Titration Calculations (Cambridge (CIE) O Level Chemistry): Revision Note
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Titration Calculations
Titrations are a method of analysing the concentration of solutions
Acid-base titrations are one of the most important kinds of titrations
They can determine exactly how much alkali is needed to neutralise a quantity of acid – and vice versa
You may be asked to calculate the moles present in a given amount, the concentration or volume required to neutralise an acid or a base
Once a titration is completed and the average titre has been calculated, you can now proceed to calculate the unknown variable using the formula triangle as shown below
Formula triangle showing the relationship between concentration, number of moles and volume of liquid
Worked Example
A solution of 25.0 cm3 of hydrochloric acid was titrated against a solution of 0.100 mol/dm3 NaOH and 12.1 cm3 were required for complete reaction. Determine the concentration of the acid.
Answer
Step 1: Write the equation for the reaction:
HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
Step 2: Calculate the number of moles of the NaOH
Moles = (volume ÷ 1000) x concentration
Moles of NaOH = 0.012 dm3 x 0.100 mol/dm3 = 1.21 x 10-3 mol
Step 3: Deduce the number of moles of the acid
Since the acid reacts in a 1:1 ratio with the alkali, the number of moles of HCl is also 1.21 x 10-3 mol
This is present in 25.0 cm3 of the solution (25.0 cm3 = 0.025 dm3)
Step 4: Find the concentration of the acid
Concentration = moles ÷ volume (dm3)
Concentration of HCl =1.21 x 10-3 mol ÷ 0.025 dm3 = 0.0484 mol/dm3
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