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Chapter 3: Problem 48

Tin(II) fluoride \(\left(\mathrm{SnF}_{2}\right)\) is often added to toothpaste as an ingredient to prevent tooth decay. What is the mass of \(\mathrm{F}\) in grams in \(24.6 \mathrm{~g}\) of the compound?

Short Answer

Expert verified
The mass of fluorine in 24.6 g of the compound is approximately 5.97 grams.

Step by step solution

01

Calculate the molar mass of Tin(II) fluoride

The molar mass of Tin(II) Fluoride (\(SnF_2\)) is calculated by adding the molar masses of Sn and 2F. The molar mass of Sn is 118.7 g/mol and that of F is 19.0 g/mol. So, the molar mass of \(SnF_2\) = 118.7 g/mol + 2 * 19.0 g/mol = 156.7 g/mol.
02

Calculate the moles of Tin(II) fluoride

Using the mass and molar mass of \(SnF_2\), to calculate the number of moles use the formula: moles = mass/molar mass. Plug in the values and get moles of \(SnF_2\) = \(24.6 g / 156.7 g/mol\) = 0.157 mol.
03

Find the mass of fluorine

There are 2 moles of F in each mole of \(SnF_2\). Therefore, the moles of F in 0.157 moles of \(SnF_2\) = \(2 * 0.157 mol\) = 0.314 mol. To find the mass of F, multiply the moles of F by its molar mass. Mass of F = \(0.314 mol * 19.0 g/mol\) = 5.966 g.

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