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Mass Measurements In Chemistry

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  1. Mass Measurements In Chemistry Calculating Formula Weight

  2. I CAN calculate the formula weight (molar mass) of a compound from it’s formula.

  3. We’ve talked about the mass of atoms in terms of one or two….but these masses are very small. To be practical for laboratory work, a standard of measure had to be derived so that mass quantities could be easily measured. To that end, scientists created a unit called the ATOMIC MASS UNIT used to measure the mass of subatomic particles.

  4. The mass of a proton or neutron was assigned a value of 1 atomic mass unit (amu). To create a system of practical measurement, scientists used the atom CARBON-12 [6 P+ and 6 No] and assigned it a mass of 12 AMU. Then they calculated the number of atoms required to make a mass of 12 grams of Carbon-12. They found it took 6.022 x 1023 atoms of C-12 to have a mass of 12 grams. In turn, each element’s atomic mass required 6.022 x 1023 atoms to equal the same mass in grams.

  5. FOR EXAMPLE 1 atom of Oxygen 16 weighs 16 AMU . 6.022 x 1023 atoms of O-16 weighs 16 grams! This number became very important in chemistry is known as: Avagadro’s Number

  6. The quantity of matter containing Avagadro’s Number of particles, such as atoms, molecules or formula units, is known as a: Mole When working in a lab setting, the MOLE is used to determine quantities of chemicals.

  7. Mass Calculations and Chemical Formulas • Chemical Formulas represent the ELEMENTSand the NUMBER OF ATOMS of each that compose a compound. • Subscripts in formulas relate to the element immediately IN FRONT of them. • If a formula contains a PARENTHESIS followed by a subscript, the subscript multiplies ALL elements inside.

  8. EXAMPLE Ca3(PO4)2 3 atoms Ca 2 atoms P 8 atoms O

  9. Calculating Formula Weight (Molar Mass) • Formula Weight(Molar Mass)of an element or compound is the MASS in GRAMS of ONE MOLE of the element or compound. • For an element, the FW is the ATOMIC MASS from the periodic table, or for a particular ISOTOPE. • For a compound, the FW is found by counting the number of each kind of atom. • Multiply the number of atomsX the Atomic Mass Number of the element (from the PT). • Add the results and round to significant figures.

  10. Example • What is the formula weight of Calcium Carbonate? • CaCO3 From Formula From Periodic Table 1mole CaX 40.08g = 40.08 g 1 mole C X 12.011 g = 12.011 g 3 moles O X 15.9994 g = + 47.9982g ________________ = 100.0892 g = 100.09 g/mole

  11. Hydrates • Certain ionic compounds trap water molecules in their structure when they form. • These are known as HYDRATES. • Hydrates are written in this manner: • Compound Formula Dot Number of Water Molecules • CuSO4 5H2O • Hydrates are named as: • Compound Name, a Prefix for the number of water molecules, then the word Hydrate. • When calculating the formula weight of a hydrate, just include the mass of the number of water molecules in the total.

  12. Practice Problem • What would be the formula weight of Magnesium Chlorate Pentahydrate? • Formula = Mg(ClO3)25H2O • 1 mole Mg x 24.305 g = 24.305 g • 2 moles Cl x 35.453 g = 70.906 g • 6 moles O x 15.999 g = 95.994 g • 10 moles H x 1.0079 g = 10.079 g • 5 moles O x 15.999 g = 79.995 g • 281.279 g/mole

  13. PRACTICE PROBLEMS • Complete the following FORMULA WEIGHT (MOLAR MASS) calculations ON YOUR OWN PAPER! • 1. Find the formula weight of Aluminum Sulfate, Al2(SO4)3. • 2. What is the MOLAR MASS of Glucose, C6H12O6? • 3. Find the FORMULA WEIGHT of: Sodium Potassium Permanganate Tetrahydrate NaK(MnO4)2 4H2O • 4. What is the MOLAR MASS of Ammonium Phosphate Dihydrate.