Titrations & their CALCULATIONS

Titrations A titration is a laboratory technique used to find the concentration of a solution Titrations are used to measure the molarity of a solution using a standard solution. A Standard Solution is one with a precisely known concentration

Titration During a titration, the standard solution and solution with an unknown concentration A Burette is used to add on solution to another A burette can add a solution to another while carefully measuring the volume added If we know the volume added AND the concentration (from the standard solution) we can calculate the moles of reactant added

Titration We will only talk about acid-base titrations (mixing and acid and base) During an acid-base titration, an acid reacts with a base (a compound with OH-) in a double replacement reaction to form water

Titration Before titrating, an indicator is added to the solution. An Indicator changes colour when a reaction is neutralized Neutralized means the moles of acid and base are equal When the solution is neutralized, we call that the endpoint of the titration Since we can calculate the moles added and the moles of acid and base are equal, we can calculate the unknown.

Titration When performing a titration, it is important to reach the proper endpoint If you add too much, the moles you calculate will be wrong and you did a whole experiment for NOTHING!

Titration Calculations A titration calculation is a simple stoichiometric calculation. Follow the 4 steps: Balance the equation Go to moles Rebalance Go where it asks

Example 1: What volume of 0.32 M nitric acid is needed to neutralize 26 mL of 0.22 M calcium hydroxide solution?

Example 2: What volume of 0.80 mol/L KOH is needed to neutralize 15.0 mL of 0.65 M H2SO4?