A 500-mg antacid tablet has magnesium carbonate (MW = 84.3139 g/mol) and it was reacted with vinegar. Assuming that the acetic acid in the vinegar is the excess reactant, the only carbonate present in the tablet is the one compounded with the magnesium and all carbonate ions (FW = 60.008 g/mol) were converted to carbon dioxide, what is the %(w/w) of carbonate ion in the tablet when 0.15 grams of carbon dioxide (MW = 44.01 g/mol) was produced from the reaction?

A 500-mg antacid tablet has magnesium carbonate (MW = 84.3139 g/mol) and it was reacted with vinegar. Assuming that the acetic acid in the vinegar is the excess reactant, the only carbonate present in the tablet is the one compounded with the magnesium and all carbonate ions (FW = 60.008 g/mol) were converted to carbon dioxide, what is the %(w/w) of carbonate ion in the tablet when 0.15 grams of carbon dioxide (MW = 44.01 g/mol) was produced from the reaction?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 98AP

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