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

Finding out how much Acid there is in a Solution and the Molarity of acid through titration.

Extracts from this document...

Introduction

Finding out how much Acid there is in a Solution and the Molarity of acid through titration. Edward Hayden Barton Peveril College1 The aim of this investigation is to find out the morality of a sulphuric acid solution between 0.5 and 1.5 mol/dm3; the means of finding out is through titration. Apparatus needed are as follows: 25cm3 Pipette, burette, 250cm3 conical flask, 250cm3 beaker, stand, grip clamp, scales For each repeat experiment the following will be needed: 50cm3 of sulphuric acid, 25cm3 of 0.1mol Sodium Carbonate solution made from distilled water and 2.65g of solid anhydrous sodium carbonate, 2-3 drops methyl orange. First weigh a small piece of paper and record the result, then add this mass to the amount needed of sodium carbonate, in this case 2.65g. Add the amount needed of sodium carbonate to reach the total of paper and substance. Then dissolve this amount of sodium carbonate in distilled water until the solution reaches 250cm3. This makes 0.1m sodium carbonate solution. The equation shows that one mol of H2SO4 and one mol of NACO3 reacts to give one mol of sodium sulphate, one mol of water and one mol of carbon dioxide. We know the acid solution is between 0.05 and 0.15mol/dm3 therefore by making 0.1mol/dm3 solution the amount of each substance will be similar and not an excess of one is needed over the other. ...read more.

Middle

Results: Tests and repeats Amount of NaCO3 0.01 mol/dm3 (cm3) Amount of H2SO4 to neutralise the NaCO3 (cm3) 1 25 13.00 2 25 12.90 3 25 12.50 4 25 12.70 5 25 12.80 12.78 = average From the above data we are able to calculate the morality of the acid. H2SO4 (aq) + Na2CO3 (aq) --> Na2SO4 (aq) + H2O (l) + CO2 (g) 1mol 1mol 1mol 1mol 1 mol 12.78cm of ?m H2SO4 solution + 25cm of 0.1m Na2CO3 solution = titration Amount of mols of Na2CO3 used: 0.1/1000 = number of mols in 1cm3 of Na2CO3 solution = 0.0001m 0.01x25 = number of mols in 25cm3 of Na2CO3 solution = 0.0025m Morality of sulphuric acid solution: Therefore 12.78cm3 of H2SO4 solution = 0.0025m 0.0025/12.78 = number of mols in 1cm3 of H2SO4 solution = 0.000197 (3sf) 0.000197x1000 = the morality of solution (number of moles in 1000cm3) = 0.197 mol/dm3 (3sf) solution From taking the average of my results I have calculated that the morality of the sulphuric acid is 0.197m/dm3. However, at the beginning of the experiment I was told that the morality would lie between 0.05 and 0.15m/dm3. Therefore I believe that a small fault in the experiment resulted in me calculating the morality higher than previously expected. ...read more.

Conclusion

If possible, use small measuring apparatus this reduces the percentage error significantly. Then it is possible to transfer this into the larger container. The best idea however is to use a control colour so that it is possible to ensure the results all have the same pH reading. If possible use a control that you know is pH neutral then add the methyl orange and compare the results from the experiment to this control. Also by making larger quantities of the sodium carbonate solution there is a reduction in the percentage error, as a slight misjudgement has less effect the more substance and solution is being used. Instead of using the same solution of sodium carbonate for each repeat, re-make the solution, this will eliminate the possibility of the entire set of results be anomalous or inaccurate. It will provide a more accurate average at the end of the experiment than if you use the same solution throughout.2 By using all the outlines above the results gained are more likely to be accurate and therefore it is possible to come to a stronger and more accurate conclusion. After taking on the precautions outlined after hindsight of the experiment each result will be more accurate, by in a way starting all over again after each repeat minimises the possibilities of a whole set of anomalous results. 1 2 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous 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 GCSE Aqueous Chemistry essays

  1. How much Iron (II) in 100 grams of Spinach Oleracea?

    concentrations of 0.08 mol dm-3, 0.07 mol dm-3, 0.06 mol dm-3, 0.05 mol dm-3, 0.04 mol dm-3 , 0.03 mol dm-3, 0.02 mol dm-2 and 0.01 mol dm-3. 2) Make up a solution of Copper Sulphate solution 0.1 mol dm-3 by completing the following steps : a.

  2. Finding out how much acid there is in a solution.

    A titration involving a weak acid and a weak alkali cannot use an indicator as this will not work. A pH meter will be more suitable. The solution of which the concentration that will be known will be the sodium carbonate solution, which the sulphuric acid will be added to.

  1. Titrating Sodium hydroxide with an unknown molarity, against hydrochloric acid to find its' molarity.

    However, we need to make up 0.25dm3 of sodium carbonate solution; this means that in order to find the correct mass of anhydrous sodium carbonate that needs to be used, so I therefore need to multiply the above answer by ten.

  2. In order to find out the exact concentration of sulphuric acid, I will have ...

    These percentage errors are reflected in the accuracy of the equipment used. Particular attention was paid to calibration and measurements through out titration and this is why percentage errors are so marginal. Furthermore by making sure that the solution of sodium carbonate in the volumetric flask was exactly 250cm3 I

  1. To carry out a titration between a strong acid and a weak alkali, to ...

    and shake it to mix the solution thoroughly. 9. Set up a burette and place it on the stool to ensure it is at eye level (so you can accurately read off the amount of sulphuric acid in the burette).

  2. Investigating the Effects of Increasing Copper Sulphate Solution Concentrations on the Germination of Cress ...

    The water will then hydrolyse insoluble storage material to soluble substances which can be transported. These are transported to the point at which the embryo is growing. This was prevented from happening in the strongest solutions. The uptake of water depends on osmosis, which relates to the diffusion of water

  1. Findingout how much acid

    To make the calculation more accurate and the result in standard figures I will add 10cm3 of Sulphuric acid. When coming onto the calculations it will be easier to calculate as this is a sensible figure. Indicators A chemical indicator is a compound which can change colour to indicate that the endpoint of a titration has been reached.

  2. Finding out How Much Acid There is in a Solution

    Variables The control variables, which are the factors I shall be keeping the same, are that I shall use the same solution of sodium carbonate for each titration, use the same batch of sulphuric acid because there's no guarantee the concentration of it is always the same for each batch, and the temperature will be constant.

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