4. An old antacid commercial claimed that each tablet of their product could "neutralize 47 times its mass in stomach acid". The active ingredient in the antiacid tablet, NaAl(OH)₂CO3, reacts with HCl in stomach acid according to this balanced reaction: NaAl(OH)₂CO3 + 4 HCl →→ NaCl + AlCl3 + 3H₂O + CO₂ How many moles of HCl can a 1.03 g of antiacid tablet neutralize if the tablet contains 0.246 g of the active ingredient?
4. An old antacid commercial claimed that each tablet of their product could "neutralize 47 times its mass in stomach acid". The active ingredient in the antiacid tablet, NaAl(OH)₂CO3, reacts with HCl in stomach acid according to this balanced reaction: NaAl(OH)₂CO3 + 4 HCl →→ NaCl + AlCl3 + 3H₂O + CO₂ How many moles of HCl can a 1.03 g of antiacid tablet neutralize if the tablet contains 0.246 g of the active ingredient?
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
Chapter4: Types Of Chemical Reactions And Solution Stoichiometry
Section: Chapter Questions
Problem 120AE: Saccharin (C7H5NO3S) is sometimes dispensed in tablet form. Ten tablets with a total mass of 0.5894...
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Question
![4.
An old antacid commercial claimed that
each tablet of their product could "neutralize 47
times its
mass in stomach acid". The active
ingredient in the antiacid tablet, NaAl(OH)₂CO3,
reacts with
HCl in stomach acid according to this
balanced reaction:
NaAl(OH)₂CO3 + 4 HCl →→ NaCl + AlCl³ + 3 H₂O + CO₂
How many moles of HCl can a 1.03 g of
antiacid tablet neutralize if the tablet
contains 0.246 g of the active ingredient?
If stomach acid has a concentration of 0.14
M HCl, assuming the density of stomach
acid to be similar to that of water (1.00
g/mL), what is the mass of stomach acid
that the 1.03 g of antiacid tablet can
neutralize? Does this number support the
claim in the commercial?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe7417eb4-c4f6-4b23-b299-1f887648c283%2Fbd2172c2-372b-46a8-a637-0291ffc5ef35%2F01uscdj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:4.
An old antacid commercial claimed that
each tablet of their product could "neutralize 47
times its
mass in stomach acid". The active
ingredient in the antiacid tablet, NaAl(OH)₂CO3,
reacts with
HCl in stomach acid according to this
balanced reaction:
NaAl(OH)₂CO3 + 4 HCl →→ NaCl + AlCl³ + 3 H₂O + CO₂
How many moles of HCl can a 1.03 g of
antiacid tablet neutralize if the tablet
contains 0.246 g of the active ingredient?
If stomach acid has a concentration of 0.14
M HCl, assuming the density of stomach
acid to be similar to that of water (1.00
g/mL), what is the mass of stomach acid
that the 1.03 g of antiacid tablet can
neutralize? Does this number support the
claim in the commercial?
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