Beverly D. Panes January 24‚ 2013 Prof. Hazel G. Carreon 12 :30 – 3:30pm Summary Thermal Analysis The branch of material science known as thermal analysis is the study of the change of temperature within the properties of materials. A number of different properties are studied using this method including
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06.03 Calorimetry: Lab Report Procedure: Part II: Determining the Specific Heat of an Unknown Metal Data and Observations: Part I: Determining the Specific Heat of a Known Metal Metal: Aluminum Zinc Iron Copper Mass of metal 27.776g 41.664g 34.720g 41.664g Volume of water in the calorimeter 26.0mL 26.0mL 26.0mL 26.0mL Initial temperature of water in calorimeter 25.3 °C 25.3 °C 25.3 °C 25.3 °C Temperature of hot water and metal in hot water bath 100.5 °C 100.5 °C 100
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Determining the Specific Heat of an Unknown Metal Objective: To determine the specific heat of an unknown metal through the use of a calorimeter. Background: The specific heat of any substance represents the quantity of heat energy in joules required to heat one gram of the substances by one °C. The specific heat of a substance is dependent upon the temperature; this means that there is a temperature range for which the specific heat of a substance applies. For metals and metallic substances
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Results : Calculation : Part A Molecular weight of 1M of NaOH = 23g/mol + 16g/mol + 1g/mol = 40g/mol 1M = 40g/mol dissolved in 1L and 20g dissolved in 500ml 20g of NaOH was used to prepare 500ml of 1M NaOH. Part B Molecular weight of 1M of HCl = 35.5g/mol + 1g/mol = 36.5g/mol Specific gravity = 1.19kg/L 37% HC1 × 1.19kg/L = 0.44kg/L Convert w/v to mol/v = = 12mol/L = (12mol/L) = (1M)250ml = 20.83ml ≈ 21ml 21ml of concentrated HC1 is used to prepare 250ml of 1M of HC1. Part C For 0.1N of NaOH
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Figure 1: Titration curve of 0.160 grams of an unknown diprotic acid that was dissociated in distilled water. Shown is the pH versus the volume in milliliters of 0.1 M NaOH‚ a strong base‚ added to the solution. The initial pH reading of the solution was a pH of 2.60. Although the pH of the ½ equivalence point was unknown‚ it could be estimated by halving the volume of NaOH used at the first equivalence point. At the first equivalence point‚ 13.63 milliliters of NaOH had been added to the unknown
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Question # 1: You are titrating 50 ml. of nitrous acid with sodium hydroxide (0.15 M). Equivalence is reached at 22.0 ml of NaOH delivered. Calculate the pH of the solution in the flask: a- before the beginning of the titration - after the delivery of 5 ml. of titrant b- at half-equivalence c-at equivalence d-after delivery of 23 ml. of titrant Part A) Reaction is: HNO2 + OH- NO2- + H2O Ka for Nitrous acid = 7.2E-4 Kw = Ka*Lb Kb = 1.0E-14/7.2E-4 Kb = 1.38E-11 Moles of base:
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The dissolution of the drug in different liquisolid formulations was performed in 500 ml simulated salivary fluid (phosphate buffer pH 6.8) maintained at 37 ± 0.5 ºC using the USP dissolution tester apparatus II‚ at a rotation speed of 50 rpm. Aliquots from the dissolution medium were withdrawn at 1‚ 2‚ 3‚ 4‚ 5‚ 6‚ 7‚ 8‚ 9‚ 10‚ 12.5‚ 15‚ 20‚ 25 and 30 minutes time intervals. The samples were changed with fresh dissolution medium of same amount to maintain a constant volume in the vessels. Samples
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MA‚ PAULINE Date Performed: 10 SEPTEMBER 2014 NACIONGAYO‚ DANIELLE Date Submitted: 17 SEPTEMBER 2014 TEDERA‚ YVES HEAT EFFECTS AND CALORIMETRY Experiment No. 2 I. RESULTS A. Determination of Heat Capacity In this experiment‚ an improvised calorimeter was used to determine the heat capacity. The calorimeter weighed 4.47 grams prior to the addition of water. Tap water‚ 40 mL to be exact‚ was added to the calorimeter which increased the weight to 43.87 grams. The water was measured using
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I. Objective: The objective of this experiment is to determine the mass percent of iron in an iron compound using a spectrophotometer. From there‚ determine which iron compounds are in the stock room bottles based off of the experimental mass percent results. II. Introduction: The objective is to determine the mass percent of iron in an iron compound using a spectrophotometer. From there‚ determine which iron compounds are in the stock room bottles based off of the experimental mass percent results
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First‚ prepare a data table. Record what you see throughout the laboratory activity. Your teacher will demonstrate for the class the reaction of metallic copper with concentrated nitric acid‚ HNO3. This must be done in the fume hood. (Caution: Avoid breathing poisonous gases. Avoid contact of skin with nitric acid. It burns skin and clothing.) One student will be asked to feel the side of the demonstration beaker and report to the group. The products formed are copper(II) nitrate solution‚ Cu(NO3)2(aq)
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