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Redox Titrations (OCR)

Authored by Kitty Murdoch

Science, Chemistry

11th - 12th Grade

Used 3+ times

Redox Titrations (OCR)
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5 questions

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1.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

24.3 cm3 of 0.0200 mol dm-3 KMnO4 reacted with 20.0 cm3 of an iron(II) solution in the presence of sulfuric acid. Calculate the concentration of the iron(II) ion.

Ratio MnO4-:Fe2+ is 1:5

0.122 mol dm-3

0.0243 mol dm-3

2.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

3.00 g of a lawn sand containing an iron(II) salt was shaken with dilute H2SO4. The resulting solution required 25.00 cm3 of 0.0200 mol dm-3 potassium manganate(VII) to oxidise the Fe2+ ions in the solution to Fe3+ ions. Use this to calculate the percentage by mass of Fe2+ ions in this sample of lawn sand.

Ratio MnO4-: Fe2+ is 1:5

4.65%

0.93%

3.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Calculate x in the formula FeSO4.xH2O from the following data: 12.18 g of iron(II) sulfate crystals were made up to 500 cm3 acidified with sulfuric acid in a volumetric flask. 25.0 cm3 of this solution required 43.85 cm3 of 0.0100 mol dm-3 KMnO4 for complete oxidation.

Ratio MnO4- : Fe2+ is 1:5

7

69

300

6.5

4.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

A tablet with mass 0.940 g was dissolved in dilute sulfuric acid made up to 250 cm3 with water. 25.0 cm3 of this solution was titrated with 0.00133 mol dm-3 KMnO4 requiring 32.5 cm3 of the KMnO4. Calculate the percentage by mass of Fe2+ in the tablet.

Ratio MnO4- : Fe2+ is 1:5

12.8%

2.57%

1.28%

25.7%

5.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

13.2 g of iron(III) alum were dissolved in water and reduced to an iron(II) ion solution by zinc and dilute sulfuric acid. The mixture was filtered and the filtrate and washings made up to 500 cm3 in a standard volumetric flask. 20.0 cm3 of this solution required 26.5 cm3 of 0.0100 mol dm-3 KMnO4 for oxidation. Calculate the percentage by mass of iron in iron alum.

Ratio MnO4- : Fe2+ is 1:5

14.0%

2.8%

0.56%

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