how do you calculate a buffer's pHpH = 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)
Frozen!
Frozen!
Boost!
Boost!
strong acid strong base equivalence pointpH = 7 @ 25 C / 298 K
maximum buffering capacitypH = pKa
strong acid-weak base reaction
weak acid-strong base reaction
pH + pOH =
equivalence point
H2O pH is always...
in what range are buffers effectivewithin 1 pH of its pKa, up or down
Kw =1.0 x 10^-14 at 25 C or 298 K
what is a buffer
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)
Kw =1.0 x 10^-14 at 25 C or 298 K
Frozen!
Frozen!
maximum buffering capacity
how to increase/decrease buffering capacityincreasing/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 buffersolution 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 pHpH = 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)
strong acid-weak base reaction
14 always!!
strong acid strong base equivalence pointpH = 7 @ 25 C / 298 K
weak acid-strong base reactionHA(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
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
in what range are buffers effectivewithin 1 pH of its pKa, up or down
Boost!
Boost!
H2O pH is always...7, could be acid (pH) or base (pOH)