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

experiment to find the concentration of the ethanedioic acid

Extracts from this document...

Introduction

A2 Chemistry Experiment 1 - Redox Titration As this is a redox reaction there are two half equations: 5C2O42- -10e- ==> 10CO2 and 2MnO4- + 16H+ + 10e- ==> 2Mn2+ + 8H2O Combining these 2 half equations we get: 5C2O42- + 2MnO4- + 16H+ ==> 10CO2 + 2Mn2+ + 8H2O Therefore to find the concentration of the ethanedioic acid I can titrate with Potassium Permanganate which acts as an oxidising agent, with Ethanedioic acid acting as a reducing agent. The sulphuric acid will act as an acid catalyst, providing extra H+. H2SO4 IN EXCESS The Sulphuric acid is in excess to ensure all the ethanedioic acid will react with the KMnO4 until the equivalence point is reached. I will use a 0.05mol dm-3 concentration of KMnO4. Method: * Set up titration apparatus, and fill the burette with 0.05M Potassium Permanganate, fill up to zero on the burette, use a funnel and place apparatus on a stool if necessary. ...read more.

Middle

And finally to get the concentration of H2C2O4 simply do moles/volume, so moles of H2C2O4 / 0.025dm3 = concentration of H2C2O4 Experiment 2 I can use a gas collection to find the overall concentration of the acid mixture, and as I already have the concentration of H2C2O4 , I can simply minus that from the total concentration to get the concentration of the H2SO4. Both strong and weak acids will react with a metal, therefore I will react the acid mixture with magnesium metal. Quantities of chemicals to use As I have been told that the concentrations are approximately 0.1 mol dm-3 H2C2O4 and 0.2 mol dm-3 H2SO4, I can say that the total concentration is approximately 0.1+0.2=0.3 mol dm-3. I am going to use 25cm3 of the acid mixture, therefore total moles of acid mixture is 0.3 x 0.025 = 0.0075 moles H2SO4 + Mg ==> MgSO4 + H2 and H2C2O4 + Mg ==> MgC2O4 + H2 I need these in one equation so I can get the molar ratios, therefore I formed this ionic equation. ...read more.

Conclusion

Diagram: Safety Ethanedioic acid is a highly poisonous carboxylic acid. It is corrosive and may cause burns. If it comes to contact with skin rinse with plenty of water immediately. Wear a lab coat to prevent exposure to skin. Specimen calculation If 22cm3 of KMnO4 was needed for the redox titration, then 0.022 x 0.05= 1.1x10-3 moles of KMnO4 . Using 5:2 ratio of 5C2O42- 2MnO4- moles of H2C2O4 is (1.1x10-3 /2) x5=2.75x10-3 moles, and finally to get concentration 2.75x10-3 /0.025=0.11 mol dm-3. Which is almost 0.1mol dm-3 as suggested the concentration was approximately. The above was all from experiment 1, and now to get the concentration of the Sulphuric acid was experiment 2. If the volume of gas collected was 80cm3, then moles of Hydrogen would be (80/1000)/24=0.0033moles, however 4:2 ratio with acid so multiply by 2 to get 0.0066moles, and as I used 25cm3 acid, concentration is 0.0066/(25/1000)=0.27mol dm-3. To get the H2SO4 concentration minus the H2C2O4 concentration (0.11), 0.27-0.11=0.16mol dm-3, this is close to 0.20mol dm-3 ?? ?? ?? ?? 1 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Inorganic 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 AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    achieved that are less than 0.1cm3 apart Results Titre Rough 1 2 3 4 Final burette reading/ cm3 26.95 27.20 24.20 27.10 26.80 Initial burette reading/ cm3 1.35 2.05 0.35 2.50 2.20 Titre/ cm3 25.60 25.15 24.55 24.60 24.60 Mass of solid sodium carbonate used: 7.19g I stopped collecting data

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    that it is not contaminated at all, so it is going to be more precise. Then we add the same number of drops of indicator, and repeat the procedure again. Now we have an idea of when the endpoint is, so now we deliver solution (very important: always swirling the flask)

  1. effects Concentration and Temperature on the Rate of Reaction

    The amount of molecules reaching the activation enthalpy is about twice as many at 310K than at 300K, so this means that the reaction will go around twice as fast at 310K in comparison to the reaction taking place at 300K.

  2. Chem Lab report. Objective: To determine the concentration of potassium manganate(VII) solution using ...

    solution into the burette at once after pouring it out from the brown bottle to a beaker and do the titration at once after adding the potassium manganate(VII) solution into the burette. Then the time for potassium manganate(VII) solution to expose to light would be lower and the decomposition of it would be reduced.

  1. The Effects of Strong and Weak Acids on the Order of a Reaction.

    them surpass the activation energy - but there is also a greater chance of correct collisions. With more particles able to react now due to their increase in kinetic energy, the number of correct collisions will increase which means the overall rate of reaction will increase.

  2. sulphuric acid is dibasic

    X1 NaOH will be placed in it Burette (50cm3) X1 HCl/H2SO4 will be placed in it Sodium Hydroxide (NaOH) 200 cm3 To donate a pair of electrons/as a base Indicator phenolphthalein Beakers (100mls) X4 To store acids and bases Labels X2 Distilled water To rinse the burette and conical flask

  1. The aim of the courework is to find the unknow concentration of HCl

    Wash the beaker, rod and funnel several times using de-ioned water from the wash bottle, letting the washing go in to the flask. 7. make up the mark on the volumatric flask with de-ionised water. Stopper firmly, and shake the flask throughlyto mix the contents.

  2. An investigation into the behaviour of mono-di-tri protic acids with a pure metal.

    Increase in temperature not only increases average kinetic energy of the reactant particles, but also the fraction of particles having kinetic energy higher than the activation energy. Thus, the effective collision frequency increases. The activation energy (minimum energy required for a chemical reaction to occur)

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