In this chapter of IBDP Chemistry, titration and its calcuations will be discussed. Let's check it below~

• A titration is used to measure accurately how much acid and alkali react completely together
• A pipette is used to accurately measure the volume of alkali put into a conical flask then an indicator is added to this
• In this chapter of IBDP Chemistry, a burette is filled with acid which is gradually added
• When the indicator changes colour the end point has been reached.
  • The volume of acid used is found from the initial and final burette reading
• Titration should be done several times for more accurate and reliable results

• Concentrations of solutions are measured in g/dm³ or mol/dm³
• In this chapter of IBDP Chemistry, if we know the mass or the number of moles of a substance dissolved in a given volume of solution we can calculate its concentration
• If we know the volume of a solution and its concentration we can calculate the mass or the number of moles of the substance in any volume of solution

• In this chapter of IBDP Chemistry, titrations are used to find the volumes of solutions that react exactly
• The concentrations are calculated using balanced symbol equations and moles

Worked example

A student found that 25.0cm³ of sodium hydroxide solution with an unknown concentration reacted with exactly 20.0cm³ of 0.50mol/dm³ hydrochloric acid. What was the concentration of the sodium hydroxide solution?

• The equation for this reaction is: NaOH_(aq) + HCl_(aq) → NaCl_(aq) + H₂O_(l)
• The concentration of the HCl is 0.50mol/dm³, so 0.50mol of HCl are dissolved in 1000cm³ of acid.
• Therefore 20.0cm³ of acid contains 20 x 0.50/1000mol = 0.010mol HCl
• The equation for the reaction tells us that 0.010mol of HCl will react exactly with 0.010mol of NaOH.
• This means that there must be 0.010 moles of NaOH in the 25.0cm³ of solution in the conical flask.
• So, the concentration of NaOH solution = (0.010/25) x 1000 = 0.40mol/dm³

In this chapter of IBDP Chemistry, the equations are

• Number of moles = mass in grams ÷ relative formula mass
• Number of moles = concentration x (volume ÷ 1000)
• Concentration = (Number of moles ÷ volume) x 1000

This is the end of this topic.

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