Acid-Base equalibria

what is a bronsed lowery acid

proton doners, (donate protones to a base)

What are bronsted lower bases

proton acceptors ( accept proton from acids)

what is special about water

it can accept of donate a proton (h+) and is therefor referred to as amphiprotic

for neutral solutions, what is the OH/H3O concentration equal to

1 x 10 ^-7

how do you calculate pH

pH= -log[H3O]

how do you calculate pOH

pOH=-log[OH]

what is kw equal to for solutions at 25 degrees

1 x 10 ^ -14

what is the definition of strong acids

strong acids ionize completely in water

what are examples of strong acids

HClO4, H2SO4, HNO3, HBr, HI

what is the definition of a strong base

disassociation reaction happens completely in water

what are examples of strong bases

LiOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

what is the definition of a weak acid

partially ionize in aqueous solution and establish an equilibrium (forms an equilibrium)

what is the definition of a weak base

a weak base is one that does not completely disassociate in water ( forms an equilibrium)

how do you calculate % ionization for acids

[H3O]/[HA] x 100

how do you calculate % ionization for bases

[OH]/[BOH] x 100

what is % ionization for strong acids or bases

100%

what is the conjugate base of a weak acid

a weak base

what is a buffer

a buffer is a solution which presents small pH changes when concentrated strong acids or bases are added to it, hs similar concentrations or a weak acid and salt of its conjugate base or similar concentration of a weak base and a slat of its conjugate acid

what happens as the concentration of CO2 in the atmosphere increases

the concentration of aqueous CO2 in natural waters increases (pH decreases)