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Edexcel | Chemistry WCH0 | W 19 5 1 | 1 hour 45 minutes
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19
(a) (I)
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1 Mark

The reaction between iron(II) ions and manganate(VII) ions was investigated by

setting up a cell.

Solution A contains both iron(II) and iron(III) ions.

 Identify the substance used for the electrodes.

 X .............................................................................................

   Y .............................................................................................

X: Platinum / Pt((s)) and

Y: Platinum / Pt((s))

19
(a) (II)
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2 Mark s

A student suggested that, for standard conditions, solution A should be

made by mixing equal volumes of 1 mol dm  iron(II) sulfate solution and

1 mol dm iron(III) sulfate solution.

This mixture is not suitable for measuring the standard electrode potential of 

this cell.

State how this mixture should be changed.  Justify your answer.

19
(a) (III)
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2 Mark s

 Identify the compounds that may be used to make solution B

Potassium manganate((VII))/

potassium permanganate/ KMnO4

(1)

Manganese(II) sulfate/ MnSO4

(and (dilute) sulfuric acid / H2SO4)

ALLOW

Manganese(II) nitrate/ Mn(NO3)2

Manganese(II) chloride/ MnCl2

(1)

IGNORE

MnO4− , H+ , Mn2+, H2O, “acidified” Dilute hydrochloric acid/ HCl

19
(a) (IV)
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2 Mark s

A student suggested that the salt bridge could be made by soaking a strip of

filter paper in barium nitrate solution.

   A reaction occurs when this salt bridge comes into contact with iron(II) sulfate

in solution A.

   State what observation would be made and write the ionic equation for this

reaction. Include state symbols.

Observation:...........................................

19
(a) (V)
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1 Mark

Suggest a more suitable compound to use when making the salt bridge.

 

19
(a) (VI)
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1 Mark

 Calculate  for the cell.  Use the data on page 17 of the Data Booklet.

 

19
(b) (I)
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2 Mark s

A 3.00 g sample of powdered haematite contains iron(III) oxide, , as the

only iron compound.  It was dissolved in dilute sulfuric acid forming a solution of

iron(III) sulfate.

THE(aq) was reduced to  (aq) using a solution of sulfur dioxide   

The resulting solution was made up to 250.0 cm  The resulting solution was made up to 250.0 cm

25.00 cm portions of this solution were titrated with

  0.0250 mol dm potassium manganate(VII) solution.

  The mean titre was 24.50 cm

Explain why the solution of sulfur dioxide is suitable for reducing the iron(III) ionsUse the electrode potentials on page 15 of the Data Booklet.

19
(b) (II)
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4 Mark s

Calculate the percentage, by mass, of iron(III) oxide in this sample of

haematite.

19
(b) (III)
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2 Mark s

Iron(II) sulfate can be oxidised by dichromate(VI) ions in acid conditions. 

Use the half equations for the oxidation of iron(II) ions and the reduction of

dichromate(VI) ions to write the overall ionic equation for the reaction.

   State symbols are not required.

 

19
(b) (IV)
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1 Mark

Suggest a practical reason why potassium manganate(VII) is preferred to

potassium dichromate(VI) for use in titrations with iron(II) sulfate.

The colour change at the end point with manganate(VII) is clearer / more distinct / more obvious

OR

With dichromate(VI) the end point would not be a clear change /

would be from greenish yellow to yellowish green

ALLOW

MnO4— does not need an indicator/ is self indicating

Any reasonable colours

IGNORE

Potassium dichromate is toxic/

Is more expensive/

Is a better oxidising agent/

Has a higher Eo value

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