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

Preparation of a standard solution of oxalic acid and using it to standardize a solution of sodium hydroxide.

Extracts from this document...

Introduction

Preparation of a standard solution of oxalic acid and using it to standardize a solution of sodium hydroxide. Data collection Mass of oxalic acid crystals = 1.5g �0.001g Burette: oxalic acid solution made using a 250cm3 volumetric flask with an uncertainty of � 0.5cm3 Pipette: 25.0cm3 of 0.100 mol dm -3 NaOH(aq) �0.04cm3 Indicator: 3 drops of phenolphthalein End point: taken to one drop when the faint pink colour of the indicator just disappeared. Trial Volume of oxalic acid cm3 uncertainty �0.05 Observations 1 13 The solution turned colourless once this amount of acid was added. 2 12 The solution turned colourless at this volume of acid. 3 11.5 The solution was a clear light pink colour at this volume. ...read more.

Middle

+ 2NaOH(aq) (COONa)2(aq) + 2H2O(l) Concentration = amount of solute Volume in dm3 Volume = 12.2 / 1000 = 0.0122dm3 Moles = 25 / 1000 = 0.025*2 = 0.05 Concentration = 0.05 / 0.0122 = 4.09M = 4M Uncertainties Balance = 0.001/ 1.50 * 100 = 0.06% Burette = 0.5/25.0 *100 = 2% Pipette = 0.04/ 25.0 *100 = 0.16% Volumetric flask = 0.50/250*100 = 0.20% Total uncertainty = 0.06% + 2% + 0.16% + 0.20% = 2.42% Therefore concentration of sodium hydroxide = 4 � 2.42% = 4 � 2 Conclusion and evaluation The concentration of the given Sodium Hydroxide solution is 4M. This value is calculated from finding the amount (number of moles) ...read more.

Conclusion

However if the burette tap was left open for longer the solution would be clear but it would be more acidic than neutral. The balance was very sensitive to the environment; this could have increased the uncertainty of the experiment. Improvements Ensure that all the equipment is thoroughly cleaned / sterilized before use. This reduces the amount of uncertainties and ensures that the solutions are clean and not contaminated. Repeat the experiment several times so as to reduce the amount of errors and uncertainties. Read measurements correctly, keeping the eye at the correct level that would enable accurate results. Ensure that all the apparatus function correctly before beginning the experiment. Place the balance in a room where minor factors would not affect it. Use more accurate apparatus so as to decrease percentage errors. ?? ?? ?? ?? Njeri Kabanga ...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. The preparation of Benzoic acid from benzamide

    The crystal will be dissolved completely. Because the NaOH react with the benzamide and give the salt form of benzoic acid. 5. How can you tell when an excess amount of HCl has been added in step 3 ?

  2. pKa. When constant successive portions of Sodium Hydroxide are added to Acetic Acid; how ...

    at regular intervals which will ultimately allow the pKa to be determined. Hypothesis: In this experiment, the amount of Sodium Hydroxide released from the burette will never change. What changes, however, is how much base is in the conical flask.

  1. Esterification Equilibrium

    Moles of water are 0.378�0.0017mols Mixture 5 contained 1ml of ethanol and 4ml of ethyl ethanoate; hence the amount in moles of ethyl ethanoate and ethanol present in the original mixture are; Moles of ethyl ethanoate; calculating uncertainty 0.041 � 2.3x10-4 mol of ethyl ethanoate was present.

  2. Standardization of sodium hydroxide solution using oxalic acid.

    Chemical equation : H2C2O4+ 2NaOH ? Na2C2O4 + 2H2O The number of moles of H2C2O4.2H2O : = Mass of H2C2O4.2H2O (g) Relative Molecular Mass = 1.6253 g 126g/mol = 0.0129 mol. Uncertainty : 0.0001 x 0.0129 1.6253 = 7.937 x 10-7 mol.

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

    of the specific heat capacity of the solution. Since Q = mc.?T, a understatement in the value of c would lead to a understatement in the value of Q which in turn, would lead to an understatement in the value of ?HMgO. Secondly, since Magnesium is a fairly reactive material, it would not be wrong to say that

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

    form of methyl esters, an organic chain compound that has a set of properties. The experiment involves the reaction between vegetable oil and potassium hydroxide and methanol mixed together. The equation for the reaction of the transesterification is: Vegetable Oil (l)

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

    + Na+ OH- (aq) →Na + A- (aq)+ H2O 1 mole of acid reacts with 1 mole of NaOH solution. Hence 0.02488 moles of potassium hydrogen phthalate will react with 0.02488 moles of NaOH solution. Concentration of solution = Moles of solution/Volume of solution =0.02488/0.02554 = 0.097450 M ±

  2. Measuring the fatty acid percentage of the reused sunflower oil after numerous times of ...

    VEGETABLE OILS SMOKE POINTS ( ± 0.5oC) Safflower 265.0 Sunflower 246.0 Soybean 241.0 Canola 238.0 Corn 236.0 8 ASLAN Özge Cemre D129077 4 Ta ble 1: Smoke points of some vegetable oils in C degree. In this experiment the free fatty acids in the refined sunflower oil which is used

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