CHEM 11b Lecture Notes - Lecture 17: Conjugate Acid, Electronegativity, Oxoacid
Document Summary
Acid: a substance that produces h+ ions (protons) in water. Base: a substance that produces oh- ions in water. Acids combine naturally with bases to neutralize each other and form water. A strong acid ionizes completely into protons (h+ ions) and accompanying anions. A weak acid undergoes a reversible reaction with water to ionize only partially. Strong bases are ionic compounds in which the anion is oh-. Amphiprotic and amphoteric means it can be a proton donor and acceptor. Double arrow means the reaction will come to equilibrium because it is reversible. Every bronsted lowry model has two sets of acid-base pairs. Strong acids ionize completely and strong bases dissociate completely. Weak acids and bases only partially ionize in water. Auto-ionization of water = most water is just water but is can have some proton transfers. *dont include liquids or solids when solving for k. [h3o+] = [oh-] = 1. 0 10-7 m (at 25 c)