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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?

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 1 year ago

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