Empirical Formula of Magnesium Oxide

Empirical Formula of Magnesium Oxide Data Collection and Data Processing Submitted To: Ms. G. Fronczak Submitted By: Sonia Michniewicz Due Date: May 11, 2010 Course: SCH3UC-01 Design Purpose: To determine the empirical formula of Magnesium Oxide Independent Variable: amount of oxygen available Dependent Variable: amount of magnesium oxide produced Controlled Variables: Heat of the flame, height of the flame, room temperature, mass of magnesium strip, and the same electronic balance were some of the controlled variables in this experiment. For all the trials that were conducted, the gas valve and the needle valve were not altered which kept the flame consistent- intensity and height. Since the whole experiment was completed during one period and in the same room the room temperature remained the same. 10cm±0.1cm of magnesium strip was measured for each trial and the mass each time was around 2.0g±0.1g. The same electronic balance was used to minimize the error. - Wire gauze - Crucible with lid - Ring stand - Flint starter - Bunsen burner - Steel wool - Ring clamp - Goggles - Electronic balance - Crucible tongs - 10cm±0.1cm of magnesium strip - Clay triangle Materials Procedure . Safety First! Put on goggles 2. Using a balance, determine the mass of a clean, dry porcelain crucible and lid 3. Clean the surface of a 10 cm±0.01cm strip of magnesium

  • Word count: 1040
  • Level: International Baccalaureate
  • Subject: Chemistry
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The use of volumetric flask, burette and pipette in determining the concentration of NaOH solution

Experiment 2 Name Teoh Han Xuan ID No 11ADB05289 Partners Name Loo De Jing Date 13 June 2012 Title The use of volumetric flask, burette and pipette in determining the concentration of NaOH solution Objectives 1. To carry out acid base titration 2. To determine the end point with the use of indicators such as phenolphthalein Introduction In a titration, a burette is used to dispense measured increments of one solution into a known volume of another solution. The object of the titration is the detection of the equivalence point. In the reaction of HCl and Naoh, the equivalence point does occur when same mole of HCl has reacted with same mole of NaOH. The titration technique can be applied to many types of reactions, including oxidation-reduction, precipitation, complexation and acid-base neutralization reactions. An indicator is a substance that undergoes a distinct color change occurs is called the end point of titration, the indicator used in a titration must be selected carefully. Material & Apparatus NaOH solution, HCl solution, Phenolphthalein solution, Beaker, Burette, Pipette, Volumetric flask, Erlenmeyer flask, Funnel, Watch Glass Procedures 1. The volumetric flask was cleaned and rinsed with distilled water 2. 5 ml of NaOH solution was transferred into the volumetric flask

  • Word count: 1605
  • Level: International Baccalaureate
  • Subject: Chemistry
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