Ch 4 Solubility, Precipitation, Titration Flashcards
aqueous solution
liquid solution made with a solute and solvent
aqueous solutions and electrolytes
some aqueous solutions form ions within a solution that are called electrolytes; others are called nonelectrolytes
electrolytes
can be observed with lightbulbs; ions in the solution are conductors’ electrolytes are either strong, weak, or non
ionic compounds in water
when an ionic compound dissolves it’s component ions disassociate; because Oxygen in water is slightly negative and Hydrogens are slightly positive, they separately attract the solute’s ions and disassociate them
ions in a solution are…
stable, ions not in a solution aren’t really stable
molecular compounds in water
molecules remain intact and disperse as nonelectrolytes; acids are the exceptions here
writing aqueous solution equations
if weak electrolytes, the arrows flowing both ways indicate only small amounts of ions disassociated; if a strong electrolyte or nonelectrolyte, a one way arrow is used
strong electrolyte reactants
ionic compounds and acids
precipitation reaction
when two pairs of ionic compounds switch ions to form new ions; one of the new products is a compound
soluble ionic compounds
all nitrates and acetates.
Chloride, Bromide, and Iodide are soluble except with Silver, Mercuriy and Lead.
Sulfates except with Strontium, Barium, Mercury, and Lead
insoluble ionic compounds
Sulfide and Hydroxide except with ammonium, calcium, strontium, barium, and all alkalis.
Carbonate and Phosphate except with ammonium and all alkalis.
how do you identify the precipitate?
the precipitate is identified using solubility rules, if one of the new ionic compounds are insoluble, that’s your precipitate
ionic equations
complete ionic is when you pull all compounds apart and list all elements as ions; the net ionic equation identifies which ions created a new compound end excludes spectator ions
acids and bases when dissolved
acids are dissolved into H ions and disassociate; bases accept H ions and disassociate into OH ions.
strength of electrolytes
all ionic are strong, strong acids are strong; weak acids and bases are weak; no ionic compounds are weak; all other molecular compounds are nonelectrolytes and no ionic compounds are nonelectrolytes
neutralization reactions
when an acid and base react they neutralize each other and the products don’t share any properties; one product is a salt
salt formation
occurs in neutralization when the cation is from a base and the anion is from an acid; metal hydroxide and an acid always makes a salt
gas formation from acids and bases
non hydroxide bases sometimes produce gases when reacted with an acid; carbonates and bicarbonates create carbonic acid (which is unstable) that then decomposes to water and CO2
molarity
mol/Liter
Dilution
the moles of solute never change, but the total volume increases by adding solvent.
Strong Acids
HI HBr HClO4 HCl HClO3 H2SO4 HNO3
Strong Bases
NaOH KOH LiOH RbOH CsOH Ca(OH)2 Ba(OH)2 Sr(OH)2
