• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

To determine the concentration of hydrogen peroxide

Extracts from this document...

Introduction

TO DETERMINE THE CONCENTRATION OF HYDROGEN PEROXYDE Aim: To determine the concentration and the volume strength of hydrogen peroxide in locally purchased solution using a redox titration. Introduction: Hydrogen Peroxide is a strong oxidizing agent, readily breaking down to form water and oxygen; and aqueous solution of hydrogen peroxide can be used for bleaching hair and used as an antiseptic for minor skin wounds. However, it is a highly efficient cellular poison. It is so devastating that we have an enzyme called "peroxidase" in our body that constantly removes any hydrogen peroxide that gets into our cells. In this experiment we will use a 20-volume hydrogen peroxide solution. It has to be diluted for the use. The solution will then be titrated against an acidified standard solution of potassium manganate(VII). The concentration of hydrogen peroxide in the titrated sample is then calculated, from which it is easy to calculate the concentration of the original sample. ...read more.

Middle

26.6 26.6 Readings used Volumetric Flask: 250ml + 0.15ml Volume of diluted H2O2 250ml+0.15ml Purity of potassium permanganate 99.0% Molarity of H2O2 ? Data Processing and Presentation: Correct answer given:- Molarity of H2O2- 6.54mol dm-3 Calculation From Titration: 5H2O2(aq) + 2MnO4-(aq) + 16 H+(aq) --> 10 H+(aq) + 5O2(g) + 5Mn2+(aq) + 20H2O(l) * Concentration of H2O2= no of moles/volume of H2O2 * Concentration of H2O2= No. of moles/10 ml * No. of moles= concentration x volume. However, we do not have the concentration of H2O2. * From the equation above we know that H2O2 and MnO4- are in the ratio 5:2. Therefore, form this ratio, if we can find the number of moles of MnO4- we can find the number of moles of H2O2. * Number of moles of MnO4- = concentration x volume = 0.01993(given) ...read more.

Conclusion

KMnO4- TOTAL ERROR PERCENTAGE= Systematic Errors: Even though my calculated value is within the random errors, some of the systematic errors which could have occurred are: * Judging the end point of the titration. * Diluting solutions while using some of the equipment * Overshot the mark in the volumetric flask. Conclusion: * From the titration results, the concentration of H2O2 is 6.63 mol/dm3 + 0.2 mol/dm3 * The expected value was 6.54mol/dm3 * The expected value was within the range of our calculated errors. 6.43mol/dm3 <--6.63 mol/dm3 -->6.83 mol/dm3 * Total error= [(6.63-6.54)/6.54] x 100 = 1.38% * Systematic errors are none or negligible as the calculated answer is within the limits of our calculated error. Evaluation: * The total error was less than the random errors. Our expected value was within the range of our random errors. Therefore, there were no systematic errors. Improvements: * Use better equipment- A grade glasswork. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Investigate the rate of reaction of luminol in various factors. The objective was to ...

    Dangerous if swallowed. Causes serious internal damage due to release of oxygen. If swallowed: Wash out the mouth and give a glass or two of water. Seek medical attention. If solution gets in eyes: Flood the eye with gently running tap water until a first-aider arrives.

  2. THE CATALYTIC DECOMPOSITION OF HYDROGEN PEROXIDE

    conducting the experiment, I observed that once the hydrogen peroxide comes into contact with the manganese (V) oxide the decomposition of hydrogen peroxide would begin very quickly. The mixture turns grey colour and produces a lot of effervescence. A slightly pungent odour is also produced.

  1. Determination of potassium hydrogen carbonate into potassium carbonate

    Also send back the electronic balance to the manufacturer to re-calibrate it. Thermometer Systematic error � 0.10K Equipment limitation. This is because the actual reading might be designated at another place. i.e placed incorrectly. Use multiple scales and increase the number of trials done. In order to increase the accuracy.

  2. Aim: Using an iodine clock reaction to find the order of hydrogen peroxide and ...

    Conclusion From this experiment I can conclude that the order of H2O2 is 1st order and that Ethanoic Acid (CH3COOH) is 0 order. This is because as the volume of H2O2 increased by a factor of two, the rate increased at a constant rate.

  1. Using Redox Titration to Analyze the Oxidizing Strength of Bleach Lab

    cm3 Start 0.30 20.9 25.6 End 20.90 40.9 40.70 Total 20.60 20.00 20.10 Average Titre value= (20.00 + 20.10)/2 = 20.05 cm3 = 0.02005 dm3 Uncertainty Propagation found later The following table shows values for the mass taken each trial Titration No.

  2. Decomposition of Hydrogen Peroxide Lab

    Determining Rate Orders at Table of Volumes and Concentrations Part Volume Molarity Volume Molarity Initial Rate (kPa/s) 1 4.00 0.88 M 1.0 0.5 M 0.1356 2 4.00 0.88 M 1.0 0.25 M 0.06263 3 4.00 0.44 M 1.0 0.5M 0.07641 3)

  1. Biodiesel Investigation - How the concentration of Potassium Hydroxide solution would affect the yield ...

    The centrifugation process will separate the biodiesel and glycerol. Extract the thin biodiesel layer (on top), measure the mass of the biodiesel in the initial beaker and derive the percentage yield of biodiesel from the mass difference between the solutions, density from mass and volume and make observations on the mass obtained.

  2. The purpose of this experiment is to determine the concentration of a solution of ...

    Since the discrepancy % is low, we have accepted the experimental value. The deviation from the theoretical amount is small and the errors that could have affected the result range from systematic errors such as calibration of the apparatus used to random human errors such as parallax in reading the values.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work