Jan 30 2022 10 mins 1
All hydrohalic acids, but hydrofluoric acid, are strong acids. Why is that (0:31)? Strong acids fully dissociate and have a large Ka, weak acids only dissociate to a small percentage (1:20). When looking at strength, we are comparing the stability of the conjugate acid/base pair partners (2:00). For binary acids across a period (2:37) as well as down a group (3:09) electronegativity determines acid strength. For oxyacids, we can compare acids with different numbers of oxygen atoms, which affects the inductive effect, as well as resonance structures (4:58). We can also discuss acid strength across a period (6:44) and down a group (7:34). Bases are proton acceptors. Common bases are conjugate bases of weak acids, like carboxylic acids, and amines (7:53).
Question of the Day: Acid A has a Ka = 3.5 x 10-8, acid B has a Ka = 1.2 x 10-2. Which acid is HClO, which one is HClO2?
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