00:01
The titration reaction that we're considering is ammonia, nh3, reacting with hcl, which i'll represent as hydronium ion, producing its conjugate base, ammonium, and water.
00:18
We're starting with 100 milliliters of ammonia at a concentration of 0 .0500 moles per liter.
00:34
If we convert this to liters and multiply by the molarity, we'll get the moles.
00:45
So 0 .00, sorry, 0 .100 liters, that gives us 0 .005 moles of ammonia.
00:56
That's all we've got.
00:58
And we're adding 50 milliliters.
01:06
Looks like that's the only one i see.
01:07
It said after these given volumes, but all i see is 50.
01:12
50 milliliters is 0 .0500 liters, and its concentration is 0 .100 moles per liter.
01:21
So that also gives us 0 .005 moles of the acid.
01:31
So with the stoichiometry being one to one, and the moles of each of them that we're adding as 0 .05, then we're going to end up making 0 .005 moles of ammonium and an additional 0 .005 moles of water...