Chapter 3: Problem 51
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 grams of SnF2 is approximately 5.96 grams.
Step by step solution
01
Understand the problem
We are given a total mass of 24.6 g for the compound \( \text{SnF}_2 \) and need to find the mass of the element Fluorine (F) present in this compound.
02
Find the Molar Mass of \( \text{SnF}_2 \)
Calculate the molar mass of \( \text{SnF}_2 \) using the periodic table. Tin (Sn) has an atomic mass of approximately 118.71 g/mol and Fluorine (F) 19.00 g/mol. The formula \( \text{SnF}_2 \) has one Sn and two F atoms:\[\text{Molar mass of SnF}_2 = (1 \times 118.71) + (2 \times 19.00) = 156.71 \text{ g/mol}\]
03
Determine the Mass Fraction of Fluorine
Calculate the mass of Fluorine in one mole of \( \text{SnF}_2 \), then find the mass fraction. With 2 Fluorine atoms:\[\text{Mass of F in SnF}_2 = 2 \times 19.00 = 38.00 \text{ g}\]The mass fraction of Fluorine is:\[\text{Mass fraction of F} = \frac{38.00}{156.71}\]
04
Calculate Mass of F in Given Sample
Use the mass fraction to find the mass of Fluorine in 24.6 g of \( \text{SnF}_2 \):\[\text{Mass of F} = \text{Total mass} \times \text{Mass fraction of F} = 24.6 \times \left(\frac{38.00}{156.71}\right)\]
05
Solve the Calculation
Perform the arithmetic:\[\text{Mass of F} = 24.6 \times 0.2426 \approx 5.96 \text{ g}\]
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Molar Mass
Understanding molar mass is essential for solving chemistry problems that involve calculations with substances. Molar mass is the mass of one mole of a substance, usually expressed in grams per mole (g/mol).
It's computed by adding up the atomic masses of all the atoms in a given formula, which are readily found in the periodic table.
For example, in tin(II) fluoride, or \( \text{SnF}_2 \), the molar mass is determined as follows:
It's computed by adding up the atomic masses of all the atoms in a given formula, which are readily found in the periodic table.
For example, in tin(II) fluoride, or \( \text{SnF}_2 \), the molar mass is determined as follows:
- Tin (\( \text{Sn} \)) has an atomic mass of about 118.71 g/mol.
- Fluorine (\( \text{F} \)) has an atomic mass of about 19.00 g/mol.
- The formula \( \text{SnF}_2 \) includes one Sn atom and two F atoms.
Stoichiometry
Stoichiometry is the area of chemistry that involves the relative quantities of reactants and products in chemical reactions. It connects deeply with molar mass by allowing us to transition between amounts of chemicals in moles and their masses in grams.
In exercises like the one tackled here, stoichiometry helps deduce how much of a specific component, like fluorine in \( \text{SnF}_2 \), is present in any given mass of the whole compound.
This process involves setting up a ratio based on the molar masses and then using proportions to find unknown quantities. Using stoichiometry ensures that we're accounting for every part of the molecules in reactions, whether they are reactants or products.
In exercises like the one tackled here, stoichiometry helps deduce how much of a specific component, like fluorine in \( \text{SnF}_2 \), is present in any given mass of the whole compound.
This process involves setting up a ratio based on the molar masses and then using proportions to find unknown quantities. Using stoichiometry ensures that we're accounting for every part of the molecules in reactions, whether they are reactants or products.
Mass Fraction
The mass fraction is a way to determine the ratio of the mass of a part to the total mass of a compound. It is highly useful when assessing how much of a specific component is in a compound.
Calculating the mass fraction of an element involves dividing the total mass of that element in one mole of the compound by the total molar mass of the compound itself.
In our example, to find the mass of fluorine in \( \text{SnF}_2 \):
This value means that 24.26% of \( \text{SnF}_2 \)'s mass is from fluorine.
Calculating the mass fraction of an element involves dividing the total mass of that element in one mole of the compound by the total molar mass of the compound itself.
In our example, to find the mass of fluorine in \( \text{SnF}_2 \):
- The total mass of fluorine in one mole of \( \text{SnF}_2 \) is 38.00 g.
- The molar mass of \( \text{SnF}_2 \) is 156.71 g/mol, as calculated earlier.
This value means that 24.26% of \( \text{SnF}_2 \)'s mass is from fluorine.
Tin(II) fluoride
Tin(II) fluoride, sometimes referred to as stannous fluoride, is commonly known for its use in dental care products, particularly toothpaste.
Its chemical formula \( \text{SnF}_2 \) consists of one tin atom and two fluorine atoms.
Its chemical formula \( \text{SnF}_2 \) consists of one tin atom and two fluorine atoms.
- The element tin in this compound contributes to the structural stability of the molecule.
- Fluoride, derived from fluorine, plays a significant role in preventing tooth decay.