Colligative Properties & Osmotic Pressure Peter Jeschofnig‚ Ph.D. Version 42-0149-00-01 Lab Report Assistant This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions‚ diagrams if needed‚ and data tables that should be addressed in a formal lab report. The intent is to facilitate student’s writing of lab
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a. Determine the freezing point depression 53.02 – 50.78 = 2.24 °C b. Calculate the molar mass of the unknown substance 7.1 °C/m X 2.04 g (solute) X 24.8 g (solvent) X 2.24 °C = 260.0 g molar mass = 260. g 2. What are colligative properties? Colligative properties are properties of a solution that change when the condition of the solution changes. II. PROCEDURE Part B 1. Set up a Bunsen Burner‚ ring stand and clamp‚ as shown in picture below. 2. Fill a
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Report Submitted: September 4‚ 2013 Title: Observations of Chemical Changes Purpose: To observe some properties of chemical reactions and to associate chemical properties with household products. Procedure: In this experiment I used a 96-well plate to hold each of the chemical reactions that occurred during this lab. Using a pipet‚ I added two drops of one chemical with two drops of another chemical and observed the effects of each reaction. Data Table 1: Experimental Data Well # |
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Experiment 1: Colligative Properties & Osmotic Pressure Name: Ima Student Lab Partners: None Date of Experiment: June 4th – 6th 2011 Location: My apartment Course Number: CHE112 Abstract: In this experiment‚ the objective was to observe the effects of some of the colligative properties of solutions.
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Abstract If we live in a place that gets cold in the winter‚ we have probably seen trucks out spreading a mixture of sand and salt on the streets after a snowfall to help deice the road. Do we sometimes dump ice cubes into a drink to help keep cool on a hot summer day? Have we ever watched the ice cubes melt and wondered how we could make them melt more slowly—or even faster? In this science activity we will get to try some different‚ common household substances to try and answer this question:
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Department of Chemistry Physical and Chemical Properties Submitted by: Date Submitted: 2/2/2014 Date Performed: 1 Lab Section: Course Instructor: PURPOSE: To identify chemical and physical change in matter. PROCEDURE: Finding out the physical and chemical change in matter. There was seven different substances that were being tested; Mossy Zinc (Zn)‚ Magnesium (Mn)‚ Copper (Cu)‚ Magnesium Oxide (MgO)‚ Copper II Nitrate (Cu(NO3)2)‚ Copper II Carbonate (CuCO3) and Sodium Chloride
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Mini-Lab Report Objectives: There were two major goals of the “Observing Bacteria and Blood” experiment. The first was to establish a familiarity with the proper techniques for using a microscope. The experiment focused on both the basic components of a microscope (i.e. how to adjust the knobs and levers for the desired result) as well as how do decide the proper objective to use for observing a specimen. The second goal major goal of this experiment was to practice observing live specimens
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COLLIGATIVE PROPERTIES: FREEZING POINT DEPRESSION AND BOILING POINT ELEVATION DAY 1 – 04 FEBRUARY 2015 Colligative Properties Depends on the NUMBER of solute‚ not on the nature of solute particles Freezing Point Depression Boiling Point Elevation Vapor Pressure Lowering Osmotic Pressure Electrolyte and Nonelectrolytes Electrolytes •Separates in water forming a solution that conducts electric current •IONIC COMPOUNDS Non- electrolytes • does not allow the flow of an electric current • COVALENT
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Determining the Molar Mass of an Unknown Solute by Freezing Point Depression Introduction: Colligative properties of solutions are only influenced by the concentration of solute particles and are independent of the nature of the solute. Some examples of colligative properties are boiling point elevation‚ vapor pressure lowering‚ and freezing point lowering (depression) (Brown‚ 542). For a substance to freeze‚ the kinetic energy of the particles must be low enough for the
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Zn(NO3)2 into well A3 of the 24-well plate. 4. Place 10 drops of Iron (III) chloride‚ FeCl3 into well A4 of the 24-well plate. 5. Place 10 drops of Copper (II) sulfate‚ Cu SO4 into well A5 of the 24-well plate. 6. Take the metal solids from your LabPaq; there should be one piece each of magnesium‚ zinc‚ and iron plus two pieces of lead. Note: Magnesium and lead oxidize very easily and an almost invisible oxidation layer may coat the metal. To insure good reactions you should scrape the surface
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