Textbook Ch.4: Reactions in Aqueous Solution

the concentration of a solute in solution molarity (M) = moles of solute / liters of solution

the molarity of a species in solution

• The number of moles of solute in a given volume of solution • The volume of solution containing a given number of moles of solute

formed when two different ionic compounds are mixed, an insoluble solid separates out of a solution • The precipitate that forms is itself ionic • The cation comes from one solution, the anion comes from the other

the chemical equation that shows only those elements, compounds, and ions that are directly involved in the chemical reaction.

• Atom balance (same number of atoms of each element on both sides) • Charge balance (must be the same total charge on both sides)

a species that produces H⁺ ions in water solution

a species that produces OH⁻ ions in a water solution

acids that ionize completely, forming H⁺ ions and anions

acids that only partially ionize to H⁺ ions in water

the reaction does not go into completion, instead a mixture is formed containing significant amounts of both products and reactants

bases that completely ionize into OH⁻ ions and cations

produce OH⁻ ions by reacting with water molecules, acquiring H⁺ ions and leaving OH⁻ ions behind

acids and bases both completely and the H⁺ and OH⁻ ions react with each other to form H₂O molecules, this reaction is referred to as neutralization

H⁺(aq) + OH⁻(aq) —> H₂O

a two-step reaction occurs • Ionization of the weak acid into H+ and an anion • Neutralization of the H+ ions produced from (1) react with the OH- of the base to produce water

HB(aq) + OH⁻(aq) —> H₂O + B⁻(aq)

two-step reaction occurs • Acid reacts with water to form cations and OH⁻ • Neutralization occurs when ions produced from (1) react with the OH⁻ of the base to produce water

H⁺(aq) + B(aq) —> BH⁺(aq)

when acid-base reactions in water solution are commonly used to determine the concentration of a dissolved species or its percentage in a solid measure, so the volume of a standard solution (a solution of known concentration) required to react with a measured amount of sample is measured

a reaction in an aqueous solution that involves a transfer of electrons between two species

the species that loses (i.e. donates) electrons

the species that gains (i.e. received) electrons

it can be split into two half-equations, one of oxidation and the other of reduction