0 recently 
0/10| 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 |
pH = pKa + log [A-]/[HA] ---> acids
pOH = pKb + log [BH+]/[B] ---> bases
the conjugate salt is on top, and the bottom is either the base or the acid
assume there is a limiting and excess reagent (because it will contain either a strong acid or base) |
| in what range are buffers effective |
within 1 pH of its pKa, up or down |
| pH + pOH = |
14 always!! |
| H2O pH is always... |
7, could be acid (pH) or base (pOH) |
| Kw = |
1.0 x 10^-14 at 25 C or 298 K |
| 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 |
| 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 |
| maximum buffering capacity |
pH = pKa |
| how to increase/decrease buffering capacity |
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) |
| 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 |
| strong acid strong base equivalence point |
pH = 7 @ 25 C / 298 K |
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Elias A 
Physical chemistry
Milena Z 
Matteo Z 
