Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: washey on May 29, 2008, 02:07:05 AM
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We are using Iodine to determine the concentration of Ascorbic acid in orange juice. I have determined the molarity of the Iodine solution to be .00172M I2 in procedure 1.
In procedure 2 I determined that 10.10mL of Iodine was needed for titration of the fresh orange juice solution.
In this solution 10.00mL of orange juice was used with 10.00mL of H2O. We use the formula M1 x V1 = M2 x V2. So,
M1 = .00172M I2
V1 = 10.10mL I2
M2 O.J. = ? ( what we are looking for)
V2 O.J.= 10.00mL ( or would I use 20mL since the solution had 10.00mL H2O added)
Will the formula be M2 = (0.00172M x .01001mL)/.01mL
or M2 = (0.00172M x .01001mL)/.02mL ?
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It is all cutting corners without understanding what is going on :(
Do you know why you can use formula M1 x V1 = M2 x V2?
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My lab background states that this a redox reaction with a one to one mole reation, and therefore M1 x V1 = M2 x V2 will apply.
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i think wkat borek tries to say is that what does the equation implies....
M1V1=M2V2
what does this equaiton mean....
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M1 = concentration of the component
V1 = volume of that component
M2= is the unknown
V2 = is the volume of the solution being added ( the question is does this volume include the added H20? )
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My lab background states that this a redox reaction with a one to one mole reation, and therefore M1 x V1 = M2 x V2 will apply.
Much better now. This equation is so often abused by neglecting stoichiometry, that I get sick when I see it in the context of titration.
What does MV product stand for?
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If you want to understand something :
1- start to write equation reaction
2 - Is it a 1 mole for 1 mole reaction?
3 - If yes, how many moles of titrating reagent did I use ?
4 -..