01/27/15 To Do: ▫Bell Work ▫Hydrated Crystals ▫Family Project ▫Pre-Lab Hydrated Crystals Lab. Bell Work: ▫Copy To Do list into Agenda. ▫Name the following compounds:  Al(NO 3 ) 3  Aluminum Nitrate  NaOH  Sodium hydroxide  Cu(NO 3 ) 2  Copper (II) nitrate H2SH2S  Hydrosulfuric acid  HClO 3  Chlorous acid  CCl4  Carbon tetrachloride

Announcements New Seats Google Science Fair SIN Procedure Changes: ▫No more test corrections, but retakes will be available. ▫Students who have a C- or below will receive after school detention on Thursdays to provide time for improvement (assignment corrections, test retakes, complete missing work, etc.).  You, your parents, and the administration will be notified. ▫ No Late Work without Mac Pass!  You have 4 for the semester, use them!  Complete them well, or you don’t get full credit.  May not use the last two weeks of the quarter.

Naming a Hydrate – Notes on pg.66 1.Name the crystal 2.Water is referred to as a hydrate. 3.Use the prefix to tell the number of water molecules. 4.The two have a dot (▪) between them.  Example: CaCl 2 ▪ 2 H 2 O  Use the rules above to try and name the compound on your own. 3

Naming a Hydrate 1.Name the crystal 2.Water is referred to as a hydrate. 3.Use the prefix to tell the number of water molecules. 4.The two have a dot (▪) between them.  Example: CaCl 2 ▪ 2 H 2 O  Calcium chloride dihydrate 4

Analyzing a Hydrate How do you find the amount of H2O in a hydrate? ▫You must find the number of moles of water present in 1 mole of the compound. ▫You must find the n coefficient of the H2O (xH2O) in the formula. ▫You will use the math we have learned to do this: 5.00 g BaCl2 hydrate – 4.26 g anhydrous BaCL2 = 0.74 g H2O Note: we knew the starting mass, heated off the H2O, and found the difference, which must be the H2O present. 5

Analyzing a Hydrate How do you find the amount of H 2 O in a hydrate? 5.00 g BaCl2 hydrate – 4.26 g anhydrous BaCL 2 = 0.74 g H 2 O Now lets figure out the moles present – you have to convert the masses to moles using the molar mass: 4.26 g BaCL 2 x 1 mol BaCL 2 = g BaCL g H 2 O x 1 mol H 2 O = g H 2 O Do the math and find the answer! 6

Analyzing a Hydrate How do you find the amount of H 2 O in a hydrate? 5.00 g BaCl2 hydrate – 4.26 g anhydrous BaCL 2 = 0.74 g H 2 O Now lets figure out the moles present – you have to convert the masses to moles using the molar mass: 4.26 g BaCL 2 x 1 mol BaCL 2 = mol BaCL g BaCL g H 2 O x 1 mol H 2 O = mol H 2 O g H 2 O Now calculate the ratio of H 2 O moles to BaCL 2 moles: 7

Analyzing a Hydrate How do you find the amount of H 2 O in a hydrate? 5.00 g BaCl2 hydrate – 4.26 g anhydrous BaCL 2 = 0.74 g H 2 O Now lets figure out the moles present – you have to convert the masses to moles using the molar mass: 4.26 g BaCL 2 x 1 mol BaCL 2 = mol BaCL g BaCL g H 2 O x 1 mol H 2 O = mol H 2 O g H 2 O Now calculate the ratio of H 2 O moles to BaCL 2 moles: x = moles H 2 O = mol H 2 O = 2.00 mol H 2 O = 2:1 ratio moles BaCL mol BaCL mol BaCL 2 8

Uses of Hydrates Why are hydrates useful? ▫They can absorbed water if in anhydrous form.  Used as drying agents ▫Hydrate form can be used to store water.  Used in solar panels. 9

Left Side Practice ▫Old Textbook, pg. 340, practice problems 63 & 64. ▫When complete, get Family Project Document and read through it. 10