Chapter 4: Reactions in Aqueous Solutions

solution

homogenous mixture of two or more substances

solute

substance present in a smaller amount

solvent

substance present in a larger amount

Aqueous solution

a solution in which the solute in initially a liquid or solid and the solvent is water

electrolyte

a substance that when dissolved in water conducts electricity 

non electrolyte 

a substance that when dissolved in water does not conduct electricity 

dissociation

process by which ions separate in an ionic compound 

hydration

the process in which an ion is surrounded by water molecule arranged in a specific manner 

precipitation reaction

a reaction that results in the formation of an insoluble product (a precipitate)

solubility 

the maximum amount that will dissolve in a given quantity of solvent at a specific temperature 

molecular equation 

formulas of the compounds are written as though all species existed as molecules or whole units 

ionic equation

shows dissolved species as free ions

net ionic equation

shows only the species that actually take part in the reaction

spectator ions 

ions that are unchanged during a chemical reaction, aqueous on both sides 

Arrhenius definition of acid 

contain H+ and release (ionize) it in solution 

Arrhenius definition of base 

contain OH- and release (ionized) it in solution

Bronsted acid

a proton donor

Bronsted base

a proton acceptor

hydronium ion

a hydrated proton

monoprotic acid

can donate one hydrogen ion

diprotic acid

can donate 2 hydrogen ions

triprotic acid

can donate 3 hydrogen ions

neutralization reaction

a reaction between an acid and a basem usually producing water and a salt 

salt 

an ionic compound made up of a cation other than H+ an anion other than OH^- and O^2-

Combination/synthesis reaction

a reaction in which two or more substances combine to form a single product

A + B → AB

Decomposition reaction

the breakdown of a compound into two or more components

AB_² → A + 2B

Combustion reaction

a reaction in which a substance reacts with oxygen, usually with the release of heat and light to produce a flame (balance oxygens last)

double replacement reaction

the cations of two different compounds switch places

AB + CD → CB + AD

Single replacement reaction

an ion (or atom) in a compound is replaced an ion (or atom) of another element

A + BC → B+ AC

hydrogen displacement (type of single replacement reaction) 

very reactive metals generate H₂  gas when mixed with water; many metals will generate H₂  gas when mixed with acids 

metal displacement

a metal in a compound can be displaced by another metal in the elemental state

activity series

a list of metals with the most reactive metals at the top and the least at the bottom; used to predict if metal displacement reactions will or will not occur 

disproportionation reaction

an element in one oxidation state is simultaneously oxidized and reduced 

molarity

number of moles of solute per liter of solution

halogen displacement

similar to metal displacement but with the halogen