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02-29-2008, 01:46 PM
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| How do I solve this question for Chemistry?
The question is: Municipal drinking water frequently has fluoride added to improve the dental health of the citizens. The "fluoride" is often present the range of 1.4ppm. But in reality, because the HF is a weak acid, this total "Fluoride" is a mixture of F- and HF, ir [HF] + [F-] = 1.4 ppm. Assuming the water is buffered sufficiently to assure that its pH is 4.4 and the concentration is 1.4 ppm "Fluoride", what percentage of the "fluoride" exists as fluoride ion, F-, and what percentage exists as HF molecules? How do I solve this?      |
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