Extraction of Jathropa curcas Seed Fats and Oil and Identification and Characterization of Unknown Oil Jose G. Intano‚ Jr. and Niescee Eiscene Talaman University of the Philippines Visayas Miagao‚ Iloilo xdvm_apollo469@yahoo.com‚ messyisnessy@gmail.com Abstract The experiment had the objectives of extracting fats and oil from plant sample using 3:2 hexane-isopropanol solvent through Soxhlet method and of identifying and characterizing unknown oil sample using different chemical analyses
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Chapter 1: Measuring the amount of substance Analytical chemistry: science of chemical measurement. Its object is the generation‚ treatment and evaluation of signals from which information is obtained on the composition and structure of matter Measurement: process of obtaining the magnitude of a quantity Example: The amount of saturated fat in the sample is 3 g/serving. Quantity: attribute of a phenomenon that may be distinguished qualitatively and determined quantitatively Value: magnitude
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The first flask was placed under a buret. Finally we titrated the KHP by adding the base until the end point was reached‚ which was when it turned pink completely. We repeated this twice and then cleaned up. The procedure does not include very difficult math‚ however the calculations did. The harder math calculations included finding moles of the acid‚ moles of the base that was used to neutralize‚ and the molarity of the base. After all calculations‚ below is what we concluded. The molarity you
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tablets by titrating the solution with a base. Also determine whether the aspirin is a strong or weak acid according to the Bronsted- Lowry and Lewis theories and deduce the formula of the acid- base reaction. Independent Variable: The amount of base (NaOH) in moles that are needed to neutralize the solution. Dependent Variable: Percentage of aspirin (acetylsalicylic acid) found in each tablet. Materials: * Balance * 2 aspirin samples from different brands * 50 cm3 conical flask * 10.00cm3
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concentration of NaOH: Trial 1: .96g H C O 2 H ) Mol H C O 2H O= 126 g/mol = .0076 mol Mol of NaOH= (.0076 mol H C O 2H O) ( 2NaOH ) = .0152 mol 1 H C O 2H O M NaOH= 0.0152 mol NaOH = .530M NaOH 0.02870 L NaOH Trial 2: Mol H C O 2H O= 0.9g H C O 2 H O = .0075 mol 126 g/mol mol of NaOH= (0.0075mol H C O 2H O) ( 2NaOH ) = 0.0151 mol 1 H C O 2H O M of NaOH= 0.0151 mol NaOH = 0.522M
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HNO3 and H2SO4 have the same molarity. Why did H2SO4 require about twice the volume of NaOH solution for the titration? 2. Explain the effect of each of the following sources of error on the molarity of NaOH as determined in this experiment stating whether the concentration of NaOH obtained would be too high or too low. a. The buret is contaminated with an acid solution. b. The buret contains a large air bubble in the tip‚ which
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Heats of Reaction Lab Report Purpose: To measure the heats of reaction for three related exothermic reactions and to verify Hess’s Law of Heat Summation. NaOH(s) ( Na+(aq) + OH-(aq) ΔH = -10.6kcal/mol NaOH(s) + H+(aq) + Cl-(aq) ( H2O + Na+(aq) + Cl-(aq) ΔH = -23.9kcal/mol Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) ( H2O + Na+(aq) + Cl-(aq) ΔH = -13.3kcal/mol Background: Energy changes occur in all chemical reactions; energy is either absorbed or released. If energy is released in
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Indicator 1. Fill the 50-milliliter buret with a 0.25 molar NaOH solution. 2. Record volume. 3. Measure out between 20 milliliters and 40 milliliters of the unknown HCl solution. 4. Record volume. 5. The amount of unknown HCl is then added to the 100-milliliter Erlenmeyer flask. 6. Add two drops of the indicator‚ phenolphthalein‚ to the acid in the flask. 7. Using the slider on the right hand side‚ add NaOH to the HCl in the Erlenmeyer flask (This action is known astitrate)
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Hypothesis: If I increase the concentration of NaOH from 0.5M to 1M‚ then I will see the temperature slope increase in the reaction with an increased concentration because with an increase of moles‚ the particles will be colliding more often‚ therefore increasing the probability that the proper energy and alignment will occur to create more collisions in the same amount of time. Methods: List of Materials: • 110 mL of NaOH at 1 M (10 mL per run) • 110 mL of NaOH at 0.5 M (10 mL per run) • 220 mL of Acetic
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measuring the pH levels of each. The experiment also helped students classify different substances through their conductivity properties. The preparation of a 1 M stock solution from NaOH pellets diluted to a 0.1 M NaOH solution was also utilized in making the students understand the concept of titration. Using 0.1 M NaOH as a standard solution‚ the concentration of an unknown acid was calculated from the endpoint of an acid-base titration. II. Keywords: acid‚ base‚ salt‚ pH‚ electrolytes‚ conductivity
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