Tin(II) fluoride (SnF2) is often added to toothpaste as an...

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?

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Key Concepts

Stoichiometric Calculations

Stoichiometric calculations involve using the relationships between reactants and products, as well as the conversion between moles and mass using the molar mass, to solve chemical problems. This includes determining how much of a component element is present in a given mass of a compound, which is essential for quantitative chemical analysis.

Molar Mass

Molar mass is the mass of one mole of a substance, calculated by adding together the atomic masses of all the atoms in its chemical formula. This concept is fundamental for converting between the mass of a sample and the number of moles, which is a central step in quantitative chemical calculations.

Percent Composition

Percent composition refers to the mass percentage of each element in a compound, determined by dividing the total mass of a specific element in one mole of the compound by the molar mass of the compound itself. This concept is crucial when calculating the mass of a particular element present in a given sample of a compound.

Transcript

00:04 So for this problem, we're told that we have 24 .6 grams of tin fluoride.

00:14 And we're trying to determine how many grams in 24 .6 grams of 10 fluoride is the fluoride itself.

00:25 So the way we can do this is by first in doing problems where we're going to use mole ratios and transfer things from grams to moles.

00:38 I find it best normally to start with what's given in the problem.

00:43 So in this case, that's 24 .6.

00:48 So write out 24 .6 grams of the tin fluoride.

00:56 And so first, in order to be able to compare that to fluoride to fluorine itself, we're going to want to compare it in terms of number of moles.

01:06 So first, we're going to have to convert this 24 .6 grams into moles, using the molecular weight that i calculated beforehand and wrote up here.

01:16 So 156 .17 grams moles, and this is tin fluoride.

01:27 Then we can stop here and calculate or just do all of the calculations in the end when we're done converting, which is what i like to do.

01:36 So now we're looking at our units being moles of tin fluoride.

01:40 So what we know is that in tin fluoride, it has, for every one unit of the compound tin fluoride, there are two units of fluorine.

01:58 So that helps us determine our mole ratio where for one mole of tin fluoride, there are two moles of fluorine.

02:13 Now back to mole ratios by matt...

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