To look for the content of iron in iron tablets ...

METHODS:

Making a remedy of the tablets

1 . five iron tablets were acessed accurately, then dissolved in about 100cm3 of 1. 0 moldm-3 sulphuric acid within a conical flask. Some heat was needed, but not more than necessary required to dissolve the tablets.

2 . The blend was strained into a beaker, making sure that simply no solution was lost, then the conical flask was beaten up with normal water and the washings were put through the filtration.

3. Finally, distilled drinking water was poured over the remains and these types of washings we collected too.

The filtrate was then poured into a 250cm3 standard volumetric flask, washing out the beaker and adding washings to the standard flask. The mark was made up using distilled water.

Titration with Potassium Manganate (VII)

1. Using a pipette (safety) filler, 25cm3 of the iron (II) solution was pipette from the volumetric flask into a conical flask.

2. About 25cm3 of 1.0 moldm-3 sulphuric acid was added and titrated with 0.01 moldm-3 Potassium Manganate (VII) solution.

3. The experiment was repeated until two coincident results were obtained.

OBSERVATIONS, RESULTS, DATA:

Description

Initial Reading

Final Reading

Volume of HCl

Rough

0

12.5

12.5

First Titration

12.5

23.2

11.3

Second Titration

23.2

35.2

12.0

Average

7.5

15.3

7.7

TABLE SHOWING RESULTS OF IRON TABLET SOLUTION AND POTASSIUM MANGANATE (VII) TITRATION

CALCULATIONS:

To calculate the amount of iron dissolved in volumetric flask

Iron + sulphuric acid “>iron sulphate + hydrogen gas

Fe(s) + H2SO4(aq) “>FeSO4(aq) + H2(g)

Concerned with 1 mole of iron sulphate produced from 1 mole sulphuric acid

# of moles of H2SO4 = volume/1000 X concentration

= 100/1000 X 1.0

= 0.1 mol of H2SO4

1 mole iron sulphate produced from 1 mole sulphuric acid

x 0.1

hence x = 0.1 mol

volume of solution = 100cm3

volume of solution with water = 250cm3

dilution = 250/100 = 25

# of moles of FeSO4 = 0.1 x 25

= 2.5 moles of FeSO4 (original amount)

To calculate the amount of iron left over after titration

Iron + sulphuric acid “>iron sulphate + hydrogen gas

Fe(s) + H2SO4(aq) “>FeSO4(aq) + H2(g)

Concerned with

CONVERSATION:

CONCLUSION: The proportion of 2-ethanoylhydroxybenzoic acid (acetylsalicylic acid) in aspirin tablets was identified to be 51. 3%. The hydrolysis of aspirin tablets was as well successfully finished by using sodium hydroxide basic. The conclusions drawn aren’t as correct as expected due to the high big difference in percentage of acetylsalicylic acid content material found when compared with that provided.

Analyzing Flat iron Tablets

Examination: (M/M)

Tag Scheme

Considering

” No before considering [1]

Heating

” Usage of proper clothing (apron/goggles)

” Heat gradually

” readjusting flame to proper height/color

(any 2 ” one particular mark; every 3 ” 2 marks)

Measuring Volume

” Calculating Cylinder: On the flat Surface

examine bottom of meniscus [1]

” Volumetric flask: load to the draw [1]

Pipette: Rinse with required answer [1]

Feel top of pipette to surface liquefied [1]

Correct use of pipette filler [1]

” Burette: rinse with required solution

Use channel to load burette

Nozzle free of surroundings bubbles.

(any 3- one particular mark; any kind of 4- most 2 marks)

one particular