ClO- (aq) + 2I- (aq) + 2H+ ---> I2 (aq) + Cl- (aq) + H2O and I2 (aq) + 2S2O3-2 (aq) ---> 2I- (aq) + S4O6-2 (aq). KI is added to dilute bleach in which the hypochlorite will reduce I- to form I2. Once this solution is created‚ it will be titrated with the sodium thisulfate solution from part 1 to find the mass percent of sodium hypochlorite. Balanced equations are very important in this experiment because‚ if the equation is balanced‚ mole ratios between reactions can be found. If the equations
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conducted. A change in the strip to a deep blue color would signal an excess of sodium hypochlorite reagent present. An excess is the reagent symbolizes the end of the reaction because there is no longer any reactant left to consume reagent. After the reaction was deemed completed‚ the product was isolated and purified by ether extraction‚ aqueous extraction and evaporation. To determine how sodium hypochlorite acts as an oxidizing agent‚ the starting diol and final product were characterized through
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Catalase and Catalyst Catalyst is a chemical‚ which can break down hydrogen peroxide to water and oxygen. Catalase is a common enzyme that is found in almost all living organisms exposed to oxygen. Hydrogen Peroxide and Sodium Hypochlorite Hydrogen peroxide is in bleaches too‚ but only the mild ones‚ which is the non-chlorine bleaches. Since only hydrogen peroxide isn’t very strong‚ other products usually use other chemicals to make the reaction and results more effective‚ for
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difference between mineral oil and water using a hand lens. * Making iodine in water- We added one drop of potassium iodide and sodium hypochlorite (bleach) then mixed the two together producing iodine. * Making iodine in oil-We added two drops of mineral oil‚ one drop of water on the mineral oil‚ then added one drop of potassium iodide and sodium hypochlorite. Producing Iodine. Results: In class we conducted four experiments on
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Green Oxidation of Borneol to Camphor Abstract: This lab converted borneol to camphor using a green oxidation. Sodium hypochlorite was used instead of the less “green” Jones reagent. Borneol was mixed with glacial acetic acid and oxidized with sodium hypochlorite to make crude camphor. The crude camphor was purified by sublimation. The final product was characterized by obtaining a melting point and inferred spectroscopy. The experiment was carried out to see if bleach could oxidize borneol
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Paragraph 1 In experiment 2‚ the statistical analysis of data collected showed that Clorox Household Cleaner was not significantly different than the Clorox Toilet Bowl cleaner. This is due to the fact our calculated P-value was 11.45%‚ which is larger than the 5% maximum allowed to us to be able to support the alternative hypothesis. This indicates there was not support for our alternative hypothesis‚ causing us to reject it. In doing so‚ we had to accept our null hypothesis. Our Null hypothesis
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reduction‚ or in the addition of a functional group. In this lab we will examine the stereoselectivity of the reduction of 4-tert-butylcyclohexanone (Figure 1) using sodium borohydride (Figure 2). In the first week of this lab we will use sodium hypochlorite (Figure 3) to oxidize (Mechanism: Figure 6) commercial 4-tert-butylcyclohexanol‚ synthesizing 4-tert-butylcyclohexanone and using IR analysis to confirm that our oxidation was successful. In the second week of this lab we will use sodium borohydride
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Introduction The purpose of this lab was to determine the mole ratios of the reactants hypochlorite ion (OCI ) and thiosulfate (S O ) when reacted in a chemical reaction. A chemical equation gives the mole ratios of the reactants and products involved in the chemical reaction. When some formulas of the products are not known‚ experimental measurements can be made to determine those ratios. During this reaction‚ hypochlorite ions oxidize the thiosulfate ions according to the unbalanced and incomplete reaction
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4th form Chemistry questionnaire 1. All of the following structures show the same molecule‚ except one. Which structure is different? H H H H A) H -- C -- C -- C --- C -- H B) CH3 CH2 CH2 CH3 H H H H H H -- C -- H CH3 C) H H D)
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Fluorine Properties - What are the Physical Properties of Fluorine? What are the Physical Properties of Fluorine? The Physical properties of Fluorine are the characteristics that can be observed withoutchanging the substance into another substance. Physical properties are usually those that can be observed using our senses such as color‚ luster‚ freezing point‚ boiling point‚ melting point‚ density‚ hardness and odor. The Physical Properties of Fluorine are as follows: What are the Physical
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