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At the end of the experiment how will you determine which tablet is more effective than the other

At the end of the experiment how will you determine which tablet is more effective than the other

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 82E: The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they...
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At the end of the experiment how will you determine which tablet is more effective than the other
21:34 Acid indigestion is a common ailment caused by the overproduction of stomach acid, HCI. Over-the-counter antacids provide some relief from the symptoms of acid indigestion. They are generally made up of some mixture of weak bases such as Mg(OH)2, Al(OH)s, and Cacos that can react with acid as shown in these net ionic equations: H*(aq)+OH"(aq)- H2O(1) 2H"(aq) +CO"(aq) - H2O(1)+CO:(g) In this exercise, the method of titration will be used to determine the number of moles of H+ neutralized per gram of antacid. In the "back-titration," a portion of antacid will be mixed with an excess of HCI. The H* that has not reacted with the antacid is then titrated with standardized NaOH in the presence of the indicator bromophenol blue to a blue end point. Total moles of H* = moles of H* neutralized by antacid + moles of H* neutralized by NaOH Because the antacid includes both OH and CO23, it is not possible to calculate the number of moles of each these ion species independently. Instead, the number of H* neutralized by the antacid is found. The amount of antacid required to neutralize one mole of H* neutralized is said to be one "equivalent." total equivalent of antacid=total mole of H' neutralized Add a caption... > Status (Custom) +
Transcribed Image Text:21:34 Acid indigestion is a common ailment caused by the overproduction of stomach acid, HCI. Over-the-counter antacids provide some relief from the symptoms of acid indigestion. They are generally made up of some mixture of weak bases such as Mg(OH)2, Al(OH)s, and Cacos that can react with acid as shown in these net ionic equations: H*(aq)+OH"(aq)- H2O(1) 2H"(aq) +CO"(aq) - H2O(1)+CO:(g) In this exercise, the method of titration will be used to determine the number of moles of H+ neutralized per gram of antacid. In the "back-titration," a portion of antacid will be mixed with an excess of HCI. The H* that has not reacted with the antacid is then titrated with standardized NaOH in the presence of the indicator bromophenol blue to a blue end point. Total moles of H* = moles of H* neutralized by antacid + moles of H* neutralized by NaOH Because the antacid includes both OH and CO23, it is not possible to calculate the number of moles of each these ion species independently. Instead, the number of H* neutralized by the antacid is found. The amount of antacid required to neutralize one mole of H* neutralized is said to be one "equivalent." total equivalent of antacid=total mole of H' neutralized Add a caption... > Status (Custom) +
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