In: Chemistry
Titration question:
How do I calculate the mass of Na2CO3 and NaHCO3 in the initial (250mL) solution?
-The titrant is .09522 M HCl
-An unknown solution containing a Na2CO3 & NaHCO3 mixture is being titrated
-The unknown solution was made using 2.3051g of the mixture in 250mL of CO2-free water and a 25mL aliquot of this solution is what is being titrated.
-Bromocresol green indicator was used
-The first equivalence point occurred when 19.81mL titrant was added
-The second equivalence point was added when 42.84mL of titrant was added
When a mixture of Na2CO3 & NaHCO3 is titrated against HCl the following reactions take place:
1st -
This reaction gives the first equivalence point.
2nd -
This reaction gives the second equivalence point.
The volume of HCl required to reach the 1st equivalence point is 19.81ml (0.09522M)
Therefore moles of HCl used = Molarity x Volume = 0.09522 x 19.81 = 1.8863 mmoles
Since one mole of HCl requires one mole Na2CO3, moles of Na2CO3 present in 25ml of aliquot = 1.8863 mmoles
Moles of Na2CO3 present in 250ml = 18.863 mmoles
Mass of Na2CO3 in 250ml = 18.863 x 106 = 1999.5 mg = 1.9995 gms
You can calculate mass of NaHCO3 in the foloowing ways:
This volume of HCl is used to neutralize NaHCO3 (from Na2CO3 and the one initially present)
Moles of HCl used = Molarity x Volume = 0.09522 x 23.03 = 2.1929 mmoles
Hence moles of NaHCO3 present = 2.1929 moles
Of this 1.8863 mmoles is obtained from Na2CO3 during 1st reaction, therefore NaHCO3 present in 25ml aliquot = 2.1929 - 1.8863 = 0.3066 mmoles
Hence NaHCO3 in 250ml solution = 3.066 mmoles
Mass of NaHCO3 = 3.066 x 84 = 257.54 mg = 0.2575 gms
2. Since mass of the mixture is 2.3051 gms and mass of Na2CO3 calculated is 1.9995 gms, remaining amount should be NaHCO3
Mass of NaHCO3 = 2.3051 - 1.9995 = 0.3056 gms
P.S:- The slight error in mass of NaHCO3 from the two methods may be attributed to calculation error due to approximation.