Acids increase H+ ions in aqueous solutions, bases increase OH- ions. Strong acids completely react with water, weak acids partially react. Common bases are ionic hydroxides, weak bases include ammonia
Dissociation constant measures propensity of larger objects to separate into smaller components. KD is inverse of association constant and can be called ionization constant for salts. KD equals concentration of free A at half of B molecules associated with A
Bases have three main definitions: Arrhenius, Brønsted, and Lewis bases. Arrhenius bases dissociate in water to form OH- ions. Brønsted bases accept protons in water solutions. Lewis bases donate electron pairs to accept protons
Synthesis reactions form one new compound from two reactants. Decomposition reactions break down compounds into simpler ones. Single replacement reactions replace parts of compounds to form new ones. Double replacement reactions exchange ions between compounds
Student attempted to balance CH3COOH + KOH → CH3COOK + H2O reaction. Student questioned why K+ doesn't form with CH3COO-. Student was confused about weak acid dissociation in solution
Hydroxide ion (OH-) is a negatively charged diatomic anion. Contains one hydrogen and one oxygen atom bonded covalently. Has valency of -1 and molecular weight of 17.003 g/mol. Conjugate acid is water, conjugate base is oxide anion