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October 25, 2014

Homework Help: college chemistry

Posted by Aubree on Wednesday, April 21, 2010 at 5:59pm.

In class, we discussed the titration of a 50.0 mL sample of 0.100 M HCL with a 0.100 M solution of NaOH.
How would this system change if we used a 0.100 M solution of Sr(OH)2 instead of NaOH? To answer this question, complete each of the following:
a) What volume of 0.100 M Sr(OH)2 solution would be needed to reach the equivalence point of this titration? In a short (2-3 sentence) paragraph, compare this volume to the volume of NaOH required, as discovered in class. Does your answer make sense? Why or why not?
b) What will be the pH of the combined HCl- Sr(OH)2 at this point (the equivalence point)? Once again, use a short (2-3 sentence) paragraph to compare your answer to that obtained in class for the titration of HCl with NaOH. Is this pH at the equivalence point the same in both titrations? If so why? If not, why not? In either case, do(es) the answer(s) obtained make sense?

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