homogenous mixture of 2+ substances universally dispersed thoughout a single phase

capable of dissolving in a particular solvent

increasing surface area of solute speeds up dissolution.

the ability of one substance to dissolve in a another at a given temperature and pressure; expressed in terms of the amount of solute that will dissolve in a a given amount of solvent to produce a saturate solution

solute is dissolved by the solvent

concentration of molecules in a substance (moles/Liter)

Adding water to a solution in order to decrease the concentration

states that chemical reactions can occur when atoms, ions, and molecules collide

A substance that changes the rate of a chemical reaction without being changed or consumed significantly

what you get/ accepted x 100

the reactant that is completely consumed when a reaction is run to completion

tiny particles that are far apart, elastic collision= no net loss of kinetic energy, continuous, rapid motion, no forces of attraction, temperature depends on average kinetic energy

spontaneous mixing of the particles of two substances caused by their random motion

hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory

definite volume and takes shape of container, particles in constant motion, greater attractive forces, particles not fixed-fluid, relatively high density, relative incompressibility, ability to diffuse

process by which a liquid or solid changes to a gas

process by which particles escape from the surface area of a non boiling liquid and enter the gas state.

closely packed, strong attractive forces, only vibrational movement, ordered particles, definite shape and volume, definite melting point, high density and incompressibility, low rate of diffusion

physical change of a solid to a liquid by the addition of energy as heat

measure of the average kinetic energy of the particles in a sample of matter

energy transferred between samples of matter bc of a difference in their temperatures

the force per unit area on a surface; pressure = force/area

Standard Temperature and Pressure- 273 degrees Kelvin/0 degrees celsius and 1 atm

Law of partial pressures

See image

1. aqueous solutions have a sour taste

1. aq solutions taste bitter

P1V1=P2V2

one decreases as other increases

P1V1/T1=P2V2/T2

equal volumes of equal gases at the same temperature and pressure contain equal numbers of molecules

the volume occupied by one mole of a gas at STP is 22.414 Liters; this value can be used to find the mass of a gas at STP

The study of the relationships between amounts of products and reactants

PV = nRT; P = pressure(atm); V = volume(L); n = number of moles; R = .0821 L x atm/Kmol; T = temperature

the negative of the common logarithm of the hydronium ion concentration

the react of the ions that characterize acids (hydronium ions) and the ions that characterize bases (hydroxide ions) to form water molecules and salt

An ionic compound made from the neutralization of an acid with a base.

a value that is used to express the acidity or alkalinity of a system; each whole number on the scale indicates a tenfold change in acidity; pH of 7 in neutral, a pH less than 7 is acidic, a pH more than 7 is basic

compounds whose colors are sensitive to pH

a method to determine the concentration of a substance in solution by adding a solution of known volume and concentration until the reaction is completed, which is usually indicated by a change in color

-log[OH-]

the reactant that is not completely used up in a reaction

V1/T1=V2/T2

P1/T1=P2/T2

AB + CD --> AD + CB

A + BC --> B + AC

occurs when a substance reacts with oxygen to produce energy in the form of heat and light

a reaction in which a single compound breaks down to form two or more simpler substances

a reaction in which two or more substances combine to form a new compound