chemistry

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.

  1. 👍
  2. 👎
  3. 👁
  1. CaCO3 + 2HCl ==> CaCl2 + H2O + CO2

    mols HCl added initially = M x L = approx 0.0025 but you need a more accurate answer than that estimate. That HCl is more than enough to dissolve all of the tablet and have some HCl left over.
    mols NaOH needed to neutralize the excess HCl = M x L = approx 0.0015.
    mols HCl used for the tablet is
    0.0025-0.0015 = approx 0.0010
    Convert mols HCl used in the neutralization of the tablet to mols CaCO3 using the coefficients in the balanaced equation. That will be mols CaCO3 = 1/2 x mols HCl.
    Convert to grams in the 0.2455 and then to mg. Then convert to mg in the entire sample.
    Post your work if you get stuck.

    1. 👍
    2. 👎
  2. FFFF

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    A solution formed by dissolving an antacid tablet has a pH of 9.18. Calculate [H+].

  2. Chemistry

    Different manufacturers claim to have the best antacid. Which of the following tablets would neutralize the most acid for the money? A. Rolaids (550 mg CaCO3 and 110 mg Mg(OH)2 per tablet) – 150 tablets for $9.44 B. Tums (500 mg

  3. Chemistry

    Determine the mass of CaCO3 in your TUMS tablet? The weight of the tablet was 0.013g Concentration of HCl was 0.1494 M Volume of HCl was 95 mL Concentration of NaOH was 0.1422 M The average amount it took to titrate was 2.13 mL I

  4. chemistry

    A 5.309 g antacid tablet, with CaCO3 as the active ingredient, was mixed was 30.0 mL of 0.831 M HCl. After the reaction occurred, it took 15.3 mL of 0.7034 M NaOH to neutralize the excess acid. a) How much HCl (in mL) of was

  1. Chemistry

    Calculate the percentage by mass of the active ingredient in an antacid tablet that weighs 1.36 g if it contains 520 mg of calcium carbonate

  2. Chemistry

    Pharmacists sell tablets containing magnesium hydroxide, Mg(OH)2, to combat indigestion. A student carried out an investigation to find the percentage by mass of Mg(OH)2 in an indigestion tablet. The student reacted the tablet

  3. Science!

    If a bowling ball were moved from Earth to the moon, how would it's weight and mass change? A. The bowling ball would weigh the same, but it's mass would increase. B. The bowling ball would weigh the same, but it's mass would

  4. Chemistry

    A solution formed by dissolving an antacid tablet has a pH of 9.18. Calculate [H+].

  1. Chem 1212

    An antacid tablet containing calcium carbonate as an active ingredient required 9.19 mL of 0.0956 M H2SO4 for complete neutralization. The mass of the tablet was 0.193 g. What percent of calcium carbonate was in the tablet?

  2. chem

    How many mL of stomach acid (assume it is .035 M HCI) can be neutralized by an antacid tablet containing .231g Mg(OH)2?

  3. calculus

    I solved this problem, can someone check it to make sure I did it right. There are two parts to this intrepation and estimate of the value. Let C(t) be the total value of the US currency (coins and banknotes) in circulation at

  4. Chemistry

    An antacid tablet containing magnesium hydroxide instead of calcium carbonate was dissolved in 100.0 mL of 0.2893 M HCL. 10 mL of this solutions was titrated to endpoint with 25.20 mL of 0.1007 M NaOH. How much magnesium hydroxide

You can view more similar questions or ask a new question.