unit 8 must knows duel

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

H2O pH is always...

how do you calculate a buffer's pH

pH = pKa

strong acid strong base equivalence point

14 always!!

strong acid-weak base reaction

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 to increase/decrease buffering capacity

within 1 pH of its pKa, up or down

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

strong acid-weak base reaction

14 always!!

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

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)

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

in what range are buffers effective

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

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

pH = 7 @ 25 C / 298 K

pH = pKa

End this game?