CHEMISTRY

posted by .

If a tablet contains 129 mg of Mg(OH)2 and 505 mg of CaCO3, how many moles of HCl would theoretically be neutralized?

  • CHEMISTRY -

    Mg(OH)2 + 2HCl ==> MgCl2 + 2H2O
    CaCO3 + 2HCl ==> CaCl2 + H2O + CO2

    mols Mg(OH)2 = 0.129/molar mass = ?
    mols CaCl3 = 0.505/molar mass.

    ?mol Mg(OH)2 x 2 = mols HCl
    ? mol CaCO3 x 2 = mols HCl
    Total mols HCl = sum of the above.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Mylanta is composed of aluminum hydroxide and calcium carbonate. assuming that a mylanta tablet contains 175 mg of aluminum hydroxide and 145 mg of cakcium carbonate, answer the following: how many mL of 0.00836 M HCL (aq) can be neutralized …
  2. chemistry

    A beaker contains 250.0 mL of a 1.00 M HCl solution. How many moles of the acid would remain in the solution after 0.199 moles of HCl are neutralized?
  3. CHEMISTRY

    ANTACID TABLET OF WEIGHT 1.3183G WAS DISSOLVED IN 75 MLOF CONC. HCl OF 0.1807M IS TITRATED WITH 20.36ML OF CONC. NaOH OF 0.1481M . FIND MILIMOLES OF HCl ADDED, FIND MILIMOLES OF NaOH USED IN TITRATION, FIND MILIMOLES OF HCl THAT DID …
  4. chemistry

    CaCO3(s) + 2 HCl(aq) --> CaCl3(aq) + H2O(l) + CO2 It takes 19.26 mL of 0.6721 M HCl to completely react with the CaCO3. What is the mass of CaCO3 in the tablet?
  5. Chemistry

    4. A 5.309 g antacid tablet, with CaCO3 as the active ingredient, was mixed was 30.0 mL of 0.831 M HCl. It took 15.3 mL of 0.7034 M NaOH to neutralize the excess acid. a) Calculate the volume of HCl neutralized by the NaOH. b) Calculate …
  6. Chemistry

    Some antacid tablets actually contain a mixture of calcium carbonate and magnesium hydroxide (though they usually have the same “strength” as those that only contain CaCO3). If this had been the case for the antacid you tested, …
  7. Chemistry

    If a tablet of TUMS contains 500mg of the active ingredient, CaCO3, how many tablets would it take to neturalize the 1.5g of HCl?
  8. Chemistry

    Tums tablets contain CaCO3 that reacts with stomach acid as follows: CaCO3 (s) + 2HCl (aq) → CaCl2 (aq) + H2O (l) + CO2 (g)  Suppose the tablet was analyzed by adding 50.00 mL of 0.200 M HCl, which resulted in leftover …
  9. Chemistry

    Determine the mass of CaCO3 in your TUMS tablet?
  10. 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 neutralized …

More Similar Questions