A Rolaids tablet contains calcium carbonate for neutralizing stomach acid. If a Rolaids tablet neutralizes 24.65 mL of 0.547 M hydrochloric acid, how many milligrams of calcium carbon are in a Rolaids tablet?
1 Answer
Explanation:
Your starting point here will be the balanced chemical equation for this neutralization reaction.
Calcium carbonate,
#"CaCO"_ (3(s)) + color(red)(2)"HCl"_ ((aq)) -> "CaCl"_ (2(aq)) + "H"_ 2"O"_ ((l)) + "CO"_ (2(g)) uarr#
Notice that it takes
The problem provides you with the molarity and volume of the hydrochloric acid solution. This means that you can use the definition of molarity to find how many moles of acid it contained
#color(blue)(c = n/V implies n = c * V)#
#n_(HCl) = "0.547 M" * 24.65 * 10^(-3)"L" = "0.013484 moles HCl"#
Use the aforementioned mole ratio to find the number of moles of calcium carbonate that must have been present in the Rolaids table
#0.013484 color(red)(cancel(color(black)("moles HCl"))) * ("1 mole CaCO"_3)/(color(red)(2)color(red)(cancel(color(black)("moles HCl")))) = "0.0067420 moles CaCO"_3#
Finally, to find the mass of calcium carbonate that contains this many moles, use the compound's molar mass
#0.0067420 color(red)(cancel(color(black)("moles CaCO"_3))) * "100.1 g"/(1color(red)(cancel(color(black)("mole CaCO"_3)))) = "0.645 g"#
Expressed in milligrams, the answer will be
#0.645 color(red)(cancel(color(black)("g"))) * (10^3"mg")/(1color(red)(cancel(color(black)("g")))) = color(green)("645 mg")#
The answer is rounded to three sig figs.