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

Redox titration of copper evaluation

Extracts from this document...

Introduction

Redox Titration of Sodium Thiosulphate against Copper (II) Sulphate My results from this titration can be seen in the table below: Rough 1st 2nd 3rd Final Reading/cm3 29.30 25.25 30.40 28.80 Initial reading/ cm3 05.05 0.80 6.20 4.55 Titre/ cm3 24.25 24.45 24.20 24.25 The concordant results I will be using in my calculation are the titres from my 2nd and 3rd titration as there are within 0.01 cm3 of one another. To calculate the average titre I will use the following method: Average Titre = (24.20 + 25.25) ...read more.

Middle

This is because in each step of the reaction there are 2 moles of each. This will mean that the number of moles of Cu2+ will be the same as the number of moles of S2O32-: n = c x v n of S2O32- = 0.102827763 x 24.225 1000 = 2.491002571 x 10-3 mol n of Cu2+ = 2.491002571 x 10-3 mol Now that I have the number of moles of Cu2+ I can calculate the concentration of it: c = n v c of Cu2+ = 2.491002571 x 10-3 (25/1000) ...read more.

Conclusion

percentage error I need to work out the percentage of the concentration that could be incorrect: Percentage Error = Total uncertainty x Concentration 100 = 0.582759211 x 0.099640102 mol dm-3 100 = � 5.806618723 x 10-4 Now that I have the percentage error I can show the possible errors that there could be in the calculation of the concentration of Cu2+: Highest possible c of Cu2+ = 0.100220763 mol dm-3 Lowest possible c of Cu2+ = 0.09905944 mol dm-3 However I will represent the final concentration I have calculated of the Cu2+as: 0.099640102 � 5.806618723 x 10-4 mol dm-3 0.0996 � 5.81 mol dm -3 (3sf) ...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

Here's what a star student thought of this essay

3 star(s)

Response to the question

Overall a good example of calculations needed for experiments. The candidate titles this essay as an 'evaluation,' but rather than an evaluation being present, there is just a set of calculations. For an evaluation the candidate should have included possible ...

Read full review

Response to the question

Overall a good example of calculations needed for experiments. The candidate titles this essay as an 'evaluation,' but rather than an evaluation being present, there is just a set of calculations. For an evaluation the candidate should have included possible errors that might have gone wrong with the experiment and how this could have been improved. The candidate should have displayed the method used so that they could have shown where they got this information from about possible errors in a concise format. To do this sort of evaluation displays a higher understanding of every aspect of the practical and these are important skills to develop for the chemistry industry.

Level of analysis

The decimal places the candidate uses is consistent in the table which means that the candidate could make accurate calculations from them. They also repeated the titrations four times and started off with a trial meaning their results have a greater chance of being reliable. The number of decimal places presented in the end result should ideally be consistent with the number of decimal places used in the table, and in this instance it is not. The candidate does calculate percentage errors which is good to know the margin of possible error in the experiment and how this may affect it, but they do not explain the significance of the results.

Quality of writing

The candidates spelling, grammar and punctuation are all fine, they highlight their final answers in bold which will also make the answers clear and easier to mark.


Did you find this review helpful? Join our team of reviewers and help other students learn

Reviewed by skatealexia 08/07/2012

Read less
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)

    Wash off if spilt on skin or surfaces Solid hydrated sodium carbonate No significant risk N/A N/A Sodium carbonate solution 0.1 mol dm-3 No significant risk N/A Avoid spillages Methyl red indicator No significant risk N/A Avoid spillages as it may stain Procedure Making up the sodium carbonate solution *

  2. THERMOMETRIC TITRATION

    Both the mists are solution have corrosive effect on human tissues. * Can cause damage your respiratory organs * Burn your skin severely * Cause damage to your eye sight if came into contact with eyes. * It can also harm intestines if drunk.

  1. Bleaching experiment. Estimation of available chlorine in commercial bleaching solution.

    + Cl-(aq) --> Cl2(g) + H2O(l)------------(1) Cl2(g) + 2I- (aq) +2H+ (aq)--> I2(aq) +H2O(l) + 2Cl- (aq)-(2) I2(aq) + 2S2O32-(aq) --> 2I-(aq) +S4O62-(aq)-------------------(3) Average volume of Na2S2O3 used to titrate with the dilute bleaching solution= [(29.05 + 28.75 + 29.00)/3] /1000 =0.02893dm3 In reaction (3), it is known: no.

  2. PPA1 Preparation of Potassium Trioxalatoferrate

    2Fe(OH)3 + 3H2C2O4 +3K2C2O4 --> 2K3(Fe(C2O4)3) + 6H2O Brown/Orange --> Green * The hot solution is filtered through fluted filter paper into a crystallising basin * 25 cm3 of Ethanol is added to the filtrate and any crystals that formed were dissolved by gentle heating.

  1. determination of the percentage of oxalate in iron (II) oxalate by redox titration

    The burette was filled with standard potassium manganate (VII) solution. 13) The initial reading on the burette was recorded. 14) The reaction mixture inside the conical flask was warmed over a heating machine to about 60�C before titration. 15)

  2. Determination of the formula of hydrated Iron (II) Sulphate crystals (FeSO4xH2O)

    = 0.05 x 100 = 0.34% 14.80g The main procedural error that may have occurred in method one is that the crucible and the FeSO4(H2O)7 may not have cooled completely before they were weighed. If this happened for every time that the crucible was weighed after heating, the end measurement

  1. Making Copper (II) Sulphate Stock Solution evaluation

    x 2 = 0.001 x 100 24.954g = 4 x 10-3 % % uncertainty of the 1dm3 flask = 0.8 x 100 1000 = 0.08 % Therefore the total uncertainty = 0.08 % + 4 x 10-3 % = 0.084 % So, to work out the percentage error I need

  2. Essay on the Oxides of Period 3 Elements

    This is because many molecules of silicon dioxide are joined together to form a giant lattice. It does not conduct electricity in any state as the ions are not free to move around. As for phosphorus pentoxide and chlorine(VII) oxide, they have simple covalent structure.

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