! ! To review oxidation-reduction reactions and their stoichiometry. To learn the concept and technique of redox titration. To determine the percent (m/v) of an active ingredient‚ sodium hypochlorite (NaOCl)‚ in a commercial bleaching agent. B. Theoretical Background Whereas acid-base reactions involve the transfer of a proton‚ oxidation-reduction or redox reactions involve the transfer of electrons from one substance to another‚ resulting in changes in oxidation numbers of two or more
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CHEMISTRY REVISION GUIDE for IGCSE Coordinated Science This revision guide is designed to help you study for the chemistry part of the IGCSE Coordinated Science course. The guide contains everything that the syllabus says you need you need to know‚ and nothing extra. The material that is only covered in the supplementary part of the course (which can be ignored by core candidates) is highlighted in dashed boxes: Some very useful websites to help you further your understanding include: •http://www
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Writing Half Reaction and Net Ionic Equation Going back to our first concept or topic‚ we’ve learn how to identify the Oxidizing and Reducing agent and the Oxidation as well as the Reduction. In this part of the Redox reaction or in this step‚ it is very important that you already know the Oxidizing and Reducing agent for us to find the half reaction. In this step or part‚ we will also learn how to balance using the addition of electrons in both sides if necessary. After this step we can now write
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this reaction are the dissociation of Cu(OH)2(s)‚ redox of Cu2+ and Zn‚ and precipitation of Zn(OH)2‚ leading to an overall reaction of Cu(OH)2(s) + Zn(s) ⇌ Zn(OH)2(s) + Cu(s). When 6.0 M HNO3 was added to the fourth test tube‚ the precipitate disappeared. The H+ ions from the complete dissociation of HNO3 neutralize the OH- ions. This results to the shifting of the system to the right. The addition of 6.0 M NH3 in the fifth test tube caused the formation of the deep blue [Cu(NH3)4]2+ complex.
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according to Table 1. Table 1. The reagents to be added for Cu(OH)2(s) equilibrium Test tube | Reagent to be added | 1 | 2.0 mL distilled water | 2 | 2.0 mL 1.0 M H2C2O4 solution | 3 | 2.0 mL water + pinch of Zn dust | 4 | 2.0 mL of 1.0 HNO3 | 5 | 2.0 mL of 6.0 M NH3 | 6 | 2.0 mL of 0.10 M Na3PO4 | 7 | 2.0 mL of 0.10 M Cu(NO3)2 | Each mixture was shaken thoroughly. The observations‚ specifically‚ the change in colour or amount of precipitate for each test tube are shown in Table
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colorless‚ the end point in the titrations using potassium permanganate as the titrant can be taken as the first permanent pink color that appears in the solution. This titration involves the oxidation of Fe2+ ions to Fe3+ ions by the permanganate ion‚ and is carried out in sulfuric acid solution to prevent the air oxidation of the ferrous ion. The end point of the titration is sharpened markedly if phosphoric acid is present. The reason being the Fe3+ ion by itself has a yellow color that can partly mask
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Report Introduction Mummification is an ancient Egyptian method which is a natural or deliberate process intended to dehydrate the body to preserve it. They done this because they believed that if a body was left to rot then it would destroy their soul‚ so they believed that the body needed to be intact to serve as host for the soul. So they preserved bodies so they could use them in the afterlife‚ where the Egyptians believed they would make a journey to another life. To start to mummify a body
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reaction between the Ferric Ion (Fe3+) and the Thiocyanate Ion (SCN-) which produces Ferric Thiocyanate Ion (Fe(SCN)2+): Fe3+(aq) + SCN-(aq) Fe(SCN)2 (aq) MATERIALS 1. Cuvette 2. Pipet 3. Genesys 20 spectrophotometer 4. Dilute nitric acid‚ HNO3 5. Iron Nitrate‚ Fe(NO3)3 6 . Potassium thiocyanate‚ KSCN 7. Thermometer 8. Tissues 9.Protective devices PROCEDURE OR METHODS In Part A of the lab‚ I prepared six solutions – including a reference solution (known concentration)
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force. Background Redox (reduction-oxidation) reactions include all chemical reactions in which atoms have their oxidation state changed. So‚ when a metal and a nonmetal react‚ there is an ionic bond formed‚ which means one of them loses electrons while the other gains them. Since this reaction involves the exchange of electrons it is termed as a redox reaction. The oxidation states in a metal- nonmetal are simple to determine because they are given oxidation states similar to their charges. However
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← Muon ← Is created when a neutrino collides and combines with an H2O proton (weak force) ← Creates blue light ← High energy; travels faster than the speed of light (in water) ← Neutrino ← Type of particle: Lepton (like electrons and muons) ← Most abundant particle in the universe ▪ 1016 neutrinos are passing through your body at any point in time ← Theoretically discovered by Wolfgang Pauli (1930); actually discovered in 1955 ← Produced during nuclear reaction or changes
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