Posted by Anonymous on Monday, November 21, 2011 at 12:32am.
You didn't provide the volume or M of the HCl and you must have that to answer this question.
You added an excess of HCl. How much HCl did you add? moles HCl = M x L = ?
Then you back titrated with NaOH. mols NaOH = M x L = ?
The difference in moles = moles of acid consumed by the TUMS. I would calculate each titration separately and divide the final result of each by the mass of the original sample which should give you moles H^+/grams and that times 2 will give moles/2 grams.
the volume and M of HCl is 0.1312M and 150mL
how do i find then excess of HCl
What volume of 0.1125 M K2Cr2O7 would be required to oxidize 48.16 mL of 0.1006 M Na2SO3 in acidic solution? The products include Cr3+ and SO42- ions.
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