| By Leejwwc (Leejwwc) on Wednesday, March 31, 2004 - 08:31 pm: Edit |
An aqueous solution of calcium hydroxide is titrated with a strong acid.
If water is added to the erlynmeyer flask in the course of the above titration, would the calculated value of Ksp be too high, too low, or correct, and why?
| By Joel_Set (Joel_Set) on Thursday, April 01, 2004 - 02:29 am: Edit |
somebody answer this?
| By Eastsoldier (Eastsoldier) on Friday, April 02, 2004 - 08:56 am: Edit |
Ca(OH)2 is titrated ->
Ca2+ and anion of the acid remains (aqueous)
->
add water
->
nothing happens
(water doesn't react. If it did, it would have happened before you put the water)
unless... it is not completely titrated
Note : Ksp : solubility constant
At equilibrium Ksp=Q
--------------------------------------------------------------------
I'm not 100% sure with this, though.
Concentration will get lowered as you add water
(Was there some indication of what that acid was? ie. monoprotic or polyprotic?)
Report an offensive message on this page
E-mail this page to a friend
| Posting is currently disabled in this topic. Contact your discussion moderator for more information. |
| Administrator's Control Panel -- Board Moderators Only Administer Page |