All India Senior Secondary Examination Examination 2010 - 2011 An investigatory project on Chemistry PROJECT: TO STUDY THE PRESENCE OF OXALATE ION CONTENT IN GUAVA FRUIT AT DIFFERENT STAGES OF RIPENING. Submitted by: ANUKRITI SHARMA Class- XII – A (sci.) Roll no: 06 Air force school Chakeri ‚ Kanpur(up) CERTIFICATE This is to certify that ANUKRITI SHARMA has satisfactorily completed the project in CHEMISTRY on ‘OXALATE ION´ prescribed by the AISSCE course in this school in
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Melissa Benning Introduction The purpose of the coordination complex lab is to determine the absorbance spectra of complexes based on their color. Every complex has its own color which results from the wavelengths of white light it reflects. The complexes will be compared by the color each reflects and by the energy of the waves each absorbs. The purity of the synthesized complex will also be found. Procedure Part I: Preparation of the Complex A sample of copper sulfate pentahydrate (6.285g)
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Grayland Martin Period 5 9/4/12 Laboratory 2 Report: Enzyme Catakysis 1. Title • The effect that temperature‚ pH‚ time‚ enzyme concentration‚ and substrate concentration has on Enzyme Catalysis. 2. Abstract • Assess the general functions and activities of enzymes. Analyze the relationship between the structure and function of enzymes. Understand the concept of initial reaction rates of enzymes. Change the temperature‚ pH‚ enzyme concentration‚ substrate
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(CH3C6H5) (3ml) - Potassium Permanganate solution (KMnO4) .01 mol L-1 (4ml) - Sulfuric Acid (H2SO4) 2mol L-1 (2ml) - Bromine Water (Br2) (5ml) Procedure: Reaction of hydrocarbons with acidified permanganate: 1) Into three separate‚ labeled test tubes place 1 ml of cyclohexane‚ cyclohexene and toluene respectively. 2) In a separate test tube add 4 ml of 0.01mol L-1 KMnO4 to 2 ml of 2mol L-1 H2SO4 3) Add 1 ml of this acidified KMnO4 solution to each of the test tubes containing the hydrocarbons
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EQUIPMENT The materials required for this experiment include the following: • 2-50ml Burets • 60 mL of 0.755M H2C2O4 • 60 mL of 0.13M KMnO4 • Thermometer • Stirring rod • Hot Plate • 6- Clean test tubes • 2 Buret clamps • Timer PROCEDURE Two burets were rinsed‚ labeled‚ and filled with one having 0.755M H2C2O4 and the other with 0.13M KMnO4. Exact readings and concentrations of both burets were recorded on the data sheets. For determination 1‚ 5 mL of H2C2O4 was dispensed from
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CuSO4·5H2O(s) → CuSO4(s) + 5H2O(g) | 8. Red litmus paper changes to blue color; white precipitate. | double-displacement reaction | 2 Na2O2(s) + 2 H2O(l) = 4 NaOH(aq) + O2(g)↑ | 9. purple KMnO4 changes to yellow brown | double-displacement reaction | FeSo4(aq) + KMnO4 (aq) = KMnSo4 + FeO4 ( 8 H2SO4 + 2 KMnO4 + 10 FeSO4 = 5 Fe2(SO4 )3 + 2 MnSO4 + K2SO4 + 8H2O) | 10. Blue litmus changes to red; base becomes acid. | acid-base reactions | Na2CO3 +2HCl -> 2NaCl + H2O + CO2 | TYPES OF
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entire tablet has a mass of 0.115g. Calculate the mass percent of vitamin D in the tablet. 0.022% vitamin D Example 3: A sample of potassium permanganate (KMnO4) is known to contain some impurities. It is found that K+ makes up 19.24% of the entire mass of the impure sample. All of the K+ comes from the KMnO4 compound. Find the mass percent of KMnO4 in the sample. 77.77% Molecular & Empirical Formulas Molecular Formula Chemical formulas that provide the actual number of each type of atom in a molecule
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vigorously‚ NOTE time required (less than 10m mins only) to form an emulsion or separate layers. Oxidation (Confirms if alcohol is oxidizable: presence of H in C-OH bond) Reagent: Neutral KMnO4 Observation: purple color ( brown ppt Procedure: 5 drops test sample in test tube+ 1 drop dilute neutral KMnO4‚ if NO DECOLORIZATION warm mixture. Primary Alcohol( carboxylic acid Secondary Alcohol( ketones Tertiary( none Phenols Reaction with bromine/water (Confirms if phenol compound) Reagent:
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Experiments 4A-C: Synthesis and Component Analysis of an Iron (III) Oxalate Complex My Name TA‚ Section B## Work Performed on 10/23‚ 10/30‚ & 11/4‚ 200# Report due Tuesday‚ November ##‚ 200# 1. Abstract This experiment initially involved the synthesis of an iron (III) oxalate complex with the general formula Kw[Fex(C2O4)y]·zH2O. The variables x‚ y‚ and z were determined through the duration of the entire experiment. From 1.2000g of Fe(NH4)2(SO4)2 were synthesized 1.1###g of K3[FeIII(C2O4)3]·3H2O
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1.Mg + HCl ( MgCl2 + H2 2.Fe + V2O3 ( Fe2O3 + VO 3.KMnO4 + KNO2 + H2SO4 ( MnSO4 + H2O + KNO3 + K2SO4 4.K2Cr2O7 + SnCl2 + HCl ( CrCl3 + SnCl4 + KCl + H2O 5.KMnO4 + NaCl + H2SO4 ( Cl2 + K2SO4 + MnSO4 + H2O + Na2SO4 6.K2Cr2O7 + H2O + S ( SO2 + KOH + Cr2O3 7.KClO3 + C12H22O11 ( KCl + H2O + CO2 8.H2C2O4 + K2MnO4 ( CO2 + K2O + Mn2O3 + H2O 9.Mn(NO3) 2 + NaBiO3 + HNO3 ( HMnO4 + Bi(NO3) 3 + NaNO3 + H2O 10.H2C2O4 + KMnO4 ( CO2 + K2O + Mn2O3 + H2O Oxidation Reduction
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