The active ingredient in an antacid tablet is calcium carbonate, CaCO_3. One tab

Question

The active ingredient in an antacid tablet is calcium carbonate, CaCO_3. One tablet of a generic brand of antacid contains 270 mg of CaCO_3. What is the molar mass of CaCO_3? How many moles of CaCO_3 are in one roll, 12 tablets, of antacid? If a person takes two tablets, how many grams of calcium are obtained? If the daily recommended quantity of Ca^2+ to maintain bone strength in older women is 1500 mg, how many tablets are needed each day to supply the needed calcium? If two tablets are dissolved in 250 mL of water, what is the [Ca^2+] of the solution? Calcium carbonate reacts with aqueous HCl to make C0_2(g), H_2O(l) and CaCl_2(aq). Write a balanced equation for this reaction. If two tablets of antacid are added to 20.00 mL of 0.400 M HCl, how many grams of CO2 are produced? What is the volume of CO_2 produced for this reaction if P = 1.00 atm and T = 37 degree C?

Explanation / Answer

a) Molar mass of CaCO3 = Mass of Ca + Mass of C + Mass of 3O = 40.078 + 12.010 + 3* 15.999 = 100.085g/mol

b) 12 tablets contains = 12 * 270 mg = 3240 mg = 3.240 g

So, No of moles = Weight / Molecular Wt = 3.240 / 100.085 = 0.032 moles

C) 2 tablets contain = 2 * 270 = 540 mg = 0.540 g

d) Number of tablets required for 1500 mg = 1500/270 = 5.55 ( Around 5 and 1/2 tablet)

Thank You

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