it and repeat to get the other two densities. Then record the measurements and density for each trial and then average the densities. Part 2: Calibration of a Buret 1. Get 4 small beakers‚ clean and dry them‚ then record the mass of each. 2. Get & Fill the buret past the zero mark. 3. Measure 10‚ 15‚20‚25 mL of water from the Buret separately into the four small beakers. 4. Measure and record the combined mass of the beaker and the water 5. Then we determined the actual
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a series of standard solutions containing known concentrations of Fe(phen)32+‚ as well as a solution with Fe from a vitamin tablet‚ and measure their absorbances on the Chemistry Department’s Beckman DU7400 spectrophotometer. Construction of a calibration curve using your standard solutions will allow you to determine both the molar absorptivity of the Fe(phen)32+ complex and‚ with a pair of measurements of the iron tablet solution’s absorbance under the same conditions‚ the mass of iron that was
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Experiment 2 Preparation of Primary Standard solutions and Standardizing Acid and Base solutions Objectives: The objective of this experiment is: 1- To prepare two primary standard solutions‚ KHP and Na2CO3 2- To standardize a sodium hydroxide solution using the prepared primary standard KHP. 3- To standardize a hydrochloric acid solution using the prepared primary standard Na2CO3. 4- To calculate the concentration of an unknown acid or base. Introduction A primary standard is a standard that
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and slowly with swirling‚ add approximately 2 mL of 3 M HCl. The solution should be a dark yellow to redbrown from the presence of I3 - complex. 4. Titrate the iodine. Rinse the buret with distilled water and then three times with small portions of your 0.10 M sodium thiosulfate solution. Then‚ fill up the buret with the 0.10 M sodium thiosulfate solution. Titrate the bleach-iodine mixture in your Erlenmeyer flask until the iodine color becomes yellow. Add one dropperful of starch solution
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Analysis 819 12-1 “Wet” Dry Ice 822 12-2 Measuring the Triple Point Pressure of CO2 784 Pre-Lab Paper Chromatography 824 LABORATORY PROGRAM Copyright © by Holt‚ Rinehart and Winston. All rights reserved. Back Pre-Lab Volumetric Analysis 842 16-1 How Much Calcium Carbonate Is in an Eggshell? 844 16-2 Investigating Overwrite Marking Pens 848 16-3 Is It an Acid or a Base? 851 16-4 Percentage of Acetic Acid in Vinegar 854 Pre-Lab Calorimetry
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bleach using a buret in a titration procedure. The disappearance of the dark blue color of the starch-iodine complex will signal the end point. II. Procedures Pre-Lab Questions 1. What is meant by a “titration”? Titration is a technique where a solution of known (acid or base) concentration is used to determine the concentration of an unknown (acid or base) solution. 2. A solution of household vinegar (a mixture of acetic acid and water) is to be analyzed. A pipet is used to measure
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MnSO4∙ H2O‚ 1.0 M‚ 50 mL * Oxalic acid solution‚ H2C2O4‚ 0.25 M‚ 60 mL * Potassium permanganate solution‚ KMnO4‚ approx. 0.02 M‚ 100 mL * Sulfuric acid solution‚ H2SO4‚ 6 M‚ 50 mL Materials: * Buret‚ 50-mL * Erlenmeyer flasks‚ 250-mL‚ 3 * Hot plate * Thermometer * Volumetric pipet‚ 10-mL * Volumetric pipet‚ 25-mL *
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Acid-Base Titrations A Titration of Potassium Hydroxide Phthalate and Sodium Hydroxide Hanna Piper Department of Chemistry‚ SUNY College at Brockport‚ Brockport‚ NY 14420 Chemistry 205.06 Abstract Titrations are used to find the molarity of an unknown solution. A titration begins with an analyte and titrant being used to measure the unknown molarity of the analyte. In the following experiment‚ sodium hydroxide was used as the titrant and potassium hydroxide phthalate was used as the
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are obtained if the eye is not perpendicular to the scale. Read the volume of water to the nearest 0.1 mL. Record this volume. Measure the maximum amount of water that your largest test tube will hold. Record the volume. C The Thermometer and is Calibration: Place ice in beaker and cover the ice with distilled water. Allow about 15 min for the mixture to come to equilibrium and then measure and record the temperature of the mixture. Theoretically‚ this temperature is 0°C. Set up a beaker
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Review Session *The information shown below is usually provided on the exam. Also‚ remember that calculators can be used on the exam.* Absolute Uncertainties 5.00 mL pipet: ± 0.01 mL 10.00 mL pipet: ± 0.02 mL Digital balance: ± 0.2 mg 50.00 mL volumetric flask: ± 0.04 mL 100.00 mL volumetric flask: ± 0.08 mL 25.00 mL buret: ± 0.03 mL Useful information pX = -logX pH = 14 – pOH Kw = 1 x 10-14 pH = pKa + log[A-]/[HA] pKa + pKb = 14 Solution of quadratic equation of the form ax2 + bx +
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