ratios that govern the disappearance of reactants and the appearance of products. Knowing the mole ratios in a balanced chemical equation is essential to solving stoichiometry problems. General Chemistry 1 Lab Acetone Copper wire 3
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determine the solvent wherein the tannins can be best dissolved using Distilled water‚ Alcohol‚ Ether and Acetone. Table 3 Results of Solubility test Distilled water Soluble Alcohol Insoluble Ether Insoluble Acetone Insoluble The table 3 shows the result of solubility test conducted using Otaheitte Gooseberry leaves. Tannins are soluble in water and insoluble in alcohol‚ ether and acetone (organic solvents). 2.3 Melting Point 3. Chemical Properties of Tannins Expected Actual a). Ferric
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INTRODUCTION 1.1 Background of the Experiment Mass density describes how heavy an object is. Defined by the Greek letter ρ‚ read as rho‚ density is a basic yet important physical property of matter. For a bulk body without accounting its existing pores and voids‚ density is represented by the ratio of its mass and volume. It is given by the equation ρ= massvolume 1. The SI unit of density is kg/m3. However‚ its CGS units‚ g/cm3 or g/ mL‚ are the most commonly used ones in the laboratory. The
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of hair samples 1. Stainless Steel Scissors 2. Plastic bags 3. Gloves 1. Hot water 2. Ethanol Washing the hair samples 1. Forceps 2. 100 ml beakers 3. Electronic weighing balance 4. Magnetic stirrer 5. Magnets 6. Filter paper 1. Diethyl Ether 2. Acetone 3. Deionised water 4. pH 6 Shampoo Digestion of hair
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In this lab‚ we extracted spinach pigments‚ and analyzed what colors of light these pigments absorb. By using TLC plate‚ hexane and acetone‚ I separated the pigments of spinach‚ and discovered that the main pigments were green and yellow. This works because with different polarities‚ pigments move at different rates. Hexane and acetone were also used to separate chlorophyll and carotene from spinach. Since they are polar‚ they can separate organic and inorganic things. From the experiment‚ I know
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colligative properties and to use them to determine the molar mass of a substance. Materials and chemicals: 800mL beaker balance weighing paper Thermometer 400mL beaker wire stirrer ring stand unknown solid 15x150mm test tube clamp watch acetone Ice cyclohexane sodium chloride Lab Safety: Wear protective googles‚ apron‚ and gloves. Procedures: Prepare ice/salt/water bath Place 50g of solid NaCl in a 400mL beaker and add just enough water to dissolve the salt. Fill an 800mL beaker
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1. The partial molar volumes of acetone and chloroform are 74.16 cm3 mol-1 and 80.23 cm3 mol-1 respectively. Calculate the volume of a mixture containing 25.00 moles of acetone and 75.00 moles of chloroform. 2. Acetone has a molar mass of 58.1 g mol-1 and a density of 0.787 g cm-3. Chloroform has a molar mass of 119.4 g mol-1 and a density of 1.499 g cm-3. Estimate the volume of the above mixture using this information. 3. Calculate the molal freezing point depression constant Kf for
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Contents Part One Investigation of a Workplace Incident Investigation Policy PURPOSE The purpose of this policy is to ensure that: all hazards‚ near misses and injuries are reported to management. investigations are carried out in a sensible manner with preventative actions identified and put into practice in due course. follow up monitoring is undertaken to ensure hazards are removed or reduced as much as possible and that no new hazards will be introduced to the workplace
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study the test of identification of alkyl halide Chemicals and Apparatus: ~18.0 g 1-butanol‚ ~20.0 g sodium bromide‚ 15 ml of concentrated sulfuric acid‚ anhydrous magnesium sulfate‚ ~10 ml of 5% aqueous sodium bicarbonate‚ ~1 ml of sodium iodide – acetone reagent‚ 1 ml of bromine in chloroform‚ 1 piece of 100 cm3 round-bottomed flask‚ 1 piece of 50 cm3 of beaker‚ 1 piece of 50 cm3 of conical flask‚ 1 piece of 250 cm3 of separating funnel‚ 1 piece of 10 cm3 of measuring cylinder‚ 1 piece of electronic
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the 3 tubes of solution that we received were individually tested to determine its composition. Next‚ we created a solution of tube A mixed with acetone and tested it through gas chromatography. The reason this was done‚ is because if tube A really did contain acetone the tallest peak on the gas chromatography results would be at the position for acetone but only
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