Chemical quantities (AS)
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I am doing a titration to demonstrate that sulphuric acid is dibasic. I have an aqueous sulphuric acid of concentration 1.00 mol dm-3 but am unsure how to work out the volumes required for my experiment. I have the equation H2SO4 + 2Na2OH--> Na2SO4 + 2H2O...but am now stuck!
020608
Corrie writes ...
First of all, there is a slight mistake in your formula for sodium hydroxide - it should be NaOH, though it does not alter the ratio in which sulphuric acid and sodium hydroxide react in your equation, i.e. 1:2.
Your equation shows sulphuric acid acting as a dibasic acid, i.e. losing two H+'s per H2SO4. So, if you titrated a measured volume, say 25 cm3 , of it with 1.0 mol dm-3sodium hydroxide solution, then you should need twice the volume of NaOH solution to reach the end-point. If only an equal volume was needed, then each mole of sulphuric acid would be reacting with only 1 mole of NaOH, so it would be reacting as a monobasic acid.
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updated: 08 June 2008
