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Topic: mass of NaOH  (Read 6971 times)

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Offline pandabear

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mass of NaOH
« on: March 07, 2009, 09:09:23 AM »
What amount of solid NaOH must be added to 1.0 L of a .14 M H2CO3 solution to produce a solution with H+ = 3.2 x 10-11?

*No significant volume change as result of the addition of the solid.

Does it matter that it is a diprotic acid? Should we set up an ICE table? I'm not sure where to start...
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Offline Vidya

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Re: mass of NaOH
« Reply #1 on: March 07, 2009, 09:22:46 AM »
I think you need to make ice table to know how much H+ ions are present there and how much out of it you want to neutralize .Calculate no of moles of NaOH required to neutralize it.
Yes take care it is diprotic.
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Offline Borek

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Re: mass of NaOH
« Reply #2 on: March 07, 2009, 11:52:36 AM »
No need for ICE table, this is a buffer question. Use Henderson-Hasselbalch equation.
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Offline Vidya

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Re: mass of NaOH
« Reply #3 on: March 08, 2009, 09:13:11 AM »
In Buffer solution you are using a salt and its weak acid.Than ofcourse you can use Henderson-Hasselbalch equation.But I dont think concentration of salt is given to you.A strong base and weak acid is given.
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Offline Borek

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Re: mass of NaOH
« Reply #4 on: March 08, 2009, 09:26:33 AM »
Think what reactions take place when you add NaOH. Think what you will have in the solution once pH goes up to 10.5.
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