chemistry final exam review

molarity

a way of quantifying the concentration of a solution

concentration

the amount of solute dissolved in a given amount of solvent

how to calculate molarity

M = moles of solute/volume (L) of solution

dilution

reducing the concentration of a chemical solution

dilutions formula

initial molarity, initial volume = final molarity, final volume

acids

any compound that is able to ionize and form a hydrogen compound

characteristics of acids

• increase the concentration of H

• sour taste

monoprotic acids

acids that yield one H+ per molecule of acid

diprotic acid

acids that yield two H+ per molecule of acid

bases

any substance that is able to accept (react with) H+

characteristics of bases

• bitter taste

• slippery

• produce OH ions when dissolved in water

• increase the molarity of OH

salt

any ionic assembly of cations and anions that result in an electrically neutral compound (ionic compounds)

neutralization

a reaction where an acid and base are mixed to make salt and water

electrolyte

solutes that exist in ions in a solute

non electrolyte

solutes do not separate into ions

characteristics of non electrolytes

• do not conduct electricity

• ex - sugar and water

strong electrolytes

any substance that exists nearly all as ions in a solution

characteristics of strong electrolytes

• most ionic compounds

• good conductors

• ex - NaCl

weak electrolyte

compounds that only partly ionize in solution

characteristics of weak electrolytes

• soluble

• poor conductors

• ex - acetic acid

strong acid/base

completely ionize in water

• good conducter

• ex - HCl (Acid), NaOH (base)

weak acid/base

only partially ionize in water

• poor conductor

• ex - HF (acid), NH3 (base)

rules for identifying strong/weak electrolytes

• most salts are strong electrolytes

• most acids are weak electrolytes (except for these strong acids: HCl, H2SO4, HNO3, HBr, Hi, HClO4)

• hydroxide (OH-) and either group 1(alkali) or group 2 (alkaline earth) metals are

  STRONG (except for NH3)

• most other substances are non electrolytes

titration

method of determining the concentration of an unknown solution

end point

when you are close to the equivalence point

equivalence point

the point at which stoichiometrically equal amounts get together

solubility

maximum amount of solute that will dissolve in a certain amount of solvent

saturated solution

a solution that is full with solute

unsaturated solution

a solution that can accept more solute

supersaturated solution

a solution that has more solute dissolved that it normally should

solubility curves

a graph showing the solubility of a solute as temperature changes

• for solids - as temperature increases, solubility increases

• for gases - as temperature increases, solubility decreases

thermodynamics

the study of energy (or heat) and its transformations (changes)

thermochemistry

thermodynamics as related to chemical reactions

dissolving

separate in the water

dissociating

the ions seperate

force

a push/pull on an object

work

force times distance

heat

the energy that is transferred from one object to another

energy

the capacity to do work or transfer heat

kinetic energy

the energy of motion

kinetic energy formula

KE - (1/2)mv²

potential energy

stored energy based on position

formula for potential energy

PE = mgh

joule

SI unit for energy

calorie

used to measure energy in a chemical reaction

system

part that is singled out for the study (normally the chemical reaction)

surroundings

everything else

the first law of thermodynamics

either is neither created or destroyed

internal energy

the total energy of a system

delta e

change in internal energy of a system

• formula: E final -E initial

when delta e has a positive value, the system has ____ energy from the surroundings

gained

when delta e has a negative value, the system has ____ energy to the surroundings

lost

Delta E = q+w

q - the heat added to or given off from the system

w - work done on or by the system

endothermic

energy is being added to a system (+)

exothermic

energy is being released (-)