Chemistry

Acid

Substance that donates H⁺ (proton donor)

Base

Substance that accepts H⁺ (proton acceptor)

Bronsted-Lowry acid/base

Acid donates H⁺, base accepts H⁺

Amphoteric

Substance that can act as acid or base (e.g., water)

Monoprotic acid

Acid donating 1 H⁺ (e.g., HCl, HF)

Diprotic acid

Acid donating 2 H⁺ (e.g., H₂SO₄)

Triprotic acid

Acid donating 3 H⁺ (e.g., H₃PO₄)

Calorie

Energy unit

Catalyst

Speeds up reaction without being consumed

Collision theory

Reactions occur when particles collide with enough energy and correct orientation

Activation energy

Minimum energy for reaction to occur

Endothermic

Reaction absorbs heat (+∆H)

Exothermic

Reaction releases heat (–∆H)

Equilibrium

Forward and reverse reaction rates equal; concentrations stay constant

Equilibrium constant (Keq)

Ratio of product concentrations to reactants at equilibrium

LeChatelier’s Principle

System shifts to counteract stress (change in conc, temp, pressure)

Molarity (M)

Moles of solute per liter of solution

Neutralization

Acid + base reaction producing water and salt

pH

Measure of acidity, pH = –log[H⁺]

pOH

Measure of basicity, pOH = –log[OH⁻]

Rate law

Rate = k[A]^a[B]^b (reaction order = a + b)

Reaction quotient (Q)

Same formula as Keq but at any point, not just equilibrium

Specific heat (c)

Heat required to raise 1 g of substance by 1°C

Surroundings/system

In thermochemistry, system is the reaction, surroundings are everything else