Internal Assessment
Narki SACKEY IB1B
Topic: Acid-Base Titration
Aims:
1. To use methyl orange and phenolphthalein as indicators to determine accurately the end of an acid-base titration. 2. To present titration data correctly.
Observations:
Table of Results Showing The Amount Of 0.12 Mol/dm3 Hydrochloric Acid Required to Neutralise 25cm3 Of Sodium Carbonate of an unknown Concentration Using Methyl Orange Indicator. Pipette Solution | Sodium Carbonate | Mol/dm3 | Burette Solution | Hydrochloric Acid | 0.12Mol/dm3 | Indicator | Methyl Orange | | | | Trial 1 | Trial 2 | Trial 3 | Burette readings | Final/cm3 ± 0.05 | 14.80 | 14.50 | 14.60 | | Initial/cm3 ±0.05 | 0.00 | 0.00 | 0.00 | Volume Used (titre)/cm3±0.10 | | 14.80 | 14.50 | 14.60 | Mean Titre/cm3 ±0.05 | | 14.63 |
* The sodium chloride and hydrochloric acid solutions were both colourless at the start of the experiment. * When methyl orange was added to the sodium chloride, it turned orange. * As the hydrochloric acid was added to the solution in the conical flask, its colour began to change to pink. * When the solution was swirled, it became orange again. At the end point, the solution turned from orange to pink.
Calculations
2HCl + Na2CO3 -> 2NaCl + CO2 + H2O
Therefore, mole ratio of Hydrochloric Acid to Sodium Carbonate is 2:1
Percentage uncertainty of volume of HCl = 0.10/14.63 * 100 = 0.68%
Percentage uncertainty of volume of Na2CO3 = 0.06/25 * 100 =0.24%
Number of moles of sodium carbonate = 1
Number of moles of Hydrochloric acid 2
Therefore, moles of sodium carbonate = 0.5 *0.12 = 0.6Mols
Concentration of Na2CO3 = Moles of sodium carbonate Volume of Sodium Carbonate =
Topic: Acid-Base Titration
Aims:
1. To use methyl orange and phenolphthalein as indicators to determine accurately the end of an acid-base titration. 2. To present titration data correctly.
Observations:
Table of Results Showing The Amount Of 0.12 Mol/dm3 Hydrochloric Acid Required to Neutralise 25cm3 Of Sodium Carbonate of an unknown Concentration Using Methyl Orange Indicator. Pipette Solution | Sodium Carbonate | Mol/dm3 | Burette Solution | Hydrochloric Acid | 0.12Mol/dm3 | Indicator | Methyl Orange | | | | Trial 1 | Trial 2 | Trial 3 | Burette readings | Final/cm3 ± 0.05 | 14.80 | 14.50 | 14.60 | | Initial/cm3 ±0.05 | 0.00 | 0.00 | 0.00 | Volume Used (titre)/cm3±0.10 | | 14.80 | 14.50 | 14.60 | Mean Titre/cm3 ±0.05 | | 14.63 |
* The sodium chloride and hydrochloric acid solutions were both colourless at the start of the experiment. * When methyl orange was added to the sodium chloride, it turned orange. * As the hydrochloric acid was added to the solution in the conical flask, its colour began to change to pink. * When the solution was swirled, it became orange again. At the end point, the solution turned from orange to pink.
Calculations
2HCl + Na2CO3 -> 2NaCl + CO2 + H2O
Therefore, mole ratio of Hydrochloric Acid to Sodium Carbonate is 2:1
Percentage uncertainty of volume of HCl = 0.10/14.63 * 100 = 0.68%
Percentage uncertainty of volume of Na2CO3 = 0.06/25 * 100 =0.24%
Number of moles of sodium carbonate = 1
Number of moles of Hydrochloric acid 2
Therefore, moles of sodium carbonate = 0.5 *0.12 = 0.6Mols
Concentration of Na2CO3 = Moles of sodium carbonate Volume of Sodium Carbonate =