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Titration I will neutralize the sulphuric acid with a base, which will be Sodium Carbonate (Na2 CO3),

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Introduction

FINDING OUT HOW MUCH ACID IS IN A SOLUTION The aim of this experiment is to find out the concentration of acid in an acidic solution. The acidic solution I will be using is sulphuric acid, and the concentration of this solution is somewhere between 0.05 and 0.15 mol dm-3. I have to find an accurate value for this concentration and to obtain my results I will use a titration. A titration is a method of quantitive analysis, which can be used when 2 solutions react together. I will neutralize the sulphuric acid with a base, which will be Sodium Carbonate (Na2 CO3), which will already have a set concentration. I use an indicator, Methyl Orange, because when you do a titration between a strong acid and a weak alkali, as I am, Methyl Orange is the indicator used. Reaction Equation Na2 CO3 (aq) + H2 SO4 (aq) Na2 SO4 (aq) + H2O (l) + CO2 The mass of Sodium Carbonate I will need to use is shown below... Na2 CO3 = 2 X sodium + 1 X carbon + 3 X oxygen = 46 + 12 + 48 = 106 grams However this is the amount of grams for 1 mole of sodium carbonate. I need 0.1-mol dm-3 of it because this sum is between 0.05 and 0.15 dm-3 so I will divide by 10... ...read more.

Middle

> Now add 3 drops of Methyl Orange indicator to the conical flask > Use a clean, dry 100cm3 beaker to fill a burette with the sulphuric acid. Run a little of the solution out of the burette into the beaker to make sure the jet is full of solution > Record the volume reading on the burette before starting the titration and read the burette to the nearest 0.05cm3 > Add sulphuric acid in small volumes to the solution in the conical flask, swirling the flask after each addition. When the solution turns light pink stop the adding of sulphuric acid. > Record the final burette reading and calculate the volume of solution you have to run out of the flask The first titration I am going to do will be a trial run to make sure I know exactly what I am supposed to do. After wards I will repeat the titration until 3 concordant results are achieved within 0.1cm3 of each other. References Teacher support coursework guidance AS/A level GCE chemistry (salters) page 30 Activity E12 - salters advanced chemistry activity pack Hazcard 95 - sodium salts Hazcard 98 - sulphuric acid Hazcard 32 - Indicators Implementing Mass of glass weighing bottle = 50.08 grams Mass of weighing bottle and sodium Carbonate = 52.73 grams Mass of Sodium Carbonate = 2.65 grams I work out the mass ...read more.

Conclusion

To try and see when the solution turned pink I used a white tile underneath the conical flask. Basically I cannot tell the exact point when the solution turns into a pinky colour. This meant that each titration would not be exactly the same so wouldn't be a fair test. To improve this I could use computer and real time video recording because this would be far more reliable and accurate than my recording would be. The computer could save the colour of the original titration, and then the second titration could be done whilst someone is looking at the computer screen so they could see the exact point when the titration should be stopped. Another problem with my experiment was that I might not have shaken the conical flask particularly well when I was trying to dissolve the Sodium Carbonate in the distilled water. To make my results more interesting to analyse I could have done more titrations, this would mean I'd obtain a better average result and so I could find out a more precise answer for the concentration of the sulphuric acid. The exact answer to the concentration of the sulphuric acid was 0.099 (2 decimal places), but I have rounded this figure up to 0.1 mols dm-3, as I believe it takes into account the possibility of a percentage error. Finding out how much acid is in a solution Alex Pitt 1 ...read more.

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