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*Chemistry: Experiments > Q1. * Estimation of iron in an iron tablet > Flashcards

Q1. * Estimation of iron in an iron tablet Flashcards

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1
Q

What exactly is being measured in this experiment?

A

The amount of iron (II) sulfate (FeSO4) in an iron tablet

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2
Q

What does FeSO4 stand for?

A

Iron (II) sulfate

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3
Q

What is the chemical formula for iron (II) sulfate?

A

FeSO4

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4
Q

What chemicals are needed for this experiment?

3

A

Potassium permanganate solution (0.01 M approximately)

Sulfuric acid solution (1 M)

Deionised water

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5
Q

What is the first step in the procedure?

2

A

Accurately find the mass of five iron tablets using a clock glass and electronic balance

If in capsule form - empty the contents from five capsules onto a clock glass and find the mass

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6
Q

What should be used to find the mass of the iron tablets?

2

A

A clock glass

An electronic balance

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7
Q

How many iron tablets are needed for this experiment?

A

Five tablets are needed

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8
Q

What must be done if the iron tablets are in capsule form before measuring?

A

Empty the contents of five capsules onto a clock glass then measure using an electronic balance

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9
Q

What is the second step in the procedure, the mass of five iron tablets has just been found?
(2)

A

Grind up the tablets using a pestle and mortar

Add about 5 cm cubed of 1M sulfuric acid to the mortar to make the grinding process easier

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10
Q

What is used to grind up the iron tablets?

A

A pestle and mortar

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11
Q

What can be added to the mortar to make the grinding process easier?

A

Approximately 5cm cubed of 1M sulfuric acid

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12
Q

What is the third step in the procedure, the iron tablets have just been ground up with5cm cubed of 1M sulfuric acid?
(2)

A

Transfer the paste of acid and tablets to a beaker containing about 100 cm cubed of 1M sulfuric acid

Make sure to rinse the mortar and pestle to ensure all traces of the tablets have been transferred to the beaker

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13
Q

What is the paste of acid and tablets transferred to?

A

A beaker containing about 100cm cubed of 1M sulfuric acid

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14
Q

What molar sulfuric acid is used during this experiment?

A

1M

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15
Q

When transferring the paste, what must you make sure to remember to do?

A

Make sure to rinse the mortar and pestle

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16
Q

When transferring the paste, why do you need to make sure to rinse the mortar and pestle?

A

To ensure all traces of the tablets have been transferred to the beaker

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17
Q

What is the fourth step in the procedure, the paste has been transferred to a beaker of 100cm cubed sulfuric acid?
(2)

A

Stir to dissolve the paste

The outer coating may not dissolve which may give the solution a cloudy appearance

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18
Q

When stirring the sulfuric acid containing the paste, what may occur?

A

The solution may become cloudy

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19
Q

Why may the solution of sulfuric acid and the iron tablet paste become cloudy?

A

As some iron tablets have an outer coating which may not dissolve thus creating a cloudy appearance

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20
Q

Why do some iron tablets have an outer coating?

A

To reduce the rate at which they dissolve in the stomach which reduces the chance of stomach upset

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21
Q

What is the fifth step in the procedure, the solution of sulfuric acid and paste has been stirred and the solution has turned cloudy?
(3)

A

Transfer the solution to a clean 250 cm cubed volumetric flask

Transfer all the washings to the volumetric flask and make up to the mark with deionised water

Invert the stoppered flask about 20 times

22
Q

What should the 100m sulfuric acid solution and dissolved paste be transferred to?

A

A clean 250cm cubed volumetric flask

23
Q

What should you remember to do when transferring the dissolved paste and sulfuric acid solution?

A

Remember to transfer all the washings from the beaker to the volumetric flask

24
Q

What should you use to make the sulfuric acid solution and dissolved paste up to the mark on the volumetric flask?

A

Use deionised water to make the solution up to the 250cm cubed mark on the volumetric flask

25
Q

How many times should the flask be inverted?

A

Approximately 20 times

26
Q

What is the sixth step in the procedure, the volumetric flask has just been inverted 20 times.

A

Wash out a pipette, burette and conical flask with deionised water

27
Q

What pieces of equipment need to be washed with deionised water?
(3)

A

A pipette

A burette

A conical flask

28
Q

What does the pipette, burette and conical flask need to be washed out with?

A

Deionised water

29
Q

What is the seventh step in the procedure, the equipment for the titration has just been washed with deionised water?
(6)

A

The burette needs to be washed out with some of the potassium permanganate solution

Then fill the burette using a funnel with the potassium permanganate solution until it is above the zero mark

Remove the funnel from the burette

Adjust the level of the solution in the burette to the zero mark

Read from the top of the meniscus

Ensure that the tap and space below the tap are also filled with the solution

30
Q

What does the burette need to be washed out with?

A

Some potassium permanganate solution

31
Q

What should be used when filling the burette with the potassium permanganate solution?

A

A funnel

32
Q

How should the burette be filled?

5

A

Using a funnel add potassium permanganate solution until it is above the zero mark

Remove the funnel

Adjust the level of the solution to the zero mark

Read from the top of the meniscus

Ensure that the tap and space below it are filled with the solution

33
Q

How should the meniscus of the potassium permanganate solution in the burette be read?

A

Read from the top of the meniscus

34
Q

What is step 8 in the procedure, the burette has just been filled with potassium permanganate?
(3)

A

Pour approximately 100 cm cubed of the iron tablet and sulfuric acid solution into a clean dry beaker

Wash out the pipette with a small amount of this solution

Pipette 25 cm cubed of the solution into the conical flask

35
Q

How much of the solution (sulfuric acid and iron tablet paste) in the volumetric flask should be poured into a beaker?

A

Approximately 100 cm cubed

36
Q

What should the pipette be washed out with?

A

The sulfuric acid and iron tablet paste solution

37
Q

How much of the iron tablet and sulfuric acid solution needs to be pipetted into a conical flask?

A

Approximately 25 cm cubed

38
Q

Where is the sulfuric acid and iron tablet solution pipetted to?

A

A conical flask - which will be used during the titration

39
Q

What is step 9 in the procedure, the conical flask has been filled with 25cm cubed of sulfuric acid and iron tablet solution?

A

Using a graduated cylinder add approximately 20 cm cubed of dilute sulfuric acid to the conical flask

40
Q

How much dilute sulfuric acid needs to be added to the graduated cylinder?

A

Approximately 20 cm cubed

41
Q

What needs to be added to the conical flask of sulfuric acid and iron paste solution?

A

Approx. 20 cm cubed dilute sulfuric acid

42
Q

What is step 10 in the procedure, dilute sulfuric acid has just been added to the conical flask?
(3)

A

Carry out the titration until a faint permanent pink colour is observed at the end point

Perform one rough and two accurate titrations

The two accurate titrations should agree to within 0.1 cm cubed

43
Q

How do you know the end point has been reached?

A

A faint permanent pink colour is observed

44
Q

How many titrations should be carried out?

A

One rough and two accurate titrations

45
Q

Within how much should the two accurate titrations agree with each other?

A

Within 0.1 cm cubed

46
Q

What is step 11, in the procedure, the three titrations have been carried out?

A

Ensure that all glassware is washed out when the titrations have been finished as potassium permanganate stains glassware

47
Q

What is the chemical formula for potassium permanganate?

A

KMnO4

48
Q

What is KMnO4?

A

Potassium permanganate

49
Q

Why does glassware need to be washed when the titrations are over?

A

As potassium permanganate stains glassware

50
Q

What is the final step in the experiment?

A

Use the results of the experiment to calculate the mass of iron (II) sulfate in each tablet

*Chemistry: Experiments (15 decks)

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