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# chemistry - simple concentration stuff... watch

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1. ok, so this is really quite simple and i should know this but, for some reason, i'm sitting here trying to write out my final plan for this experiment.. and i'm stuck on this one annoying bit.

i'm doing a titration experiment in which the total volume of solution timed is 45cm^3. i'm varying the concentration of the potassium bromide of the solution... but it's volume (10/45) will remain the same in all the experiments to keep it a fair test.

i have 0.01M of this stuff too.

right, i know to work out the concentration of the potassium bromide in the solution i do 0.01 x (10/45) = 0.0022mol dm^-3 and so on (replacing "0.01" with "0.008" and "0.007", etc).

my question is... this 0.01/0.008/0.007/0.006... what on earth is it? the solution in moles? how do i get 0.01M of a solution and then 0.008M of that same solution?

see, i feel stupid asking it. i feel like i've gone stupid overnight lol.

pls help someone. i don't get it.
2. moles = molarity x volume
3. lol, thanks for that equation.

but i'm still stuck.

i mean, i just want to know how i'm going to get 0.01M, 0.008M, 0.007M of this potassium bromide... are they in separate bottles? can i make them myself through diltuting with water?

*stoooopid*
4. (Original post by ph9)
lol, thanks for that equation.

but i'm still stuck.

i mean, i just want to know how i'm going to get 0.01M, 0.008M, 0.007M of this potassium bromide... are they in separate bottles? can i make them myself through diltuting with water?

*stoooopid*
Probably you can make them by dilution using a volumetric flask. You should have been taught how to do this, if not do ask.
5. taught? you mean that thing teachers are supposed to do? try telling my chemistry teacher that.

worst "teacher" EVER.

but thanks, it's worth harassing her just for the crack, if not for gaining anything educational from it.

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Updated: October 11, 2006
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