00:01
First, we need to know what is the balanced chemical reaction.
00:03
We have a hydrozoic acid, which i'll represent as ha, reacting with potassium hydroxide, or most specifically, the hydroxide of the potassium hydroxide, producing the conjugate base to hydrozoic acid, which i'll represent as a - and water.
00:25
So it looks like we have enough information to know the moles of the hydrozoic acid we're starting with.
00:34
That'll be equal to the 62 .7 milliliters expressed as liters, that being 0 .0627 liters, which we multiply by its concentration to get the original moles 0 .5400 moles per liter and we get at 0 .03386 moles.
01:10
We'll then calculate the moles of sodium hydroxide that we added.
01:14
We added 4 .27, no, we added 18 .1 milliliters of the potassium hydroxide, which represents 0 .0181 liters liters at a concentration of 0 .5100 moles per liter, and we would have added 0 .009231 moles of hydroxide.
01:48
So hopefully it's obvious that we're going to have some excess ha left over because we haven't added enough hydroxide to completely neutralize all of it...