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Experiment to determine the concentration of sulphuric acid

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Introduction

Experiment to determine the concentration of aqueous Sulphuric acid Method 1 - Using Titration to determine the concentration of aqueous Sulphuric acid I am going to use a titration to work out the concentration of a solution of aqueous sulphuric acid. I will be given a solution of aqueous sulphuric acid that has a concentration of approximately 10 mol dm-� so I will dilute this. Also an aqueous solution of sodium hydroxide with concentration of 0.100 mol dm-� will be used. The neutralization reaction will occur between the two chemicals and the indicator methyl orange will be used to show when the reaction is over. Safety Goggles should be worn to protect eyes from irritant substances. Burette will be places somewhere below eye level when sulphuric acid is poured in. Gloves are worn to avoid the contact between hands and corrosive, irritant and toxic substances. Equipment Sulphuric acid (10 mol dm-� ) Aqueous sodium hydroxide (0.100 mol dm-� ) Methyl Orange Indicator. Funnel Burette Pipette and Filler Conical flask White tile Distilled water Clamp Stand Reaction H SO + 2NaOH NaSO + H O Procedure Looking at the reaction, for every one mole of sulphuric acid, there are 2 moles of sodium hydroxide. ...read more.

Middle

This is done until the solution in the conical flask turns pink. The volume on the burette is now recorded. This volume minus the starting volume gives you the volume used in the experiment. This procedure is repeated until there are three results within 0.1 cm� of each other. The average of these results are taken and is used in the final calculation. Diagram Reaction H SO + NaOH NaSO + H O Calculation to find the concentration Moles of sodium hydroxide are worked out first using: Moles = concentration x Volume Than the ratio of moles is worked out to find moles of sulphuric acid 1:1 So moles of sulphuric acid are the same as moles of sodium hydroxide. To work out concentration Concentration = Moles Volume Method 2-Using Gas collection to determine the concentration of sulphuric acid. I am going to determine the concentration of sulphuric acid by finding out how much gas will be produced from the reaction between magnesium carbonate and a certain volume of sulphuric acid. The concentration of sulphuric acid given is 10 mol dm-� so I will need to dilute this down. Gas will be collected in a burette and when no more gas is produced, the volume in the burette can be used to work out the concentration of the sulphuric acid. ...read more.

Conclusion

A bung is put on top of the dividing flask after a rubber delivery tube is placed inside the divided flask. A burette is held by a clamp and stand with the burette placed upside down in the trough . A trough is filled with distilled water until the distilled water reaches almost 0.00 cm� on the burette. This volume on the burette is recorded The end of the rubber delivery tube is placed inside the burette. The reactants are now allowed to mix. When the gas production has stopped than the volume of gas in the burette can now be found out. This is done by recording the volume of water now and minusing this volume from the volume of water recorded at the start of the experiment. Repeat until 3 results are 0.1cm� within each other. Reaction H SO + MgCO MgSO + H O + CO Calculation to work out the concentrations. Moles = Volume is to work out the moles of the carbon dioxide 24000 Than to work out the moles of sulphuric acid the ratio of moles of sulphuric acid and carbon dioxide is worked out 1:1 So to work out the concentration Concentration = Moles Volume Calculation from specimen titration experiment Reference Adams grammar A level chemistry experimental skills booklet- page 4 The website http://pubs.acs.org/cgi-bin/abstract.cgi/iecac0/1942/14/i07/f-pdf/f_i560107a025.pdf?sessid=2640 ...read more.

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