The concentration of Ca ion in a town's water supply is 0.0020M (this water is referred to as hard water because it contains such a large concentration of Ca2+.) Suppose the water is to be fluorinated by the addition of NaF for the purpose of reducing tooth decay (the most common health policy in most US counties).
The concentration of Ca ion in a town's water supply is 0.0020M (this water is referred to as hard water because it contains such a large concentration of Ca2+.) Suppose the water is to be fluorinated by the addition of NaF for the purpose of reducing tooth decay (the most common health policy in most US counties).
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.35PAE: In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial...
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![The concentration of Ca ion in a town's water supply is 0.0020M (this water is referred to as hard water because it contains
such a large concentration of Ca2+.) Suppose the water is to be fluorinated by the addition of NaF for the purpose of reducing
tooth decay (the most common health policy in most US counties).
a. What is the maximum concentration of fluoride ion that can be achieved in the water before precipitation of CaF2
begins?
b. How much NaF needs to be added to obtain the maximum concentration of F in this solution?
10- M (1 mg
c. Will the water supply attain the level of F- recommended by the U.S. Public Health Services, about 5
fluoride per liter)?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Facdff4fe-7c73-4882-a39a-fd8ef8420048%2F808ebb38-4dd5-48e5-bb06-fe846adfc3de%2Fj6ybyup_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The concentration of Ca ion in a town's water supply is 0.0020M (this water is referred to as hard water because it contains
such a large concentration of Ca2+.) Suppose the water is to be fluorinated by the addition of NaF for the purpose of reducing
tooth decay (the most common health policy in most US counties).
a. What is the maximum concentration of fluoride ion that can be achieved in the water before precipitation of CaF2
begins?
b. How much NaF needs to be added to obtain the maximum concentration of F in this solution?
10- M (1 mg
c. Will the water supply attain the level of F- recommended by the U.S. Public Health Services, about 5
fluoride per liter)?
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