SQA National 5 Chemistry Titrations
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Titrations are a laboratory method of quantifying the concentration of a solution.
This is a diagram of a titration set up.
The result of the titration can be used to calculate the previously unkown concentration of the solution. Using the known volume and concentration from the titrant, and the ratio of moles between the two solutions in a neutralisation reaction, the concentration of the solution can be found.
Titration with a weak acid, (e.g. CH₃COOH) and a strong base (e.g. NaOH) would give a titration curve. In the case where one of either acid or base is weak, and the other is strong then the equivalence point is not at pH 7.
During titrations, acid-base indicators are used to indicate a neturalisation reaction has taken place. The acid and base forms of the indicator have different colours thus a colour change indicates the reation change.
In a titration, 25.00 cm³ of sodium hydroxide acid (0.100 mol/dm³) is neutralised by 20.00 cm³ of dilute hydrochloric acid. Calculate the concentration of the hydrochloric acid to 3 decimal places.
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