One tablet of Maalox clams to contain 600 mg CaCO3. If 10 mLof 0.100 M NaOH titr

Question

One tablet of Maalox clams to contain 600 mg CaCO3. If 10 mLof 0.100 M NaOH titrant is to be used to back titrate the excess0.100 M HCl from the analysis of one-third of a Maalox tablet, howmany milliliters of 0.100 M HCl must have initially been added tothe 200 mg Maalox sample?
show work please
show work please

Explanation / Answer

1 tablet contains 600 mg CaCO3 So 1/3 tablet contains 200 mg CaCO3 CaCO3 + 2HCl-> CaCl2 + H2CO3 200 mg CaCO3 = .200 grams Molecular weight CaCO3: 40.1 + 12 + 3(16) = 100 Find the moles of CaCO3: .200 grams / 100 grams/mol = .002 moles Since 1 mole of CaCO3 requires 2 mole of HCl (look at equationabove) .002 moles x 2 = .004 moles of HCl needed to titrate the tablet # of moles of excess HCl added = amount required for neutralizationby NaOH moles of NaOH : .010 L x .100 M = .001 moles Total moles of HCl: .001 + .004 = .005 moles Volume: moles / M = .005 / .100 = .05 L or (.05 x 1000 = 50 mL)

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