UNIT SIX Flashcards
solubility rules
- NO3(-) and CH3COO(-) are soluble
- group 1 ions and NH4+ are soluble
- group 17 ions are soluble EXCEPT WITH Ag(+), Cu(+), Hg2(2+), Pb(2+)
- SO4(2-) ions are soluble EXCEPT WITH Ba(2+), Ca(2+), Hg2(2+), Pb(2+), Sr(2+)
- Ba(OH)2, CA(OH)2, Sr(OH)2 are soluble
- all other compounds are insoluble
net ionic equation
- Write balanced equation
- Determine solubility
- Break apart aqueous compounds
- Cancel like terms
- Rewrite equation
dissolution
when compounds made of ions are dissolved in water, ions separate from one another
ionization
ions formed from solute molecules by action of solvent
overall ionic equation
shows both molecular and ionic compounds present in aqueous solution reaction
spectator ions
do not take part in reaction change, found before and after reaction
net ionic equation
describes actual reaction, only includes compounds and ions that undergo chemical change in aqueous solution
freezing point depression/molal freezing point constant
freezing point of solvent in 1-molal solution of nonvolatile, nonelectrolyte solute
boiling point elevation
boiling point of solvent in 1-molal solution of nonvolatile, nonelectrolyte solute
properties of acids
- sour taste
- can react with metals to release hydrogen
- produce salt and water with braces
- conduct electric current
monoprotic acids
only donate 1 proton per molecule
polyprotic
can donate more than 1 proton per molecule
(diprotic: donates 2, triprotic: donates 3)
properties of bases
- taste bitter
- can feel slippery
Arrhenius acid
chemical compound that increases concentration of hydrogen ions in aqueous solution
Arrhenius base
increases concentration of hydroxide ions
Bronsted-Lowry acid
molecule/ion that is proton donor
Bronsted-Lowry base
molecule/ion that is proton acceptor
conjugate acid of the base
formed when B-L base gains a proton
conjugate base of the acid
species formed when B-L loses proton
Lewis acid
atom/ion/molecule that accepts electron pair to form covalent bond
Lewis base
atom/ion/molecule that donates electron pair to form covalent bond
amphoteric compounds
any species that can react as either acid or base
pH meter
determines pH of a solution by measuring voltages between 2 electrodes that are placed in solution
acid-based indicators
compounds whose colours are sensitive to pH
transition interval
pH range over which an indicator changes colour
titration
controlled addition and measurement of amount of solution of known concentration required to react completely with measured amount of a solution of unknown concentration
equivalence point
point at which 2 solutions in titration are present in chemical equivalent amount
end point of the indicator
at which the indicator changes colour
