unit 8 must knows duel

weak acid-strong base reaction

Kw = 1.0 x 10^-14 at 25 C or 298 K

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

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

pH = pKa

how do you calculate a buffer's pH

strong acid strong base equivalence point

pH + pOH =

how to increase/decrease buffering capacity

H2O pH is always...

in what range are buffers effective within 1 pH of its pKa, up or down

what is a buffer

H2O pH is always... 7, could be acid (pH) or base (pOH)

maximum buffering capacity pH = pKa

Kw = 1.0 x 10^-14 at 25 C or 298 K

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)

how to increase/decrease buffering capacity

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

equivalence point

in what range are buffers effective

pH = 7 @ 25 C / 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

14 always!!

End this game?