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7.3 Using Chemical Formulas Review Mole: SI unit for the amount of a substance (contains avogadro’s number of particles) Avogadro’s Number: 6.022 x 10 23 particles/molecules/formulas units per 1 mol Formula Unit: smallest ratio of cations to anions

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2) Formula Mass Sum of the average atomic masses of all atoms represented in a formula (Units: amu) Ex: What is the formula mass of Ca(NO 3 ) 2 ?

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3) Molar Mass mass of one mole of any substance (contains avogadro’s number of particles) Units: g/mol Ex: calculate the molar mass of Al 2 S 3

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4) Problem Solving Using Molar Mass A) Mol to mass Ex: What is the mass (grams) of 3.0 mol of NaOH? 1. determine molar mass of NaOH 2. # of moles of NaOH x molar mass

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B) mass to mol How many moles are in 135 g of NaOH? 1. determine molar mass of NaOH 2. grams of NaOH / molar mass

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C) Moles to molecules / molecules to moles How many molecules of H 2 0 are present in 1.5 mol? 1. mol NaOH x Avogadro’s #

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6. Determining % Composition A) from chemical formula Ex – Find the % composition of copper (II) sulfate? Formula -> molar mass -> mass of each element as % (disregard letter 6.B)

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6) Determing % Composition B) from mass data

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