A 0.750g of antacid containing NaHCO3 was treated with 25.00mL of 0.0800M HCl solution, heated to...

A 0.750g of antacid containing NaHCO3 was treated with 25.00mL of 0.0800M HCl solution, heated to drive off CO2, and then titrated to a pale blue endpoint with 5.61mL of 0.09132 M NaOH titrated. What is the mass percent of NaHCO3 in the tablet and how many moles of stomach acid can be neutralized per gram of tablet?

Solutions

Expert Solution

The chemical reactions that happens in the medium are the following:

- First hydrochloric acid (HCl) reacts sodium bicarbonate (NaHCO3) to for carbonic acid (H2CO3) and sodium chloride (NaCl) as shown below:

- Carbonic acid is decomposed into carbon dioxide (CO2) and water (H2O) by heating. CO2(aq) escapes from solution in the form gaz CO2(g) by heating.

- The excess of HCl remained in the solution after reaction with bicarbonate and heating is titrated by NaOH (back titration) as shown by the equation:

Based on the stoichiometry of the reactions given:

1 tablet can neutralize mol of stomach acid.

queen_honey_blossom answered 2 weeks ago

Next > < Previous

Related Solutions

A solution containing a mixture of metal cations was treated with dilute HCl and a precipitate...

A solution containing a mixture of metal cations was treated with dilute HCl and a precipitate formed. The solution was filtered and H2S was bubbled through the acidic solution. A precipitate again formed and was filtered off. Then, the pH was raised to about 8 and H2S was again bubbled through the solution. This time, no precipitate formed. Finally, the solution was treated with a sodium carbonate solution, which resulted in formation of a precipitate. Which metal ions were definitely...

Suppose that 200.0mL of a 0.1220 M HCL solution was added to a full antacid tabet...

Suppose that 200.0mL of a 0.1220 M HCL solution was added to a full antacid tabet containing CaCO3. The HCl fully reacted with the CO3^2- and the excess HCL was then back titrated with a 0.1050 M NaOH solution. The back titratin required 32.20 mL based on this data, calculate the moles of CaCO3 in the balet and the weight of CaCo3 IN THE TABLET (the molecular weight of CaCO3 is 100.09 g/mol) What would these calculations look like?

Suppose that you first titrated 25.00mL of 0.500M HCl with 0.500M NaOH and then 25.00mL of...

Suppose that you first titrated 25.00mL of 0.500M HCl with 0.500M NaOH and then 25.00mL of 0.500M of your weak acid HA with 0.500M NaOH. How would the titration curves compare at 15.00mL of NaOH beyond the equivalence points?

What is the percent by mass of NaHCO3 in a solution containing 20.0 g of NaHCO3 dissolved in 600 .0 mL of H2O?

A 25.00mL of a 0.500M trimethylamine ((C2H5)3N) solution is titrated against 0.625M HCl. Answer the following...

A 25.00mL of a 0.500M trimethylamine ((C2H5)3N) solution is titrated against 0.625M HCl. Answer the following questions or calculate the pH after the addition of each of the following volumes of HCl solution. If it is the equivalence point or the midpoint, note it. (Kb=5.6x10^-4) a. 0.00mL HCl b. 10.00 mL HCl c. 20.00mL HCl d.40.00mL HCl e. 60.00mL HCl f. At what pH would this make a good buffer? g. Select an appropriate indicator for this titration. (NEED HELP...

Antacid tablets contain a variety of bases such as NaHCO3, MgCO3, CaCO3, and Mg(OH)2. Only NaHCO3...

Antacid tablets contain a variety of bases such as NaHCO3, MgCO3, CaCO3, and Mg(OH)2. Only NaHCO3 has appreciable solubility in water. In parts 1 - 4, write a balances net ionic equation, including states of matter, for the reaction of each antacid with aqueous HCl. Then in part 5 choose the best statement to describe antacids. Part 1 a) Write the net ionic equation for NaHCO3 + HCl b)Write the net ionic equation for MgCO3 + HCl c)Write the net...

what volume of 0.200 m HCl solution is needed to neutralize 0.400 g of NaHCO3

A wastewater is simulated as a solution containing 10-2.7 M NaHCO3 and 10-3 M NH4Cl. a....

A wastewater is simulated as a solution containing 10-2.7 M NaHCO3 and 10-3 M NH4Cl. a. List the dissolved species that you expect to be present in solution. b. Prepare a log C-pH diagram for the system, and calculate the pH of the solution. c. In order to remove nitrogen by volatilizing NH3 gas, 148 mg/L Ca(OH)2 (lime) will be added to raise the pH and convert NH4+ to the NH3(aq) form. Calculate the pH after lime addition. (Assume that...

25.00mL of 0.25M of AgNO3 react with 20.00mL of 0.150M of HCl. Find the mass of...

25.00mL of 0.25M of AgNO3 react with 20.00mL of 0.150M of HCl. Find the mass of precipitate.

A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of...

A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.03742 M EDTA solution. The solution is then back titrated with 0.02190 M Zn2 solution at a pH of 5. A volume of 20.48 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...

Subjects