Malachite Synthesis Lab Report
177 Words1 Pages
2CuSO4*5H2O(aq) + 2Na2CO3(aq) CuCO3Cu(OH)2(s) + 2Na2SO4(aq) + CO2(g) + 9H2O(l)
Based on this chemical equation, two moles of aqueous hydrated copper (II) sulfate reacted with aqueous sodium carbonate, a precipitate of copper (II) carbonate hydroxide was formed along with aqueous sodium sulfate, gaseous carbon dioxide, and liquid water. The copper (II) carbonate hydroxide precipitate is also the malachite that was obtained from the solution. It was known that a chemical reaction was occurring when the copper (II) sulfate solution was mixed in with the sodium carbonate based on the fact that the color of the solution changed from blue to light blue and the solution frothed. The malachite
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Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.
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Cadet Eric Wiggins Date: 18 September 2014 Course Name: Chem 100 Instructor: Captain Zuniga Section: M3A Identification of a Copper Mineral Intro Minerals are elements or compounds that are created in the Earth by geological processes. The method of isolating metals in a compound mineral is normally conducted through two processes.
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6.7, 6.8 Synthesis, Decomposition, and Displacement Reactions Kelly Mok SNC2DE-A Mr. Cox Partner: Nidhi S. Lab performed: September 18 & 19, 2014 Due: September 26, 2014 Purpose The purpose of this experiment is to observe and compare synthesis, decomposition, single displacement and double displacement reactions and the physical and chemical reactions that occur as a result. Hypothesis
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The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
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In order to separate KNO3 and CuSO4, which are both soluble in water, recrystallization was used. The reason the two components can be separated through recrystallization is because of the temperature dependence of solubility, KNO3 is much more soluble in hot water and insoluble in cold water while CuSO4 is only slightly more soluble in hot water. When the filtrate was heated the solution was saturated with KNO3 but when the system was cooled, the KNO3 became insoluble and pure crystals reformed while CuSO4 stayed dissolved in the
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ABSORPTION, DISTRIBUTION AND METABOLISM: Eucalyptol is quickly absorbed from the gastrointestinal tract. It is lipid soluble and absorption is enhanced in the presence of milk. Inhalation of the liquid is directly toxic to the lungs; however there is no data suggesting systemic absorption via lungs 8. Eucalyptol undergoes oxidation in vivo with the formation of hydroxycineole which is Excreted as glucuronide 9.
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In this reaction NaOH was added to the Cu(NO3)2. The solution developed a precipitate which made the clear solution become cloudy and uniform in color (blue). The physical color change was demonstrated through the formation of the precipitate. The third step was the formation of CuO. In this reaction, the Cu(OH)2 product was heated on a hot plate and stirred continuously until the solution became colorless and a dark precipitate formed.
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Balanced Chemical Equation: Cu(s) + 4HNO3(aq) —> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) Reaction 2: when sodium hydroxide (NaOH) is added to copper (II) nitrate (Cu(NO3)2), a double displacement reaction will occur. Copper and sodium will displace each other to create copper (II) hydroxide and sodium nitrate. Balanced Chemical Equation: Cu(NO3)2 (aq) + 2NaOH (aq) —> CuOH2 (s) + 2NaNO3 (aq) Reaction 3: When copper (II) hydroxide is heated, a decomposition reaction will occur. The reaction will decompose forming two compounds, Copper (II) oxide, and water. Balanced Chemical Equation: Cu(OH)2 (s) + Heat —> CuO (s)
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Observations During the gradual addition of acetic anhydride, the previous solution of aniline later acquired an oil-like layer floating on the surface. Once the mixture was swirled, the solution became cloudy and milky-yellow in colour. The charcoal that was added to the warm solution began clear up the solution. The oil-like droplets began to mix with the solution. Data and Calculations See Lab K report sheet that is attached.
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Add sodium carbonate (Na2CO3), to the calcium chloride you already have. This will make calcium carbonate ( CaCO3), according to the formula: Na2CO3 + CaCl2 -> CaCO3 + 2NaCl. Afterward, filter this solution to obtain the calcium carbonate. Finally, heat the calcium carbonate at 248 degrees Fahrenheit to dry it out. Heat the calcium carbonate to 1,832 degrees Fahrenheit to get CaO.
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Tertiary alkyl halides tend to give a mixture with both inverted and retained configurations at reaction centers. This is because this reaction proceeds through a stable carbocation intermediate and the carbon at the reaction center goes to sp2 hybridized state (planar geometry). The incoming nucleophile can attack from both sides of the plane and can give two products with retained and inverted configuration. If there is a partial interaction with the leaving group (nucleofuge) with carbocation there will be more product with inverted configuration and if there is no interaction with leaving group racemic mixture can be obtained. The rate of the reaction depends on the formation of a carbocation (which is the slow step) and there is one molecule
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Title : Determination of chemical formula of hydrate Aim To determine the chemical formula of hydrated Copper (II) sulphate, CuSO4 Research Background “When the chemical is heated the hydrate will convert to an anhydrous ionic compound (this means the water will leave it). The moles of H2O will be determined by assuming the amount of mass lost by heating is the mass of the evaporated H2O. The moles of the CuSO4 (the white substance after heating) can be calculated from the mass of the white crystals. Using the molar ratio of moles of CuSO4 to moles of H2O, one can determine the chemical formula of the hydrate.” Apparatus and materials Apparatus and Materials used Quantity Crucible and lid
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Metabolic engineered of biocatalyst: A solution for PLA based problems ABSTRACT Poly lactic acid(PLA) is a biodegradable polymer used in many biomedical as well as in packaging Applications. Conventionally, PLA is produced by two method which is direct condensation of lactic acid and ring opening polymerization. The polymer produced from these conventional methods produced polymer which have low molecular weight.
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Introduction: This preparation illustatrates the benzoylation of amino acid by Schotten Baumann reaction, the hippuric acid is precipitated upon acidifying the reaction mixture. Reaction: Procedure: Dissolve 2.5g of glycine in 25 ml of 10 % NaOH contained in a conical flask. Add 5.4g (4.5 ml) of benzoyl chloride in two proportions to the solutions. Stopper the flask and shake vigorously after each addition until all the chlorine has reacted.
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Following the procedures for the bulk catalysts, the solution was stirred and was air dried for 2 to 4 days. Air-dried solution underwent the same procedure as the bulk catalysts with a final calcination temperature of 800 oC. The samples were labelled as yMo/CZ, where y represents the wt% (5, 12 or 20) concentration of molybdenum metal (present as
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