Honors Chemistry Unit 10: Acids & Bases

solution

usually aqueous, two parts are solute and solvent

molarity and dilutions

changing the amount of solvent changes concentration (molarity) of a solution

dilution equation

M1*V1=M2*V2

hydrogen ion

often referred to as a proton

properties of acids

sour and conductive, turns litmus paper blue

properties of bases

bitter and slippery, turns litmus paper red

Arrhenius model

states that acids are characterized by an hydrogen ion and bases with hydroxide

bronsted-lowry model

characterizes and acid as a hydrogen ion donor and bases as a hydrogen ion acceptor

conjugate acid

species produced when a base accepts an H+ ion

conjugate base

species produced when an acid donates an H+ ion

conjugate acid-base pair

two substances related to eachother by the donating and accepting of a single H+

naming of acids when no oxygen is present

hydro + root of element +ic + acid

naming of acids with oxygen present

root of anion + (ate-ic)/ (ite-ous) + acid

naming of bases

name of element +hydroxide

dissociation

separation of a compound into its ions when dissolved in water

neutralization

a type of double replacement where one product is always H2O+salt

strong acids and bases

a strong acid or base can dissociate completely (one sided arrow), must COMPLETELY DISSOCIATE to be considered a strong acid or base

strong acid examples

HCl, HBr, HI, HNO3, HClO4, H2SO4

strong bases examples

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Ba(OH)2, Sr(OH)2

monoprotic

one hydrogen present in an acid

diprotic

two hydrogens present in an acid

triprotic

three hydrogens present in an acid

pH

expresses acidity, concentrations of hydrogen ions are often very small numbers

pOH

expresses alkalinity, concentraions of hydroxide ions are often very small numbers

equivalence point

the point where the moles of H+ from the acid = moles of OH- from the base

indicator

chemical dye that detects the equivalence point during a titration

end point

the point at which an indicator changes during the titration, endpoint must be in same range as equivalence point

Kw

ion product constant for water, Kw = [H+][OH-] + 1.0 × 10^-14

titrations

a process in which an acid-base neutralization reaction is used to determine the concentration of a solution with an unknown concentration, the concentration of the other substance must be known

water molarity equation

[H+] = [OH-] = 1.0×10^-7