Titrations - Equivalence Point, End Point and Neutralisation Point (A-level Chemistry) 

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Great question! A weak acid against a strong base would normally give an equivalence point above pH7. For example, ethanoic acid, CH3COOH (a weak acid) and sodium hydroxide, NaOH (a strong base). At the equivalence point, all the original ethanoic acid molecules will have reacted and formed ethanoate ions, CH3COO-. However, these CH3COO- ions can form their own equilibrium with water molecules, reforming CH3COOH and releasing OH- ions. CH3COO- + H2O = CH3COOH + OH- The position of this equilibrium will be very far to the left however some OH- ions will still be present, meaning the solution will be slightly alkaline and have a pH above 7. Hope that helps :)

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Good question! This is because we can use the amount of acid or base added to reach equivalence to determine the amount of base or acid that must have been in the starting solution. By having the end point (point at which colour of indicator changes) and equivalence points (point at which all starting acid or base has been perfectly reacted) occur at the same time in the titration, we can use the end point as a visual indication that the equivalence point has been reached and then use this to determine amount of acid or base present at the start :) You may find the video on acid-base titrations useful as a general overview - ru-vid.com/video/%D0%B2%D0%B8%D0%B4%D0%B5%D0%BE-RiyD6syn-4s.html