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Acids, alkalis and titrations

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Question 15

An analytical chemist carries out a titration to determine the volume of sodium hydroxide solution needed to neutralise a sample of sulfuric acid.

She pipettes 30.0 cm330.0\text{ cm}^330.0 cm3 of sulfuric acid of concentration 0.125 mol/dm30.125\text{ mol/dm}^30.125 mol/dm3 into a conical flask.

She then titrates this against a 0.200 mol/dm30.200\text{ mol/dm}^30.200 mol/dm3 sodium hydroxide solution until the sulfuric acid is completely neutralised.

The equation for this reaction is:

H2SO4+2NaOH→Na2SO4+2H2O \text{H}_2\text{SO}_4 + 2\text{NaOH} \rightarrow \text{Na}_2\text{SO}_4 + 2\text{H}_2\text{O} H2​SO4​+2NaOH→Na2​SO4​+2H2​O
a.

Calculate the amount, in moles, of sulfuric acid used.

[2]
b.

Calculate the amount, in moles, of sodium hydroxide needed to neutralise this amount of sulfuric acid.

[2]
c.

Calculate the volume, in cm3\text{cm}^3cm3, of sodium hydroxide solution needed to neutralise this amount of sulfuric acid.

[2]

Acids, alkalis and titrations Questions

  1. IGCSE
  2. /Chemistry
  3. /Acids, alkalis and titrations