Ch.3 - Molecules and Compounds

Problem 84

Previous problem

Next problem

Chapter 3, Problem 84

Copper(II) fluoride contains 37.42% F by mass. Calculate the mass of fluorine (in g) in 23.8 g of copper(II) fluoride.

Verified step by step guidance

Identify the percentage of fluorine in copper(II) fluoride, which is given as 37.42%.

Convert the percentage to a decimal by dividing by 100, resulting in 0.3742.

Multiply the decimal form of the percentage by the total mass of copper(II) fluoride to find the mass of fluorine: 0.3742 * 23.8 g.

Set up the multiplication to calculate the mass of fluorine in grams.

Perform the multiplication to find the mass of fluorine in the given sample of copper(II) fluoride.

Verified Solution

Video duration:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Mass Percent Composition

Mass percent composition is a way to express the concentration of an element in a compound, calculated as the mass of the element divided by the total mass of the compound, multiplied by 100. In this case, knowing that copper(II) fluoride contains 37.42% fluorine by mass allows us to determine how much of a given mass of the compound is due to fluorine.

Calculating Mass from Percent Composition

To find the mass of an element in a compound using its percent composition, you multiply the total mass of the compound by the mass percent (expressed as a decimal). For example, if you have 23.8 g of copper(II) fluoride, you would calculate the mass of fluorine by taking 23.8 g and multiplying it by 0.3742 (the decimal form of 37.42%).

Unit Conversion

Unit conversion is essential in chemistry for ensuring that measurements are in the correct units for calculations. In this context, while the mass of copper(II) fluoride is given in grams, understanding how to convert between different units (if necessary) is crucial for accurate calculations, especially when dealing with larger or smaller quantities.

Recommended video:

Conversion Factors

Related Practice

Most fertilizers consist of nitrogen-containing compounds such as NH₃, CO(NH₂)₂, NH₄NO₃, and (NH₄)₂SO₄. Plants use the nitrogen content in these compounds for protein synthesis. Calculate the mass percent composition of nitrogen in CO(NH₂)₂.

1368

views

Textbook Question

Iron in the earth is in the form of iron ore. Common ores include Fe₂O₃ (hematite), Fe₃O₄ (magnetite), and FeCO₃ (siderite). Calculate the mass percent composition of iron for each of these iron ores. Which ore has the highest iron content?

1468

views

Textbook Question

Silver chloride, often used in silver plating, contains 75.27% Ag by mass. Calculate the mass of silver chloride required to plate 123 mg of pure silver.

Textbook Question

The iodide ion is a dietary mineral essential to good nutrition. In countries where potassium iodide is added to salt, iodine deficiency (or goiter) has been almost completely eliminated. The recommended daily allowance (RDA) for iodine is 150 mg/day. How much potassium iodide (76.45% I) should you consume if you want to meet the RDA?

1365

views

Textbook Question

The American Dental Association recommends that an adult female should consume 3.0 mg of fluoride (F^-) per day to prevent tooth decay. If the fluoride is consumed in the form of sodium fluoride (45.24% F), what amount of sodium fluoride contains the recommended amount of fluoride?

1422

views

Textbook Question

Write a ratio showing the relationship between the molar amounts of each element for each compound. (See Appendix IIA for color codes.) (a)

576

views