Answer the following: 1. Write the reaction for the following: Solutions of sodium iodide and lead nitrate are mixed 2. Write the formula for the following compounds and write if they are soluble or insoluble in solution: A. barium sulfate B. Hyrosulfuric acid C. Carbon dioxide D. silver nitrate E. sodium carbonate F. Silver chromate

10/9 Pre-AP Pick up a blue folder, YOUR SCANTRON, and a calculator. TURN IN REVIEW HW: DENISTY POGIL ON TEST: You must keep answers covered at all times. If a question requires you to show work, you must do that or you will lose credit. Box your answers in the FRQ. No naked numbers and don’t kill babies.  DIRECTIONS FOR TURNING IN YOUR TEST: 1. Turn test into basket UPSIDE DOWN. 2. Put the periodic table folder back in the purple container 3. Clear your calculator and place it back in the holder. 4. Pick up Density pogil and quietly work on it while others are finishing test

10/9 AP Turn in your lab report WITH THE RUBRIC TO THE FRONT OF THE LAB REPORT (given to you on side STAPLED table). MAKE SURE YOUR NAME AND PERIOD ARE ON THE REPORT. Do not turn in the precipitation HW TURN IN STOICHIOMETRY HW IF HAVEN’T ALREADY You will need: you equation writing books, the equation writing notes, something to write with, and a periodic table. We will finish going through DR reactions and then go over Acid Base reactions. HW: Precipitation reactions/Acid Base practice from notes (I will assign this during class) Reminder: POSSIBLE SOLUTIONS TEST ON FRIDAY

Copy following solubility rules (FOR HW) 1. Strong acids are soluble 2. Strong bases are soluble Hydroxides (OH-) of group 1 are soluble Hydroxides (OH-) of group 2 are soluble EXCEPT Mg and Be 3. Group 1 AND NH4+ are soluble 4. Soluble salts: 5. Molecular compounds are INSOLUBLE 6. Assume INSOLUBLE FOR EVERYTHING ELSE Always Soluble in compound Except Nitrate, group 1, ammonium, acetate, perchlorate, chlorate NONE Cl-, Br-, I- (halides) When bonded to: Pb2+, Ag+, Hg2+ Sulfate (SO42-) Sr, Ba,Ca

WRITING AP EQUATIONS

General Guidelines AP equation sets are found in the free- response section of the AP test. You are expected to: write balanced net ionic equations for three reactions when given the reactants answer a question concerning that reaction

4.4 Types of Chemical Reactions There are three general types of solution reactions. Precipitation reactions (most often include double replacement and complex ion) Acid base reactions (also called neutralization) Oxidation reduction reactions (most often single replacement, combustion, synthesis and decomposition) (FOR THIS UNIT, WE WILL LEARN PRECIPITATION AND NEUTRALIZATION)

These equations are written in terms of: molecular equation –overall reaction stoichiometry complete ionic equation –all electrolytes are represented as ions net ionic equation- spectator ions aren’t included

4.5 Precipitation Reactions In a double replacement reaction, two compounds react to form two new compounds. No changes in oxidation numbers occur. All double replacement reactions must have a "driving force" that removes a pair of ions from solution.

Write the following information on the page labeled precipitation rxn (DR): Double replacement reaction: *Two compounds react to form two new compounds. *No changes in oxidation numbers occur. All double replacement reactions must have a "driving force" that removes a pair of ions from solution. *“Switch partners”: The metal/cation “switch” places with each other. The nonmetal/anion “switch” places with each other. *There are three driving forces for these reactions.

On the opposite page: You will write the following EXAMPLES: 1. Formation of a precipiate” Ex. Solutions of lead (II) nitrate and potassium chloride are mixed 2. Formation of a gas Ex 1. Hydrochloric acid and potassium carbonate react Ex 2. Hydrochloric acid and potassium sulfite are mixed Ex 3. Sodium hydroxide and ammonium chloride react 3. Formation of a molecular compound Ex. Solution of hydrobromic acid and lithium hydroxide react

FIRST DRIVING FORCE” Formation of a precipitate A precipitate is an insoluble substance formed by the reaction of two aqueous substances. Two ions bond together so strongly that water can not pull them apart. You must know your solubility rules to write these net ionic equations to determine which product, if any, will precipitate in a double replacement reaction.

Ex. Solutions of silver nitrate and lithium bromide are mixed. AgNO3(aq) + LiBr(aq)  AgBr(s) + LiNO3(aq) Ag+ + NO3- + Li+ + Br-  AgBr + Li+ +NO3- Ag+ + Br-  AgBr

SECOND DRIVING FORCE: Formation of a gas Gases may form directly in a double replacement reaction or can form from the decomposition of a product such as H2CO3,H2SO3, or NH4OH

Ex. Excess hydrochloric acid solution is added to a solution of potassium sulfite. 2HCl(aq) + K2SO3(aq)  H2O(l) + SO2(g) + 2KCl(aq) 2H+ + 2Cl- + 2K+ + SO32-  H2O + SO2 + 2K+ +2Cl- 2H+ + SO32-  H2O + SO2

Ex. A solution of sodium hydroxide is added to a solution of ammonium chloride. NaOH(aq)+NH4Cl(aq)NaCl(aq)+NH3(g)+H2O(l) Na+ + OH- + NH4+ + Cl- Na+ + Cl- + NH3 + H2O OH- + NH4+  NH3 + H2O

THIRD DRIVING FORCE Formation of a molecular substance When a molecular substance such as water or acetic acid is formed, ions are removed from solution and the reaction "works".

OH- + H+  H2O (HBr, HCl, and HI are strong acids) Ex. Dilute solutions of lithium hydroxide and hydrobromic acid are mixed. LiOH(aq) + HBr(aq)  LiBr(aq) +H2O(l) Li+ + OH- + H+ + Br-  Li+ +Br- + H2O OH- + H+  H2O (HBr, HCl, and HI are strong acids)

Ex. Gaseous hydrofluoric acid reacts with solid silicon dioxide. 4HF(g) + SiO2(s) SiF4(g) + 2H2O(l) 4HF + SiO2  SiF4 + 2H2O

AP 10/11 DO NOT TURN IN EQUATION WRITING HW PICK UP THE NOTES PACKET Take out your mystery lab, something to write with, a highlighter, and your equation writing book We will review DR reactions, go over neutralization reactions, and then finish the lab HW: read through the solution notes, write the equations for the numbers assigned, and answer the questions on the solubility curve

HW: Pg 15-17: 1,2,3,4,5,6,7,10, 11,12,15,17,18,20,23,26,29,33,36,38 Pg 17-18: 3,6,12,15

4. 8 Acid-Base Reactions Brønsted-Lowry acid-base definitions: acid- proton donor base- proton acceptor

Neutralization When a strong acid reacts with a strong base the net ionic reaction is: H+(aq) + OH-(aq) H2O(l) Watch out for information about quantities of each reactant!

Strong and Weak Acids and Bases Remember which acids are strong (ionize completely) and which are weak (write as molecule). Sulfuric acid solution (strong acid) should be written as H+ and HSO4-. Concentrated strong acids must be left together as they do not have enough water to ionize.

Practice on white boards: Write and equation showing the ionization of hydrochloric acid Write an equation showing ionization of hydrosulfuric acid Write an equation showing the ionization of magnesium hydroxide Write an equation showing the ionization of strontium hydroxide Write an equation showing the ionization of sulfuric acid

Write on the left side of the neutralization page: In solution Produces a salt and water if ionizes completely Three types: 1. Strong Acid/Strong Base *always has following net ionic if base soluble H+ + OH- H2O 2. Strong Acid and Strong Base or Weak Acid and Strong Base *reaction is complete *NOTE: If it says the acid or base is concentrated you leave it together completely B/C there is not enough water to ionize completely 3. Solutions reacting with a pure solid or pure liquid or it’s concentrated If the problem says solid or liquid or concentrated acids/bases, you keep it together

Example of Acid/Base 1. hydrochloric acid and calcium hydroxide 2. Sulfuric acid reacts with barium hydroxide 3. solid potassium hydroxide is added to a solution of sulfuric acid

Examples Ex. A solution of sulfuric acid is added to a solution of barium hydroxide until the same number of moles of each compound has been added. H+ + HSO4- + Ba2+ + 2OH-  BaSO4 + 2H2O Ex. Hydrogen sulfide gas is bubbled through excess potassium hydroxide solution. H2S + OH-  H2O + HS- *(S2- does not exist in water)

Examples Watch out for substances that react with water before reacting with an acid or a base. These are two step reactions. Ex. Sulfur dioxide gas is bubbled into an excess of a saturated solution of calcium hydroxide. SO2 + Ca2++ 2OH-  CaSO3 + H2O