Logged out
Access All our Essays in an Instant
Swap your work for FREE access, or pay £4.99 for instant access
Assessed Practical Titration Write-up
Member rating: No Rating | Words: | Submitted: Wed Oct 05 2005
Page Preview
On the left is an image preview of every page of this document, and below are the first 150 words with formatting removed:
Assessed Practical Titration Write-up Equation: Na2CO3 + H2SO4 --> Na2SO4 + CO2 + H2O One mol of Na2CO3 reacts with one mol of H2SO4. Results: The weight of my sodium carbonate crystals was 2.67g and the results of the titrations are as follows: Rough 1st 2nd 3rd 4th 5th 6th Initial Reading 00.00 00.50 00.00 00.00 00.00 00.00 00.20 Final Reading 26.45 26.45 26.05 27.00 25.85 25.90 26.10 Titration 26.45 25.95 26.05 27.00 25.85 25.90 25.90 pH slightly acidic neutral slightly acidic slightly acidic slightly alkali neutral neutral So the average of the closest three titration results are is: 25.95 + 25.90 + 25.90 / 3 = 25.92 The mass of Na2CO3 I used is 2.67g and the relative molecular mass of Na2CO3 is 106. So the number of mols of Na2CO3 I used was: 2.67 / 106 = 0.0251 mols in 250 cm3 So the concentration of the Na2CO3 solution was: 0.1004 mol dm-3. So in the 25cm3 of Na2CO3 solution I used, there were: 0.0251 / 10 = 0.00251 mols. The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so 0.00251 mols of Na2CO3 reacts with 0.00251 mol of H2SO4. So in the 25.92...
To see the full version of this document, and 145,328 others
