IB Guide to Writing Lab Reports Example IB Chemistry IA
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IB Guide to Writing Lab Reports Example IB Chemistry IA


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Name ChemistryCandidate Number Internal Assessment0
Example IB HL Chemistry Internal Assessment
Received full marks http://ibscrewed4chemistry.blogspot.com/   Names have been removed for privacyThis document is in no way endorsed by the IBO, nor should it be used as such. This workremains the intellectual property of the original author. While you are free to seek guidancefrom this work, it should not be replicated in any manner for submission as IB assessment.This would be regarded as plagiarism and lead to cancellation of your diploma.

 

Name ChemistryCandidate Number Internal Assessment1
Contents
Experiment Design ……………….………………….………………….…………………..…….. 2Background Information ……………………………………………….………………….…….. 4Raw Data ………………….…………………..…………………..………………….………………. 5Observations ………………..…………………..………………….………………….……………. 6Processed Data………….…………………..………………….…………………..………………. 7Conclusion ………………..…………………..…………………..………………….…………….. 13Evaluation ………………..…………………..…………………..………………….…………….. 15Works Cited ……………………..…………………..………………….………………….………. 16

 

Name ChemistryCandidate Number Internal Assessment2
Experiment to investigate the calorific content of foods
Objective
 
In this experiment, you will burn several types of food in order to determine their heatcontent per gram.
Materials
 
 
one coke can
 
balance
 
stirring rod
 
retort stand and clamp
 
paper clip
 
aluminium foil
 
thermometer
 
cotton wool
 
2-3g sample of each type of food(almonds, pretzels, cheezels)
Safety and Environmental Care
 
 
Avoid contact with hot objects, do not put clothing near flame
 
If you are allergic to nuts inform your teacher immediately
 
Avoid contact with soot that forms on the bottom of the can, it may stain clothing
Method
1.
 
Secure the coke can in the clamp. Weigh 100g water and add this to the can.2.
 
Place a thermometer in the mouth of the can with a piece of cotton wool to preventheat loss. Record the initial temperature of the water.3.
 
Place a heat mat under the can. Weigh a sample of food and place it on a paper clip,with a piece of aluminium under the food sample to collect any burnt material.4.
 
After the food burns completely, record the final temperature of the water, anddetermine the actual mass of food that has burned. Repeat the procedure, using adifferent type of food sample.

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Sample IA Lab Report

The file below is an example of a lab report with the markings from the IB board.
  

Updating…
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SampleofIB2summativelab.pdf

(671k)
Tiffany Tam,

Aug 20, 2011, 5:30 PM
v.1
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90148869 ib-chemistry-lab-report-design-example

IB Chemistry Lab Report Design Example—
Effect of Temperature on Solubility of Potassium Chloride in Water
Research questi...

Materials
6 Syringes
1 Heating plate
6 distinctly labeled 50ml Beakers
1 Electric Balance
6 Stirring Rods
Distilled Water
...

Weigh each of the 50ml beakers labeled 1, 2, 3, 4, 5 and 6 and record their masses.
Introduce 100ml of distilled water int...
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90148869 ib-chemistry-lab-report-design-example

  1. 1.
    IB Chemistry Lab Report Design Example—
    Effect of Temperature on Solubility of Potassium Chloride in Water
    Research question
    How does temperature affect the solubility of potassium chloride in water?
    Hypothesis
    As the temperature of water increases, the particles of solid Potassium chloride, KCl, which
    are absorbing energy from its surrounding, start moving more easily between the solution
    and its solid state because. According to the second law of thermodynamics, the particles
    will shift to the more disordered, more highly dispersed solution state. I predict that as the
    temperature of a KCl and water mixture increases, then the solubility of the KCl will also
    increase.
    Variables
    Dependant variable
    The dependant variable will be the solubility of Potassium chloride in water that will be
    calculated at different temperatures. The solubility will change as temperature increases.
    Independent variable
    The control variables need to be constant in order to get valid and accurate results.
    The temperature of the solutions.
    Controlled variables
    The volume of distilled water used to dissolve Potassium chloride in each beaker
    The amount of Potassium chloride deposited into each beaker.
    The volume of the solution extracted by the syringe.
    Weight of each 50ml beaker

  2. 2.

    Materials
    6 Syringes
    1 Heating plate
    6 distinctly labeled 50ml Beakers
    1 Electric Balance
    6 Stirring Rods
    Distilled Water
    6 distinctly labeled 100ml Beaker
    Controlling the variables
    The mass of Potassium chloride and the volume of distilled water introduced into each
    beaker should be recorded in order to allow the experimenter to determine the molar
    concentration of Potassium chloride in water. Since the same amount of water and
    Potassium chloride are used in each beaker throughout the whole experiment, these
    variables are the least likely to be the sources of errors.
    All 6 solutions will be supersaturated in Potassium chloride. If the solutions were not
    supersaturated, an increase in solubility will not be detectable.
    In order for all the solutions be subjected to the same experimental conditions, the same
    amount of time dedicated for stirring should be the same in all 6 100ml beakers.
    The use of different syringes for the extraction of the Potassium chloride and distilled water
    solution from each beaker avoids the possibility of contamination in the case where the
    same syringe was used in all 6 beakers.
    The needle of the syringe should be placed at the midpoint between the surface of the
    solution and the bottom of the beaker upon extraction. This is because of it were placed at
    the surface of the solution some air particles might enter the syringe, and if it were placed
    at the bottom of the beaker some undissolved particles might be extracted, thereby leading
    to an increase in the actual concentration of the dissolved salt.
    The weight of each 50ml beaker (used for weighing the mass of dissolved Potassium
    chloride after the evaporation of water) should be recorded. If the experimenter were to
    weigh the mass of one beaker and take it as a default mass, the latter may be a source of
    error.
    In order to minimize errors and to "place" the solutions in the same environment, the same
    volume should be extracted from each solution using the syringes.
    After heating the extracted solution in the 50ml beaker for weighing purposes, some of the
    water might condense back into the liquid state (in the form droplets), thereby leading to an
    increase in the calculated weight of Potassium chloride. Therefore after evaporation has
    occurred and while the 50ml beaker is still hot, the beaker should be immediately weighed.
    Procedure

  3. 3.

    Weigh each of the 50ml beakers labeled 1, 2, 3, 4, 5 and 6 and record their masses.
    Introduce 100ml of distilled water into beakers 1 through 6.
    Beakers 1, 2, 3, 4, 5 and 6 are held at 0°C, 10°C, 20°C, 30°C, 40°C and 50°C respectively.
    Dissolve 50 grams of Potassium chloride into each beaker by using a stirring rod. The
    stirring in all 6 beakers should last 10 minutes.
    Insert the syringe at the midpoint between the solution's surface and the bottom of the
    beaker and extract 40ml as such from each solution.
    Push the contents of each syringe containing samples from the solutions in beakers 1, 2, 3,
    4, 5 and 6 into the 50ml beakers labeled 1, 2, 3, 4, 5 and 6 respectively.
    Heat each of the 50 ml beakers until complete evaporation of the water occurs, and then
    immediately place each beaker on the balance and record the mass.
    By subtracting from the combined mass of (1) the salt residue from the evaporated
    extracted solution and (2) the 50 ml beaker, the mass of the corresponding 50ml beaker, the
    mass of the salt dissolved in the extracted solution can be obtained. The number of moles
    can be calculated, by using the formula n= m/MM , where m is the mass of the salt and
    MM the molar mass, which is equal to 74.60g/mol . The number of moles is then divided
    by the volume of the extracted sample (40ml). The obtained concentration is then
    multiplied by a factor of 5, in order to get the concentration of the initial solution. As
    expected, the solubility will be directly proportional to the temperature, for as the
    temperature increases so will the molar concentration of KCl in distilled water.

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