You weigh out an antacid tablet and determine the mass to be 1.1990 g. After taking...

You weigh out an antacid tablet and determine the mass to be 1.1990 g. After taking a 0.2455 g sample of the antacid tablet, you dissolve it in 25.00 mL of a 0.1006 M solution of hydrochloric acid in a 250.0 mL Erlenmeyer flask. After heating the solution to get rid of carbon dioxide, you titrate the leftover hydrochloric acid in the solution in the Erlenmeyer flask with a 0.09913 M solution of sodium hydroxide and determine that it takes 14.71 mL of the sodium hydroxide solution to react with the leftover hydrochloric acid in solution. Determine the milligrams of calcium carbonate in the sample of antacid tablet and then determine the milligrams of calcium carbonate in the entire antacid tablet.

What indicator will be used for this titration reaction? What color change will occur?

Expert Solution

CaCO3 + 2 HCl ---------------> CaCl2 + H2O + CO2

moles of HCl added = 25.00 x 0.1006 / 1000

= 2.515 x 10^-3

moles of NaOH needed to neutralize the excess HCl = 14.71 x 0.09913 / 1000

= 1.458 x 10^-3

moles of HCl used = 2.515 x 10^-3 - 1.458 x 10^-3

= 1.057 x 10^-3

moles of CaCO3 = 1/2 x moles of HCl

= 5.284 x 10^-4

mass of CaCO3 = 0.05284 g in 1.1990 g tablet

mass of CaCO3 in 0.2455 g = 0.0065187 g

mass of CaCO3 in entire tablet = 6.5187 mg

indicator used is = phenolphthalein

color change = pink

queen_honey_blossom answered 2 years ago

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