Part of The Student Room Group

  • 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

or


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. Determination of potassium hydrogen carbonate into potassium carbonate

    A larger cup of polystyrene is required to be used in order for the fizzing of the solution to not travel far away from the reaction. As mentioned before the experimental value obtained is well below the accepted literature value this also could be due to several reasons.

  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. 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. DCP+CE Analysis of a Hydrogen Peroxide Solution

    the average amount of moles for NaC2O4 in 1st titration Dividing absolute uncertainty (0.30g�0.02g) / (23+23+16+16+16+12+12) = (0.30g�0.067%)/ (23+23+16+16+16+12+12) = 0.30/134 � 0.067%+0% = 0.0022 � 0.0067% = 0.0022mol � 1.8x10-7mol Adding absolute and dividing absolute uncertainty 0.0022�1.8x10-7mol + 0.0023�1.8x10-7mol + 0.0023�1.8x10-7mol + 0.0022�1.8x10-7mol + 0.0025�1.8x10-7mol + 0.0026�1.8x10-7mol = (0.0022 + 0.0023 + 0.0023 + 0.0022 + 0.0025 + 0.0026)

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

    titre M = n/v M = 0.0003 moles/ 0.01525 dm3 M = 0.019672131 mol dm-3 The following table shows values from part two of the calculations which are for determining the oxidizing power of bleach. (Trial) Titration 1 � 0.05 cm3 Titration 2 � 0.05 cm3 Titration 3 � 0.05

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

    Fortunately this expectation was met with the results provided, although there were a few given anomalies formed from the systematic errors present, it was evident that the experiment did match the initial hypothesis of an increase in biodiesel yield. Although the conclusion states than an increase in concentration of the

  1. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

    2. When clamping the burette to the retort stand, it was made sure that the retort stand was not tilted towards any side as this could have introduced systematic errors in the volume readings. 3. While performing all the experiments, it was made sure that only one person was in-charge of the stopwatch.

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

    The offshot experiments have a deep characteristic pink color that doesn?t goes away with in time of 2minutes in the solution. 3. Before reaching the solution reaches the titrated value, when the burette solution is added to the conical flask the acid appears to be pink but after we swirl the solution it loses its color.

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