in what range are buffers effective
14 always!!
HA(aq) + OH- --> A-(aq) + H2O(L)
if weak acid is in excess --> a buffer --> Hendeson Hasselbalch equaiton
if strong base is in excess, the moles of excess hydroxide ions is used for pH
if acid and base are equimolar then the equilibrium concentr
equivalence point
strong acid-weak base reaction
if weak base is in excess --> a buffer --> Hendeson Hasselbalch equaiton
if strong acid is in excess, the moles of excess acid are used to determine pH
if acid and base are equimolar then the equilibrium concentrations are used to determine pH
Kw =
1.0 x 10^-14 at 25 C or 298 K
increasing/decreasing concentrations of buffer components, but keeping the ratios constant (if you don't it'll change the buffer capacity for either acid or base respectively)
what is a buffer
solution that is resistant to a small pH change, it has to contain a weak acid or base pared with its conjugate salt(Na+, H3O-, etc...) and it creates neutral compounds, keeping pH relatively stable
how do you calculate a buffer's pH
strong acid strong base equivalence point
pH = 7 @ 25 C / 298 K
H2O pH is always...
7, could be acid (pH) or base (pOH)
maximum buffering capacity
pH = pKa
