chemistry

posted by .

A TUMS tablet was dissolved in 110.00 ml of 0.1022 M HCl and analyzed for CaCO3 according to the procedure described in the lab manual. It took 7.48 ml of 0.1005 M NaOH to reach the endpoint. Calculate the mass of CaCO3 in TUMS tablet to the correct number of significant figures

CaC03(aq)+ 2HCl(aq) = CaCl2 (aq)+ H2O(l)+ CO2(g)

NaOH(aq) + HCl(aq) = NaCl(aq)+ H20(l)

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    A student performs a back-titration to determine the cost -effectiveness of an antacid. A tablet with a retail cost of $0.053 is dissolved in 25.00 ml of 1.000 M HCl, then back-titrated with 1.000 M NaOH. Exactly 14.82 ml of NaOH solution …
  2. chemistry

    Calcium carbonate CaCO3 reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s)+2HCl(aq)->CaCl2(aq)+H2O(l)+CO2(g) Tums, an antacid, contains CaCO3. If Tums is added to 35.0 mL of 0.300 M HCl,how …
  3. Chemistry

    Calcium carbonate reacts w/stomach acid according to the following chemical equation. CaCO3+2HCl(aq)-> CaCl2(aq)+H2O(l)+CO2(g) A. Balance the eqaution B. Tums is one commercially sold antacid that contains CACO3. If Tums is added …
  4. 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 …
  5. CHEMISTRY

    Suppose a student adds 25.00 mL of 1.025 M HCl to a 1.50 g antacid tablet. The student boils and then titrates the resulting solution to the endpoint with 0.4969 M NaOH. The titration requires 21.3 mL NaOH to reach the endpoint. How …
  6. CHEMISTRY

    Suppose a student adds 25.00 mL of 1.025 M HCl to a 1.50 g antacid tablet. The student boils and then titrates the resulting solution to the endpoint with 0.4969 M NaOH. The titration requires 21.3 mL NaOH to reach the endpoint. How …
  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