More Challenging Questions These questions require more thought and integrate several c...

More Challenging Questions

These questions require more thought and integrate several concepts.

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.