no, for the longest time I've been having a hard time understanding acids and bases in general :C as if there is a really basic concept I dont know off or understand but great vid
Nice! Just a quick question, does the calculation of the half equivalence point apply here as well or is it because we're dealing with a SA and SB that it wouldn't matter
Thank you! really nice video. Quick question: do you ever factor the water generated in the acid-base neutralization as part of the final volume to determine molarity of the acid (in this case) or is it too small and is never taken into account?
I’ve never factored it in…I assume it’s negligible. Also, it could reduce the volume potentially, since a hydrogen ion and a hydroxide ion combine to make each water molecule…It depends on whether two ions or one water molecule takes up more space in solution. Either way, it would be a very small change, if any change at all.
After the equivalence point you switch to calculating the hydroxide concentration. It would seem that there should be a single equation that would provide all of the pH values . The problem is that when you get to past equivalence the 'apparent' hydrogen ion concentration is negative, which of course is wrong. So my question is : Is there a single equation which would provide the pH, or the hydrogen ion concentration through the entire range?
This is because hydroxide and hydronium actually cannot be in the solution at the same time. This is because when they are together, they just make water. I used to think that pH was a measure of a ratio between hydroxide:hydronium but my chem prof said it isn’t. At 4:38, the added hydroxide ions are completely used up because they reacted with the hydronium ions to form water. This is why later on we switch to finding pH from the hydroxide (OH-) instead of the hydronium (H+); because now there are so much more OH- that the H+ is being completely used up
Hi! Any way you could clarify why you use the BAA table rather than the ICE table in these titration questions? Can't seem to wrap my head around that even though I'm sure the answer is simple. Thanks so much!
The BAA table is a stoichiometry calculation to determine how much acid or base is left over after they neutralize each other. Whenever you add an acid and a base, you can use the BAA table first. The ICE table is for when there is an equilibrium happening. If there is leftover H+ or OH-, you don’t need one. But if there is weak acid or base present, the ICE table (or HH equation, which is an ICE table shortcut) helps you determine the concentrations.
@@SiebertScience Thanks for answering! So to make sure I’ve got it, the BAA table is used for this reaction because it’s not in equilibrium? (I’m trying to teach myself chemistry, this resource is great, just stuck on this part!)
@@looprecorder Even if there is an equilibrium, you'd still need a BAA table any time you're mixing an acid and a base together. If you watch my Weak Acid / Strong Base Titration video, you'll see that we still do a BAA table for most points in the titration, followed by an ICE table (or Henderson-Hasselbalch, which is an ICE table shortcut).
