+

The Mole

Chapter 10

+Previous Skills required for this chapter

Writing formulas from names for: Ionic compounds Covalent compounds Acids

Balancing equations

Predicting Products Minor emphasis, but still needed

+Skills to be learned

Determining molar mass Elements Compounds

Determining number of moles within a compound

Molar conversions Mole to mole; gram to mole; mole to gram; gram to mole;

mole to atoms; atoms to mole

Empirical Formula and Molecular formula

Formulas and naming hydrates

+The mole, what is it?

+Mole

6.02x1023 atoms

For a given molecule, one mole is a mass (in grams) whose number is equal to the atomic mass of the molecule.

In general, one mole of any substance contains Avogadro's Number of molecules or atoms of that substance.

This relationship was first discovered by Amadeo Avogadro (1776-1858) and he received credit for this after his death.

+Molar mass

Unit: g/mol

The amount of mass (in grams) for every one mole of the element or molecule.

For elements:

+Molar Mass

For compounds

+Conversion factors of molar mass

+Empirical and molecular formulas

Percent composition from experimental data

+Empirical and molecular formulas

Percent composition from the chemical formula

+Problems

What is the percent composition of phosphoric acid?

Which has the larger percent by mass of sulfur: H2SO3 or H2S2O8?

Calcium chloride is sometimes used as a de-icer. Calculate the percent by mass of each element in CaCl2.

Challenge: Sodium sulfate is used in the manufacture of detergents. Identify each of the component elements of sodium sulfate, and

write the compound’s chemical formula. Identify the compound as ionic or covalent. Calculate the percent by mass of each element in sodium sulfate.

+Empirical Formula

Empirical formula is the formula with the smallest whole-number mole ratio of the elements.

Steps to finding empirical formula. Given Percent by mass. Convert to moles. Determine the smallest value. Divide all numbers by smallest value. If whole numbers, they are the subscripts. If they are not,

multiply in order to reach a whole number.

+Step One: Given Percent by mass

If given percentage, turn % into g.

If given grams, continue on.

+Step Two: Convert to moles.

+Step Three: Determine the smallest value.

+Step Four: Divide by smallest number.

+Step Five: Answer?

+Problems

Determine the empirical formula for a compound that contains 35.98% aluminum and 64.02% sulfur.

Propane is a hydrocarbon, a compound composed only of carbon and hydrogen. It is 81.82% carbon and 18.18% hydrogen. What is the empirical formula?

Aspirin is the world’s most-often used medication. The chemical analysis of aspirin indicates that the molecule is 60.00% carbon, 4.44% hydrogen, and 35.56% oxygen. Determine the empirical formula for aspirin.

+Molecular Formula

Molecular formula specifies the actual number of atoms of each element in one molecule or formula unit of the substance.

Steps to determine Molecular formula Given Percent by mass. Convert to moles. Determine the smallest value. Divide all numbers by smallest value. If whole numbers, they are the subscripts. If they are not,

multiply in order to reach a whole number. Determine the molar mass of the EF (answer from previous step) Divide molar mass of EF by molar mass of MF (given) Multiply EF by answer in previous step.

+Step One: Given Percent by mass

If given percentage, turn % into g.

If given grams, continue on.

+Step Two: Convert to moles.

+Step Three: Determine the smallest value.

+Step Four: Divide by smallest number.

+Step Five: Answer?

+Step Five: Empirical Formula

+Last o’ the steps:

+Problems

A compound was found to contain 49.98g of carbon and 10.47g of hydrogen. The molar mass of the compound is 58.12g/mol. Determine the molecular formula.

A colorless liquid composed of 46.68% nitrogen and 53.32% oxygen has a molar mass of 60.01g/mol. What is the molecular formula?

When an oxide of potassium is decomposed, 19.55g of K and 4.00g of O are obtained. What is the empirical formula?

+Formulas of Hydrates

Hydrate is a compound that has a specific number of water molecules bound to its atoms.

Naming Hydrates on next slide

Anhydrous – without water

+Prefix Molecules of H2O

Formula Name

Mono- 1 (NH4)2C2O4H2O Ammonium oxalate monohydrate

Di- 2 CaCl22H2O Calcium chloride dihydrate

Tri- 3 NaC2H3O23H2O Sodium acetate trihydrate

Tetra- 4 FePO44H2O Iron(III) phosphate tetrahydrate

Penta- 5 CuSO45H2O Copper(II) sulfate pentahydrate

Hexa- 6 CoCl26H2O Cobalt(III) chloride hexahydride

Hepta- 7 MgSO47H2O Magnesium sulfate heptahydrate

Octa 8 Ba(OH)28H2O Barium hydroxide octahydrate

Deca 10 Na2CO310H2O Sodium carbonate pentahydrate

+Steps for determining hydrate formulas

1. Determine given

2. Determine mass of water lost

3. Convert masses to moles

4. Solve for ratio of moles of water to moles of solid

5. Write formula

+Step One

A 20g sample of a hydrate of nickel sulfate (NiSO4) lost 9.63g of water when heated. Determine the hydrate’s formula.

Hydrate is 20g

Water lost 9.63g

+Steps continued. . .

+Problems

An 11.75g sample of a common hydrate of cobalt(II) chloride is heated. After heating, 0.0712 mol of anhydrous cobalt chloride remains. What is the formula and name of this hydrate?

+Uses of hydrates

Hydrates absorb water Desiccants prevent moisture from intergering with the

sensitive electronic circuitry

Some store solar energy When the Sun’s energy heats the hydrate to a temperature

greater than 32 degrees Celsius, the single formula unit of Na2SO4 in the hydrate dissolves in the 10mol of water of hydration. In the process, energy is absorbed by the hydrate. This energy is released when the temperature decreases and the hydrate crystallizes again.

+

The End