CHEM 001 Lecture Notes - Lecture 20: Hydronium, Nonmetal, Lone Pair
Document Summary
Strong acids produce more protons in solution than a weak acid due to the fact that they are almost all completely ionized in solution. Calculations involving strong acids and bases are easy because of this (we assume that they are 100% ionized) Ex: 0. 1m hcl(aq) implies 0. 1m h3o+ and 0. 1m cl-(aq) Weak acids are incompletely ionized in solution, you have to set up an equilibrium equation to calculate the concentrations. Ex: acetic acid only has a dissociation rate of about 1% Bases have a soapy feel (ex: detergent and soap) Water that feels soapy is alkaline due to soft salts. A base in water produces hydroxide ions (oh-) Ex: nh3(aq)+h2o(l) nh +(aq) + oh- (aq) remember that a lone pair donor is considered as a lewis base (usually these are weak bases like nh3, f-, technically the oh- ion is considered as a lewis base) Strong bases are completely ionized in water.