H2O pH is always...
7, could be acid (pH) or base (pOH)
how to increase/decrease buffering capacity
strong acid strong base equivalence point
pH = 7 @ 25 C / 298 K
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
in what range are buffers effective
within 1 pH of its pKa, up or down
pH + pOH =
14 always!!
how do you calculate a buffer's pH
strong acid-weak base reaction
maximum buffering capacity
pH = pKa
weak acid-strong base reaction
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
straight line up part of graph
#miles of titrant = #moles of analyte
concentration and volume of titrant is then used to determine concentration of analyte
1.0 x 10^-14 at 25 C or 298 K
