In the other side, Endpoint is a point where the symbol changes colour. ↩ Before the equivalence point the titration mixture’s pH is determined by a buffer of acetic acid, CH 3 COOH, and acetate, CH 3 COO –. The equivalence point of a titration. In the case of titration of weak acid with strong base, pH at the equivalence point is determined by the weak acid salt hydrolysis. A point of equivalence in a titration refers to a point at which the added titrant is chemically equivalent to the sample analyte. using conductivity to find an equivalence point: name: brianna thompson date: november 2nd 2016 lab section: 221 provide brief statement of the purpose of this The equivalence point (stoichiometric point) should be distinguished from the titration endpoint (where the indicator changes its color). ↩ CO 2 is an abbreviation for the composite carbonic acid H 2 CO 3 *, which is the sum of dissolved CO 2 (aq) and a tiny amount of true carbonic acid H 2 CO 3. Both are not exactly the same. In some cases there are multiple equivalence points which are multiples of the first equivalent point, such as in the titration of a diprotic acid. Equivalence point in titration specifically in acid- base titrations , mole of base is equal to mole of acid and indicates that the solution contains only salt and water. When the indicator changes colour, this is often described as the end point of the titration. Equivalence point is the point where the amount of titrant added is just enough to completely neutralise the analyte solution. That means we have to find pK b of conjugated base and calculate concentration of OH - starting from there, then use pH=14-pOH formula. Equivalence point or stoichiometric point occurs during a chemical titration when the amount of titrant added is equivalent, or equal, to the amount of analyte present in the sample. When you carry out a simple acid-base titration, you use an indicator to tell you when you have the acid and alkali mixed in exactly the right proportions to "neutralise" each other. Sorting out some confusing terms. Although we can easily calculate a buffer’s pH using the Henderson–Hasselbalch equation, we can avoid this calculation by making a simple assumption.