compound CCl4 using the Stock system. |a. |carbon(IV) chloride |c. |carbon chloride | |b. |carbon tetrachloride |d. |carbon hypochlorite | ____ 31. Name the compound H2O using the Stock
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Water Technology Hardness of Water: Natural waters containing large quantities of dissolved salts of Calcium (Ca) & Magnesium (Mg) is called hard water. It is a characteristic of preventing lather formation of water with soap. Ca2+ & Mg2+ ions react with soaps which are salts of fatty acids (stearic or palmitic acid) to give insoluble scums or precipitates of calcium or magnesium stearate or palmitate. 2C17H35COO- + Ca2+ → (C17H35COO)2 Ca (scum) 2C17H35COO- + Mg2+ → (C17H35COO)2
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sodium hypochlorite‚ NaClO (sometimes written NaOCl). Commercial bleaches are created by bubbling chlorine gas into a sodium hydroxide solution (remember this from your “funky redox rxns”?). Some of the chlorine is oxidized to the hypochlorite ion‚ ClO- and some is reduced to the chloride ion‚ Cl- (a disproportionation reaction). The solution remains strongly basic. The chemical equation for the process is: Cl2(g) + 2OH- (aq) ---> ClO- (aq) + Cl- (aq) + H2O (l) The amount of hypochlorite ion present
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perform a redox titration. To determine the amount of hypochlorite ion present in commercial bleach. Introduction Many commercial products‚ such as bleaches and hair coloring agents‚ contain oxidizing agents. The most common oxidizing agent in bleaches is sodium hypochlorite‚ NaClO (sometimes written NaOCl). Commercial bleaches are made by bubbling chlorine gas into a sodium hydroxide solution. Some of the chlorine is oxidized to the hypochlorite ion‚ ClO-‚ and some is reduced to the chloride ion
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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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