At 5:53, would you not just substitute your value for [H+] into the equation Kw = [H+]^2 to find Kw, so Kw would equal [H+]^2 and not the root of [H+]?
@@hongjoongswife9672 at equivalence point, the number of moles of H+ and the number of moles of OH- are equal. Since we're using NaOH and a monoprotic acid (can donate one H+), the number of moles for both acid and base are equal. Had it been a diprotic acid, the number of moles of acid required would have been half of the number of moles of NaOH.
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At 5:53, would you not just substitute your value for [H+] into the equation Kw = [H+]^2 to find Kw, so Kw would equal [H+]^2 and not the root of [H+]?
You're right and that is in fact the calculation I've done (even if that isn't what I've written). I'm sorry about that.
For question 9.2, how do you know its a half titration?
I really hoped my talk-through explained this. Try watching that part again and let me know if you're not sure of anything specific I say.
@@simonflynn4515 Still not sure. Could you explain it step by step in more detail,please?
10:10 so the number of moles for both acid and base are equal?
Moles of H+ and OH-. They’ve told us we have NaOH and a monoprotic acid.
@@simonflynn4515 so are they equal...I’m still confused?
@@hongjoongswife9672 at equivalence point, the number of moles of H+ and the number of moles of OH- are equal. Since we're using NaOH and a monoprotic acid (can donate one H+), the number of moles for both acid and base are equal. Had it been a diprotic acid, the number of moles of acid required would have been half of the number of moles of NaOH.