lab is to standardize a solution of potassium permanganate by redox titration with a standard solution of iron (II) ions. A solution of oxalic acid is then titrated with the permanganate solution to determine the exact concentration of oxalic acid. Purpose: The purpose of the experiment was to use the permanganate ion‚ a strong oxidizing agent‚ in a titration in order to determine the concentration of a FeSO4 solution. Purple MnO4- ion from a standardized potassium permanganate solution was titrated
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standard solution of potassium permanganate. Success in this analysis requires careful preparation and attention to detail. Performing this experiment also provides practice at titrations. The overall reaction is: 8H+(aq) + MnO4-(aq) + 5e- Mn2+(aq) + 4H2O Theory: In acid solutions the permanganate ion undergoes reduction to manganese (2+) ion. Since the permanganate ion is violet and the manganese ion is colorless‚ the end point in the titrations using potassium permanganate as the titrant
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Period 1 11/7/13 Chapter 35 Discussion Background: Potassium permanaganate is widely used as an oxidizing agent in volumetric analysis. In acid solution‚ MnO4- ion undergoes reduction to Mn2+ this is the equation: 8H+(aq) + Mno4-(aq) + 5e- Mn2+(aq) + 4H2O Since the KMnO4 – ion is violet and the Mn2+ ion is nearly colorless‚ the end point titrations using KMnO4 as the titrant can be taken as the first pink color that appears in the solution (and stays without disappearing).
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Aim: To determine the rate law of chemical reactions Introduction: The aqueous solution of potassium peroxydisulphate can oxidize potassium iodide as follow: Equation: K S 0 (aq) + 2KI (aq)->2K S0 (aq)+I (aq) 2 2 8 2 4 2 KI(aq) +I (aq) -> KI (aq) 2 3 _________________________________________________ K S 0 (aq) +3KI(aq) -> 2K S0 (aq)+ KI (aq) 2 2 8 2 4 2 The rate law of this reaction can be represented as follow: Rate=k[S208 2-]^a [I-]^b When the concentration of peroxydisulphate ions
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Name : ……………………………………………………………….. Date Due : …………………………………………………………….. Year 12 80% A 70% B AS Level Chemistry 60% C 2008 – 2009 50% D 40% E Below U Questions on % Haloalkanes 2.8 32 1. Chloromethane can be prepared by a reaction between methane and chlorine in the presence of ultraviolet radiation. (i) Outline the mechanism for this reaction. .....................................................................................
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the end of the tube containing HCL with a large molecular weight. In agar-water gel test‚ using agar plate and agar-water gel‚ 2 different substrate were tested- potassium permanganate (KMnO4) and methylene blue (C16H18N3SCl). By dropping it on a agar plate‚ methylene blue has a slowest diffusion rate and large molecular weight than potassium permanganate. Thus‚ the greater the molecular weight‚ lesser the rate of diffusion. INTRODUCTION Diffusion is a passive transport. It is results
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of the beaker‚ and then topped. After the eluting solution has risen to within two centimeters of the top of the filter paper‚ the paper was removed from the beaker‚ dried‚ and was stained with a staining reagent solution containing potassium ferrocyanide and potassium iodide. This reagent forms colored precipitates or reaction products with many cations‚ including all of those used in this experiment. The distance of which the spots moved were determined by calculating the Rf value of each substance
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The sulfuric acid was added after the allotted time and acted as an inhibitor. The inhibitor left a mixture of the products and original hydrogen peroxide. Our titrant of potassium permanganate (KMNO4) shows through its purple color the remnants of the hydrogen peroxide‚ which we were able to record. Hypothesis: If we add potassium permanganate to our mixtures then those beakers that were given a longer duration to react will require less titrant because of the little amount of unreacted hydrogen peroxide
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Methods of Sample Preperation Initially the plates were rinsed with ethanol‚ then dried with lint0free tissues. Next 1-2 g of benzoic acid were transferred to a mortar and a pestle was then use to grind the sample. About 100-150 mg of oven dried potassium bromide were added into the mortar and mixed well and then grinded. Next a screw was attached to a bolt and tightened together to make a sample holder. Next another screw was attached to the bolt to fasten it. The sample holder was then mounted
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On what I have seen‚ the first experiment showed chemical reaction to be more specific‚ combustion. In the experiment the Potassium permanganate (KmnO4) was used as the oxidant‚ and obviously oil as the fuel. As the two were mixed they needed to release energy in form of heat‚ that’s where combustion occurs. I learn that Combustion is the sequence of exothermic chemical reactions between a fuel and an oxidant accompanied by the production of heat and conversion of chemical species. The release of
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