CHM110H5 Lecture Notes - Hydronium, Lone Pair, Equivalence Point
Document Summary
Pre-lab questions: trifluoracetic acid will be stronger because it contains fluorine substitutes which are more electronegative than chlorine atoms. Since hf is a stronger acid than hcn (which can be inferred from the pka), hf will act as the proton donor and hcn will act as a base and accept the protons from hf. From the lewis structure of hcn, from hydronium will attach to the lone pair of electron and establish a bond. , it can be concluded that the extra proton: acid-base indicators are used to detect the equivalence points of a titration. They must be weak acid/base themselves and the hin (protonated form) and in- must have different colors. Also, the colors must be intense so that the concentration of the indicator can be low. The end point of the indicator should be close to the equivalence point of titration (especially important when one of the electrolytes is weak: ph = 5. 9.
