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5. What is the importance of standardization on this experiment ?

5. What is the importance of standardization on this experiment ?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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) +
21:36 4. Based on the introduction given above, deduce an experimental procedure that is in point form, concise, easy to follow and based only on two tablets named A and B for the title given experiment 5. What is the importance of standardization on this experiment? Add a caption... > Status (Custom) +
Transcribed Image Text:21:36 4. Based on the introduction given above, deduce an experimental procedure that is in point form, concise, easy to follow and based only on two tablets named A and B for the title given experiment 5. What is the importance of standardization on this experiment? Add a caption... > Status (Custom) +
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