidizing agent for COD removal at temperatures like 1000C, 750C and 500C. The duration of exposure time in each experimental set up was taken as temperature wise, for 1000C, it was 1-5 minutes , for 750C it was 20-40 minutes and for 500C it was 45-75 minutes. It was found that temperature plays very important role in in deciding the exposure time to be allocated for reduction of COD. -
Titration of Aspirin Tablets
Bellevue College | CHEM& 161 Titration of Aspirin Tablets In this lab, you will determine the percent purity of two commercially available aspiring tablets using an acid-base titration. In general, an acid and a base react to produce a salt and water by transferring a proton (H+): HA (aq) + NaOH (aq) H2O (l) + NaA (aq) (1) acid base salt The active ingredient in aspirin, and the chemical for which aspirin is the common name, is acetylsalicylic acid. To determine the amount of aspirin (acetylsalicylic acid) in a sample, the precise volume and concentration of the NaOH, and the overall reaction, must be known. The NaOH serves as a secondary standard, because its concentration can change over time. To find the precise concentration of the NaOH, it must be titrated against a primary standard, an acid that dissolves completely in water, has a high molar mass, that remains pure upon standing, and is not hygroscopic (tending to attract water from the air). Because sodium hydroxide is hygroscopic, it draws water from its surroundings. This mean one cannot simply weigh out a sample of sodium hydroxide, dissolve it in water, and determine the number of moles of sodium hydroxide present using the mass recorded, since any sample of sodium hydroxide is likely to be a mixture of sodium hydroxide and water. Thus, the most common way to determine the concentration of any sodium hydroxide solution is by titration. Determining the precise concentration of NaOH using a primary standard is called standardization. You will first standardize your NaOH solution, and then use it to analyze aspirin tablets for their aspirin content and purity. -
Chemistry – Midterm Part 3 Material Unit Review Packet 2014 ALLEN
Chemistry – Midterm Part 3 Material Unit Review packet 2014 ALLEN 1. Label the following as chemical or physical change: Grass growing_____physical______ Dissolving sugar in water____ physical___ Evaporating water__physical____ Na in water appears to dissolve and forms NaOH__chemical__ 2. An element is found which is a good conductor of electricity, is ductile, brittle and does not react with acid. Is this new element a metal, nonmetal or metalloid? metalloid 3. The current periodic table is arranged according to increasing____atomic number__. 4. Elements in the same vertical column are in the same group and have similar properties due to similar electron configurations. 5. An element is discovered which bonds to oxygen in a 1:1 ratio. Where would it be placed on the periodic table? ________group 2________ 6. Estimate the boiling point of Kr if the boiling point of argon is -186°C and xenon -112°C. (-186+-112)/2 = -149°C 7. Give the characteristics of each group and label the periodic table with their correct positions: Alkali metals alkaline earth metals noble gases Periods Halogens transitional metals lanthanide and actinide metals Groups or families Group 1 = alkali metals (+1), highly reactive Group 2 = alkaline metals (+2) , highly reactive but less reactive than group 1 D block = transition metals (varied charges), strong color (pigments) Group 7 = halogens, highly reactive Group 8 = noble gases, unreactive Top row of inner transition metals = lanthanide series Bottom row of “ “ “ = actinide series Periods = horizontal Groups/families = vertical 8.) Balance Equations: _2_H2 + __O2 2__H2O 9.) Define Law of Conservation of Matter Matter can be neither created or destroyed during a chemical reaction. -
Semester –I Chapter 4: Redox Titrations
Semester –I Chapter 4: Redox Titrations SHREE H. N. SHUKLA INSTITUTE OF PHARMACEUTICAL EDUCATION AND RESEARCH B.PHRAM (SEMESTER –I) SUBJECT NAME: PHARMACEUTICAL ANALYSIS -I SUBJECT CODE: BP102TP CHAPTER 4: REDOX TITRATIONS H.N. Shukla Institute of Pharmaceutical Education and Research Page 1 Semester –I Chapter 4: Redox Titrations Content Redox titrations: (a) Concepts of oxidation and reduction (b) Types of redox titrations (Principles and applications) Cerimetry, Iodimetry, Iodometry, Bromatometry, Dichrometry, Titration with potassium iodate INTRODUCTION Concept of oxidation and reduction As discussed before, in titrimetric analysis we can find out the quantity of pure component based on measurement of volume of standard solution that reacts completely with the analyte. This measurement of standard solution can be possible in different reactions, and if the reaction involved in this measurement is oxidation-reduction reaction, that method is called ns "oxidation reduction titration" or "Redox titration. In Redox titration oxidation & Reduction reaction occurs simultaneously. Oxidation Combination of the substance with oxygen is termed as oxidation. C (s) + O2 (g) CO2 (g) Removal of Hydrogen H2S + O S + H2O Loss of electron(s) is known as oxidation. By loosing electron positive valency of element increases and negative valency of element decreases. Fe2+ Fe3+ + e- Increase in oxidation number Reduction Removal of Oxygen from substance CuO + 2H Cu + H2O Additon of Hydrogen C2H2 + 2H C2H4 Gain of electron, by taking on electron positive valency is decreased and negative valency is increased. Fe3+ + e- Fe2+ Decrease in Oxidation number. H.N. Shukla Institute of Pharmaceutical Education and Research Page 2 Semester –I Chapter 4: Redox Titrations Oxidation-Reduction Reaction Oxidation-reduction reactions are the chemical processes in which a change in the valency of reacting elements or ions takes place. -
20 More About Oxidation–Reduction Reactions
More About 20 Oxidation–Reduction Reactions OOC n important group of organic reactions consists of those that O A involve the transfer of electrons C from one molecule to another. Organic chemists H OH use these reactions—called oxidation–reduction reactions or redox reactions—to synthesize a large O variety of compounds. Redox reactions are also important C in biological systems because many of these reactions produce HH energy. You have seen a number of oxidation and reduction reactions in other chapters, but discussing them as a group will give you the opportunity to CH3OH compare them. In an oxidation–reduction reaction, one compound loses electrons and one com- pound gains electrons. The compound that loses electrons is oxidized, and the one that gains electrons is reduced. One way to remember the difference between oxidation and reduction is with the phrase “LEO the lion says GER”: Loss of Electrons is Oxi- dation; Gain of Electrons is Reduction. The following is an example of an oxidation–reduction reaction involving inorganic reagents: Cu+ + Fe3+ ¡ Cu2+ + Fe2+ In this reaction,Cu+ loses an electron, so Cu+ is oxidized. Fe3+ gains an electron, so Fe3+ is reduced. The reaction demonstrates two important points about oxidation– reduction reactions. First, oxidation is always coupled with reduction. In other words, a compound cannot gain electrons (be reduced) unless another compound in the reaction simultaneously loses electrons (is oxidized). Second, the compound that is oxidized (Cu+) is called the reducing agent because it loses the electrons that are used to reduce the other compound (Fe3+). Similarly, the compound that is reduced (Fe3+) is called the oxidizing agent because it gains the electrons given up by the other compound (Cu+) when it is oxidized. -
Chemistry 120: Experiment 1
Chemistry 120: Experiment 1 Preparation of a Standard Sodium Hydroxide Solution and Titration of Hydrochloric Acid In this experiment, we prepare solutions of NaOH and HCl which will be used in later experiments. We will require knowledge of the exact concentration of the two solutions, but it is not convenient either to weigh out solid NaOH or to measure out concentrated HCl. We do not know the composition of these materials well enough to obtain accurate numbers for our solutions by weighing them out. Instead, we take another approach. We will use the primary standard acid, potassium hydrogen phthalate, to make an acid solution containing a known amount of acid. The composition and purity of this acid is very well known, and we can accurately determine the amount of potassium hydrogen phthalate by weighing a sample. We can titrate this solid acid, after dissolving it in water, with our NaOH solution to accurately determine the NaOH concentration, as discussed below. This standardizes the NaOH solution against our primary standard. Then, with our standardized NaOH solution, we can titrate the HCl solution and accurately determine the HCl concentration. Thus, the concentrations determined for the NaOH and HCl solutions ultimately depend on the weight of our primary standard taken and the volumes of the solutions needed to react. Because the NaOH and HCl will be used to analyze other materials in future weeks, it is very important to determine their concentrations as carefully as possible. This suggests that careful weighing of the potassium hydrogen phthalate is very important. The presence of carbon dioxide is one reason why we cannot weigh out pure NaOH and use it as a primary standard. -
Hydrogen Peroxide Cas #7722-84-1
HYDROGEN PEROXIDE CAS #7722-84-1 Division of Toxicology ToxFAQsTM April 2002 This fact sheet answers the most frequently asked health questions (FAQs) about hydrogen peroxicde. For more information, call the ATSDR Information Center at 1-888-422-8737. This fact sheet is one in a series of summaries about hazardous substances and their health effects. It is important you understand this information because this substance may harm you. The effects of exposure to any hazardous substance depend on the dose, the duration, how you are exposed, personal traits and habits, and whether other chemicals are present. HIGHLIGHTS: Hydrogen peroxide is a manufactured chemical, although small amounts of hydrogen peroxide gas may occur naturally in the air. Low exposure may occur from use at home; higher exposures may occur from industrial use. Exposure to hydrogen peroxide can cause irritation of the eyes, throat, respiratory airway, and skin. Drinking concentrated liquid can cause mild to severe gastrointestinal effects. This substance has been found in at least 18 of the 1,585 National Priorities List sites identified by the Environmental Protection Agency (EPA). What is hydrogen peroxide? ‘ If released to soil, hydrogen peroxide will be broken down Hydrogen peroxide is a colorless liquid at room temperature by reacting with other compounds. with a bitter taste. Small amounts of gaseous hydrogen peroxide occur naturally in the air. Hydrogen peroxide is ‘ Hydrogen peroxide does not accumulate in the food chain. unstable, decomposing readily to oxygen and water with release of heat. Although nonflammable, it is a powerful How might I be exposed to hydrogen peroxide? oxidizing agent that can cause spontaneous combustion when it comes in contact with organic material. -
Chapter 2 Web Text Box 4 Hocl, an Acid and an Oxidizing Agent
Chapter 2 Web Text Box 4 HOCl, an acid and an oxidizing agent Chlorine bleach is a solution of sodium hypochlorite, NaOCl. This is an ionic compound and in water exists as Na+ and OCl- ions. Hypochlorite is the deprotonated form of hypochlorous acid HOCl, which is a very weak acid: its pKa is 7.53. Thus in the NaOCl solution some of the hypochlorite ions grab an H+ from water, leaving OH- behind. The result is that the solution is alkaline: usually about pH 11, although more concentrated solutions have an even higher pH. You should be able to calculate what fraction of the total hypochlorite is protonated at pH 11: check that you can! Try the calculation yourself, then check the answer in the box below! The pKa of hypochlorous acid HOCl is 7.53. What percentage of the total hypochlorite is protonated at pH 11.0; that is, calculate the value of 100 x [HOCl] / ( [HOCl] + [OCl-] )? Although HOCl is a very weak acid the hypochlorous ion is a strong oxidizing agent and will readily give up the oxygen atom leaving a simple chloride ion Cl-. One of the chemical groups that it attacks is the –SH side group on the amino acid cysteine. Two cysteine side chains are oxidized and form a disulfide bond: Chlorine bleach: an illustration of acid/base and oxidation/reduction reactions The cysteines have been oxidized because they have lost hydrogen atoms. Notice the distinction between deprotonation, the loss of H+, which is what we see in the reaction - + HOCl + H2O → OCl + H3O and the loss of complete hydrogen atoms, which is what has happened to the cysteines. -
Chemical Redox Agents for Organometallic Chemistry
Chem. Rev. 1996, 96, 877−910 877 Chemical Redox Agents for Organometallic Chemistry Neil G. Connelly*,† and William E. Geiger*,‡ School of Chemistry, University of Bristol, U.K., and Department of Chemistry, University of Vermont, Burlington, Vermont 05405-0125 Received October 3, 1995 (Revised Manuscript Received January 9, 1996) Contents I. Introduction 877 A. Scope of the Review 877 B. Benefits of Redox Agents: Comparison with 878 Electrochemical Methods 1. Advantages of Chemical Redox Agents 878 2. Disadvantages of Chemical Redox Agents 879 C. Potentials in Nonaqueous Solvents 879 D. Reversible vs Irreversible ET Reagents 879 E. Categorization of Reagent Strength 881 II. Oxidants 881 A. Inorganic 881 1. Metal and Metal Complex Oxidants 881 2. Main Group Oxidants 887 B. Organic 891 The authors (Bill Geiger, left; Neil Connelly, right) have been at the forefront of organometallic electrochemistry for more than 20 years and have had 1. Radical Cations 891 a long-standing and fruitful collaboration. 2. Carbocations 893 3. Cyanocarbons and Related Electron-Rich 894 Neil Connelly took his B.Sc. (1966) and Ph.D. (1969, under the direction Compounds of Jon McCleverty) degrees at the University of Sheffield, U.K. Post- 4. Quinones 895 doctoral work at the Universities of Wisconsin (with Lawrence F. Dahl) 5. Other Organic Oxidants 896 and Cambridge (with Brian Johnson and Jack Lewis) was followed by an appointment at the University of Bristol (Lectureship, 1971; D.Sc. degree, III. Reductants 896 1973; Readership 1975). His research interests are centered on synthetic A. Inorganic 896 and structural studies of redox-active organometallic and coordination 1. -
Redox Reactions Is
Chapter 10 OXIDATION-REDUCTION REACTIONS Oxidation – reduction reactions are those involving the transfer of electrons from one substance to another (no bonding formed or broken). Example: Fe 3+ + e- çè Fe 2+ Protons (H+) are often involved in these reactions also. Another example of redox reactions is: - + H2O2 + 2e + 2H 2H2O Rules for the assigning of oxidation numbers 1. All species in their elemental form are given the oxidatio435n number of zero. 2. All monoatomic ions have the same oxidation number as the charge on the ion. e.g. Mg 2+ has the oxidation number of +2. 3. All combined hydrogen has an oxidation number of +1 (except metal hydrides where its oxidation number is -1). 4. All combined oxygen has an oxidation number of -2 (except peroxides where the oxidation number is -1). 5. In polyatomic species, the sum of the oxidation numbers of the element in the ion equals the charge on that species (we can use this to find the oxidation number of elements in polyatomic species). A. Source of electrons in soils. Electrons dTPSSo not flow around by themselves but they m ust be provided by some sources . In soils, the main source of electrons is carbon atoms of organic matter because carbon has a wide range of oxidation states. Example: CH4 + 2O2 2H2O + CO2 Ox. # (-4) Ox. # (+4) - The reaction (CH4 ® CO2) releases 8e Other common sources of e – are nitrogen and sulfur atoms because they can also have several oxidation states. The availability of electrons usually controls the oxidation/reduction reactions and this availability is expressed as redox potentials. -
Year 12 ATAR Chemistry Unit 3: Acid Base Titrations
PROCESS TO EXCLUDE A STUDENT Year 12 ATAR Chemistry Unit 3: Acid Base Titrations Acids and Bases Except where indicated, this content © Department of Education Western Australia 2020 and released under Creative Commons CC BY NC Before re-purposing any third party content in this resource refer to the owner of that content for permission. https://creativecommons.org/licenses/by-nc/4.0/ Year 12 | ATAR | Chemistry | | Acid Base Titrations | © Department of Education WA 2020 Year 12 ATAR Chemistry Acids and Bases Chemistry ATAR Year 12 Unit 3 Acid Base Titrations Syllabus Points Covered This unit of work covers volumetric analysis used in acid-base titrations. Data obtained during titration can be used to calculate information about unknown solutions. Volumetric analysis methods involving acid-base reactions rely on the identification of an equivalence point by measuring the associated change in pH, using appropriate acid-base indicators or pH meters, to reveal an observable end point. Read the information below: Volumetric Analysis Acid-base reactions can be used to determine information about unknown solutions. An example could be the concentration of acetic (ethanoic) acid in a sample of vinegar or the acidity of a sample of biodiesel. In volumetric analysis, in order to work out the concentration of the acid in the solution, a chemist will react the acid with an alkaline solution. If the chemist knows the concentration of the alkali, and measures the volume of the alkali used to neutralise all of the acid, the chemist can calculate the number of moles of alkali used. Once this is known, the unknown number of moles of the acid can be worked out.