The tablet was so titrated with 0.10 mol dm-A? Na hydrated oxide solution utilizing two beads of phenolphthalein solution as an index. The burette used had an uncertainness of A± 0.10 cmA? ( mentioned on the setup ) . The colour alteration of the index to tap marked the end-point of the reaction and it allowed me to observe the volume required of NaOH solution.

The uncertainness of volume used of NaOH solution is found by adding the uncertainness of the initial and concluding readings of the NaOH solution used for titration.

Processing Raw Data & A ; Showing it

Bayer Aspirin Cardio

Note: The absolute values for mole and mass are taken frontward in the computation till the terminal consequence where the reply is so expressed in the right figure of denary topographic points.

Average volume of NaOH solution used = ( 7.00 + 7.10 ) / 2

= 7.05 cm3

Uncertainty of the mean volume of NaOH solution is found by adding the uncertainnesss of the initial and concluding readings taken.

= A± 0.10 + A± 0.10

= A± 0.20 cm3

Uncertainty in % of the NaOH solution used = ( 0.20/7.05 ) X 100

= 2.8368 %

= 2.84 %

Gram molecules of NaOH = Concentration X Volume

= 0.10 mol dm-A? Ten 7.05 A± 0.20 cmA?

= 0.10 mol dm-A? Ten 0.00705 dm3 A±2.84 %

= 0.000705 A±2.84 %

C6H5 ( OCOCH3 ) COOH + NaOH i? C6H5 ( OCOCH3 ) COO-Na+ + H2O

Mole to mole ratio= 1:1

Gram molecules of C6H5 ( OCOCH3 ) COOH = 0.000705 A±2.84 %

Gram molecules = Mass / Mr

Mass = Moles X Mr

= 0.000705 A±2.84 % X 181.18

= 0.1277319 A±2.84 % g

Mass of tablet = 0.13 A± 0.01 g

Uncertainty % = ( Uncertainty of balance / Mass of tablet ) X 100

= ( 0.01 / 0.13 ) X 100

= A± 7.69 %

% of aspirin = ( Mass of Aspirin/ Mass of tablet ) X 100

= ( 0.1277319 A±2.84 % / 0.13 A± 7.69 % ) X 100

= 98.26 A± 10.53 %

Aspirin ASPAR

Note: The absolute values for mole and mass are taken frontward in the computation till the terminal consequence where the reply is so expressed in the right figure of denary topographic points.

Average volume of NaOH solution used = ( 18.20 + 18.30 ) / 2

= 18.25 cm3

Uncertainty of the mean volume of NaOH solution is found by adding the uncertainnesss of the initial and concluding readings taken.

= A± 0.10 + A± 0.10

= A± 0.20 cm3

Uncertainty in % of the NaOH solution used = ( 0.20/18.25 ) X 100

= 1.0958 %

= 1.10 %

Gram molecules of NaOH = Concentration X Volume

= 0.10 mol dm-A? Ten 18.25 A± 0.20 cmA?

= 0.10 mol dm-A? Ten 0.01825 dm3 A±1.10 %

= 0.001825 A±1.10 %

C6H5 ( OCOCH3 ) COOH + NaOH i? C6H5 ( OCOCH3 ) COO-Na+ + H2O

Mole to mole ratio= 1:1

Gram molecules of C6H5 ( OCOCH3 ) COOH = 0.001825 A±1.10 %

Gram molecules = Mass / Mr

Mass = Moles X Mr

= 0.001825 A±1.10 % X 181.18

= 0.3306535 A±1.10 % g

Mass of tablet = 0.34 A± 0.01 g

Uncertainty % = ( Uncertainty of balance / Mass of tablet ) X 100

= ( 0.01 / 0.34 ) X 100

= A± 2.94 %

% of aspirin = ( Mass of Aspirin/ Mass of tablet ) X 100

= ( 0.3306535 A±1.10 % / 0.34 A± 2.94 % ) X 100

= 97.25 A± 4.04 %

Conclusion & A ; Evaluation

Bayer Aspirin Cardio had stated that its commercial readying would hold approximately 100 milligrams ( 0.10 g ) of acetylsalicylic acid. Now harmonizing to my computations, their tablets had an mean mass of 0.13 A± 0.01 g and the % of aspirin nowadays in their tablets was 98.26 A± 10.53 % . Keeping in head the uncertainnesss involved, I can still state that they did hold 0.10 g of acetylsalicylic acid in their tablets. This statement of mine is based on the computations that if we take the mean mass to be the least possible value which is 0.12 g and if we take the % of aspirin nowadays besides to be the least possible value which is 87.73 % , the sum of aspirin nowadays would work out to be about 0.10 g.

Working

( 87.73/100 ) x 0.12 = 0.10 g

Aspirin Aspar had stated that its commercial readying would hold approximately 300 milligrams ( 0.30 g ) of acetylsalicylic acid. Now harmonizing to my computations, their tablets had an mean mass of 0.34 A± 0.01 g and the % of aspirin nowadays in their tablets was 97.25 A± 4.04 % . Keeping in head the uncertainnesss involved, I can still state that they did hold 0.30 g of acetylsalicylic acid in their tablets. This statement of mine is based on the computations that if we take the mean mass to be the least possible value which is 0.33 g and if we take the % of aspirin nowadays besides to be the least possible value which is 93.21 % , the sum of aspirin nowadays would work out to be about 0.30 g.

Working

( 93.21/100 ) x 0.33 = 0.30 g

Harmonizing to the above computations, I have reached the decision that to happen out which is the best value for money, I would hold to look at their market monetary value instead than the % of aspirin nowadays in them because they are about the same per centum. Bayer Aspirin Cardio was offering 30 tablets for Kenya Shillings 190. Thus the value of one tablet worked out to be Sh 6 a…“ . On the other manus, Aspirin Aspar was offering 100 tablets for Kenya Shillings 150. Thus the value of one tablet worked out to be Sh 1A? . Therefore purchasing Aspirin Aspar tablets made more economical sense.

An experimental mistake could be calculated for both the acetylsalicylic acids, but since the % of acetylsalicylic acid it contained was rather close to 100 % and besides maintaining in head the changing uncertainnesss involved, the experimental mistake value would be negligible.

The method was reasonably easy and straightforward. The mass of the tablet could hold changed from its original value during weighing, etc. because the tablet is made of pulverization which can acquire rubbed off easy. A systematic mistake was that the 10 cm3 pipette had a nothing mistake, a signifier of standardization. If an uncertainness was present, the concluding computations could hold been more accurate. The readings were largely precise which helped later in the computations. Multiple readings were taken and mean readings were processed when a difference of A±0.1 occurred so as to cut down the random mistakes. However human parallax mistake can be added to random mistakes.

When utilizing the pipette for mensurating and reassigning the intoxicant to the conelike flask, the pipette filler used for sucking in air was non tightly held by the pipette. Therefore this made the solution pour from the pipette once it was measured to its needed sum. To better on this, the pipette filler used to suck in the intoxicant should be decently fixed so that no air escapes from the pipette filler. Another mistake that could hold risen in the experiment is the alteration in the absolute value of the content of the conelike flask. This is because during stirring, some H2O might hold hung on to the side of the flask and when titrated, that value of solution might hold non been accounted for.

The setup used for the experiment was easy to run and put up. Time was managed good as the initial consequences obtained were within the A± 0.10 cm3 scope and therefore fewer repeats were needed.

One of the major premises made during the experiment was that the mass of the tablet weighed was the existent mass of the tablet. Another premise was that when the index colour changed to tap, at that exact minute the add-on of Na hydrated oxide solution was halted and this was repeated for the 2nd trade name of Aspirin excessively. These were the major failings in the computations as neglecting to obtain absolute values resulted in a concluding computation that lacked truth. Therefore although precise values were obtained, they might hold non needfully been accurate.

Certain alterations that could be made are that the burette could be washed with distilled H2O after every test and so rinsed with Na hydrated oxide solution. More truth could be obtained if the figures were non rounded up to two denary topographic points, but for the interest of uniformity, they were rounded up. Including an uncertainness for the 0.10 mol dm-3 Na hydrated oxide solution would besides help the overall truth of the computations.

If all setup had a declared uncertainness on them, the computations could go more accurate. Besides even if in the initial tests a difference of A± 0.10 cm3 is obtained for the needed Na hydroxide solution, more repeats could asseverate the exact value of the solution needed to bring forth the colour alteration of the index and therefore the overall random mistakes could be reduced.