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IN THE HENDERSON HASSELBALCH, THE
when the processes of dissolution and precipitation reach equilibrium when there is a SMALL concentration of ions
when the processes of dissolution and precipitation reach equilibrium when there is a substantial concentration of ions
is one where a solution is in equilibrium with the solid form of its solute
a small Ksp means:
that very little salt will dissolve; aka that the equilibrium concentrations of hte ions are very small
we can use Q compared to Ksp to:
- show whether a precipitate will form or not:
- if Q < Ksp, the the solution is unsaturated (b/c more ions could enter solution); no precipitate will form
- if Q > Ksp, the solution is super saturated and a precipitation will take place
- if Q = K, then the solution is saturated and ....
strong acid-strong base titration
- reaction products do NOT influce pH! aka the conjugates of the acid and base
- -pH of 7 when equal amounts have reacted
don't forget to do this weird 'starting over thing'
if you are starting with an acid dissociating but are then given a certain concentration of it's conjugate base, you can then use the acids Ka to find Kb at room temperature, then find the pH of the base if you dissolve it in water, set up eq. ratio, calculate concentration of OH- etc. etc.
weak acid-strong base
-after the equivalence point, the weak acid makes NO difference (don't even have to account for it as the limiting reagent); the solution is super basic so all you have to do is find the concentration of basic titrant = [OH-] to find the pH
strong acid - weak base titration
- -prior to eq. point the solution is a weak base with some weak conjugate acid present so that an equilibium calculation is required
- -at the equivalence pointall original weak base and strong acid titrant have reacted but conj. weak acid is present (so you need eq. calculation)
- -after equivalence point all that needs to be taken into account is excess strong acid
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