Finding the Exact Concentration of Sulphuric Acid in a Solution Through a Titration

Finding the Exact Concentration of Sulphuric Acid in a Solution Through a Titration

Aim: To find the exact concentration of sulphuric acid in a solution

through a titration. The titration is between sulphuric acid and

sodium carbonate has to be in liquid for in order to carry out the

experiment so it is dissolved into distilled water to a concentration

of 0.1 mol dm³

Introduction-

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During the extraction of a metal from its ore, sulphuric dioxide is

often produced. This is converted to sulphuric acid and is sold as a

useful by-product. I am going to be given a sample of sulphuric acid,

which is thought to have a concentration between 0.05 and 0.15-mol

dm³.

The purpose of this experiment is to find the accurate concentration

of the sulphuric acid. I will do this by carrying out a titration

between sulphuric acid and sodium carbonate solution. Therefore this

is an acid-alkali titration (which is the determination of

concentration by adding measured amounts of standard reagents to a

known volume until the end point is reached).

* Sulphuric acid is considered a strong acid, as it is completely in

the form of ions in dilute solution.

* Sodium carbonate is a weak alkali as it only partially forms ions

in dilute solution.

* For this titration methyl orange is the best indicator for the end

point between a strong acid and weak alkali.

[IMAGE]Na2CO3 (aq) + H2SO4 (aq) Na2SO4 (aq) + CO2 (g)

* One mole of sodium carbonate is needed to neutralise one mole of

sulphuric acid so it in a 1:1 ratio for moles

APPARATUS AND EQUIPMENT

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Chemicals used

Amount

Sodium carbonate

2.65g

Methyl orange

3 drops

Sulphuric acid

Will vary in total