It’s really not that bad

 mol - the quantity of a given substance that contains as many molecules or formula units as the number of atoms in exactly 12g of carbon-12. (the number is 6.02x10 23 )  Think of a mol as a dozen  Example: you can have 2 dozen roses or you can have 2 mol NaCl

 The mass in grams of one mol of a substance  How do we find Molar Mass??  Take the mass number from the periodic table and add each amount together  Example: H 2 O H = 1O = 16 Therefore: = 18grams/mol

 You will use the molar mass as a conversion factor  Example: If you need 1.5 moles of salt to make a solutions how many grams do you need to measure?

 Follow the same steps. The trick is to make sure your units cancel!  Example: How many moles is in 150 grams of H 2 SO 4 ?

 A homogeneous mixture – a mixture that is uniform in its properties throughout the sample

 The moles of solute dissolved in one liter of solution.  M = mol / L  So for a 2 molar solution of HCl you would disslolve 2 moles of HCl into 1 liter of water

 So when are we going to use all this chemistry?  Example: Make 250mL of a 6 molar concentrated solution of sugar – C 6 H 12 O 6. How many grams of sugar do you need to measure out?

 You can also dilute solutions by adding more solvent to the solution.  M i x V i = M f x V f  Example: Make 250mL of 2 Molar HCl from 6 Molar HCl.