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A 0.63% by weight aqueous tin(II) fluoride, SnF2, solution is used as an oral rinse in dentistry to decrease tooth decay.
(a) Calculate the SnF2 concentration in ppm and ppb.
(b) Calculate the molarity of SnF2 in the solution.
(c) Tin(II) fluoride is produced commercially by a series of steps that begin with reduction of cassiterite, SnO2, the principal tin ore, with carbon.
Once purified, the tin is reacted with hydrogen fluoride vapor to produce SnF2. Consider that one metric ton of cassiterite ore is reduced with sufficient carbon to tin metal in 80% yield. The tin is purified and reacted with sufficient hydrogen fluoride to produce SnF2 in 94% yield. Calculate how many 250.-mL bottles of 0.63% SnF2 solution could be prepared from the one metric ton of cassiterite by these steps.
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