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

Sulphuric Acid investigation evaluation

Extracts from this document...

Introduction

Analysis: Weight of weighing bottle 7.61g Weight of weighing bottle + anhydrous sodium carbonate 10.26g Mass of weighing bottle (after reweighing when empty) 7.61g Mass of solid anhydrous sodium Carbonate 2.65g Sodium Carbonate Solution: 250 cm3 of sodium carbonate (Na2CO3) Number of moles = mass Ar Mass: 2.65g of sodium carbonate Mr: Na =23g C=12g O=16g Ar of Na2CO3 = (23x2) + (12) + (16x3) = 106g Number of moles = 2.65g 106g = 0.025 moles in 250 cm3 of sodium carbonate Volume = 250 = 0.25 dm3 1000 Concentration (mol/dm3) = Amount in moles of solute Volume (dm3) Concentration of Na2CO3 = 0.025 = 0.1 mol/dm3 0.25 Titration Results: Na2CO3 + H2SO4 Na2SO4 + CO2 + H2O Approximate Accurate 1 2 3 Final burette reading 25.50 25.50 25.50 25.50 Initial burette reading 0 0 0 0 Titre 25.50 25.50 25.50 25.50 As my results were all the same, the Average Titre = 25.50 cm3 This means that 25.50 cm3 of sulphuric acid neutralises 25 cm3 of my sodium carbonate solution. ...read more.

Middle

However, this doesn't ensure that I used exactly 25cm3. This also applies for the volumetric flask. When making up the initial 250cm3 sodium carbonate solution, you cannot exceed the 250cm3 line; otherwise you cannot determine the correct number of moles in you solution. There may have been some errors in making up the solution to the line as it is difficult to determine whether the meniscus is on the line. This may mean that the concentration of the sodium carbonate solution is more dilute or more concentrated than what I calculated * The stand for my burette doesn't ensure the burette is completely straight. This could affect the readings for my solution if the meniscus isn't straight. . * The apparatus I use limits the accuracy of my experiment. Percentage uncertainty calculations enable me to evaluate how accurate/inaccurate my apparatus was. Percentage Uncertainty calculations: I can measure the percentage uncertainty of the following equipment I used: 1. Digital scale / Balance 2. Volumetric flask 3. Pipette 4. Burette 1. ...read more.

Conclusion

* Taking readings from a burette can be difficult as it is clear. To reduce the risk of misreading the volume, I would place a white piece of paper behind the burette, making it easier to see the meniscus. * As the stoichiometry of the reaction in my experiment was one to one, it is vital that all the sodium carbonate dissolved in the solution, allowing me to correctly calculate concentration and the number of moles. Therefore, I would heat the sodium carbonate solution using a Bunsen burner to ensure the entire solid is dissolved. I would then allow the solution to cool before transferring it to the volumetric flask. * In my experiment, I need to record the exact volume of sulphuric acid needed to neutralise the sodium carbonate solution. Therefore, noticing when my solution is neutralised is vital. To determine the colour change to a greater accuracy, I would use a colorimeter, which allows the absorbance of a solution at a particular frequency of visual light to be determined. This piece of apparatus would help me to know when the end point of experiment has been reached, when neutralisation occurs. ?? ?? ?? ?? ...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 Physical 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 AS and A Level Physical Chemistry essays

  1. Determination of the Amounts of Sodium Hydroxide Solution and Sodium Carbonate in a Mixed ...

    But this time, two determinations need to be made for every titration in the first method. If there are no definitions of 'orange' or 'colorless', which is actually the case, inconsistency and thus error will occur. Furthermore, this is my first time using phenolphthalein to do titrations since the start of F.6.

  2. Acid-Base Titrations.

    mL solution so [NH4+] = 0.5 mmol/100 mL = 0.005 mmol/L NH4+. [H3O+]2 = (5.60 x 10-10)(5 x 10-3) = 2.80 x 10-12 [H3O+] = 1.67 x 10-6, pH = 5.78 Since the pH should be approximately equal to pKa of the indicator, a reasonable choice would be either chlorphenol red or methyl red.

  1. Acid-base titration. Objective To determine the concentration of sulphuric acid (H2SO4) using sodium ...

    The beaker was rinsed with a small amount of distilled water and the rinse was transferred into the volumetric flask. The step of rinsing was repeated twice. Distilled water was added to the volumetric flask carefully. The volumetric flask was stoppered tightly.

  2. Investigating the Rate of the Reaction between Bromide and Bromate Ions in Acid Solution

    This is the method that I will use to make up solution C: 1. Put on safety goggles 2. Measure out 20cm3 of methyl orange solution (5 g dm-3) using a pipette into a beaker 3. Measure out 400cm3 of 1M sulphuric acid solution into a beaker using four 100cm3 pipettes 4.

  1. Investigating how concentration affects rate of reaction

    Wash them out with water and then with the corresponding solution. Fill each burette with its corresponding solution. 2. Add 5cm3 of potassium bromate(V) solution, 5cm3 of sulphuric acid solution and 5cm3 of phenol solution to a beaker. Add 4 drops of methyl orange indicator to the beaker.

  2. Titration. The aim of this investigation was to find out the accurate concentration of ...

    Mr (Na2CO3) = (2 x 23) + 12 + (3 x 16) = 106 To make 1000cm3 of a 0.100mol dm solution of sodium carbonate you would need 10.6g of the solid. So therefore to make 250cm3 of a 0.1mol dm solution of sodium carbonate, 2.65g was needed.

  1. We are aiming to accurately prepare a standard solution of 0.1 M (mol dm-3) ...

    We did not use 1000cm3 of water we used 250cm3 of water, so to make 0.1 M, we need to dissolve 10.6/4=2.65g of sodium carbonate in 250 cm3 of distilled water. I now have a sodium carbonate solution of 0.1 m.

  2. Individual investigation - Reaction to be studied Rate of reaction between propanone and ...

    * Propanone solution 2molddm-3 (50cm3) * Hydrochloric solution 2moldm-3 (50cm3) * 8 x Test tube * Boiling tube * 4 x Beakers * Colorimeter * Stopwatch * Pipette (5 cm3, 2 cm3, 1 cm3, 25 cm3) Methods: Steps used in "colorimetric": 1.

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