Methyl Orange

In this experiment the initial mass of the sodium carbonate used was 2.69g. In each titration, 3 drops of methyl orange was added to the sodium carbonate solution. With this information the titration can begin, and the results obtained are shown below:

Titration readings

Titration Rough 1 2 3 4 5
Initial 0.00 4.30 22.00 21.00 15.00 25.90
Final 4.30 22.00 38.60 37.60 32.60 42.20
Titre (cm3) 4.30 17.70 16.60 16.60 17.60 16.30

Therefore, the average titre would be calculated as follows; all the titre measurements added together (not including the rough titre), and divide this amount by the total number of titrations taken. In this case, I am only going to find the average titre of 3 of the results because to have successive measurements, the titrations have to be within 0.1 of each other, and in this case it was for only 3 of the results shown above. The average titre is shown below:

16.60 + 16.60 + 16.30 = 49.50 / 3 = 16.5cm3

Going back to the beginning the equation for the reaction that is taking place is as follows:

Na2CO3 (aq) + H2SO4 (aq)  Na2SO4 (aq) + CO2 (g) + H2O (l)

Concentration of sodium carbonate solution

In this experiment, a solution carbonate had to be made. This was done by mixing sodium carbonate with distilled water, to get the desired solution. The mass of the sodium carbonate used here was 2.69g. In order to find out the concentration of sodium carbonate used, the number of moles used need to be worked out first.

1. The equation for finding the number of moles is as follows:
• Amount of Na2CO3 (mol) = mass (g) / molar mass (g mol-1)
• The mass is 2.69g and the molar mass of Na2CO3 is [(26 x 2) + 12 + (16 x 3)]
• = 106 g mol-1
• Therefore, 2.69 / 106 = 0.0253mol

We can now use this number of moles to find the concentration of sodium carbonate used in solution.

2. The equation for finding the concentration of a solution is as follows:
• Concentration