Slide 1

Mix the following solutions in pairs Write down the solution pairs and record your results Potassium Iodide Barium Nitrate Lead Nitrate When finished, try Silver Nitrate with Potassium Iodide.

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Precipitate Reactions Precipitates Solubility rules Using the rules of solubility

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Reaction of PbNO 3 and KI Lead II Nitrate and Potassium Iodide Both are strong electrolytes That means they completely dissociate into ions Adding the solutions together will create something new A chemical change the evidence is the precipitate.

Slide 4

Pb (NO) 3 Look closer at Lead (II) Nitrate Strong Electrolyte Ions completely dissociate into: Lead Pb 2+ ions Nitrate NO 3 - Ions

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The KI does the same thing Posassium K+ ions and Iodide I- ions form. They are floating around in the water. (an aqueous solution)

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Slide 7

When the lead and the iodide ions come into contact, they form a precipitate The precipitate falls to the bottom, spectator ions are left in solution

Slide 8

KI.Potassium Iodide With Lead nitrate it forms Lead Iodide, A yellow precipitate. This tells us that the iodide compoud PbI 2 is not soluble So are all Iodide compounds insoluble? If you mix with barium nitrate, Ba(NO 3)2 You might expect Barium Iodide BaI 2 to form a ppt.

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The rules can be broken into 4 categories. 1 solubleno exceptions 2 solublesome exceptions 3 not solublesome exceptions 4 not solublefew exceptions

Slide 10

Solubility Rules: Always Always Soluble 1. Always Soluble: Li +, Na +,K +, NH 4 + Group 1A(Alkali Metals) and ammonium compounds are soluble. C 2 H 3 O 2 -, NO 3 -, ClO 3 -, ClO 4 - Acetates, Nitrates, Chlorates, Perchlorates are all soluble.

Slide 11

The solubility rules: Usually soluble Cl -, Br -, I - Most chlorides, bromides and Iodides are soluble Exceptions AP/H (Ag) Silver: AgCl, AgBr, AgI (Pb) Lead (II) PbCl 2, PbBr 2, PbI 2 (Hg) Mercury (I): Hg 2 Cl 2, Hg 2 Br 2, Hg 2 I 2 F - Most fluorides are soluble Exceptions CBS-PM Calcium, Barium, Strontium, Lead, Magnesium MgF 2, CaF 2, SrF 2, BaF 2 Lead (II) PbF 2 SO 4 2- Most Sulfates are soluble Exceptions CBS/PBS Calcium, Strontium, Barium, Lead (II) CaSO 4 SrSO 4 BaSO 4 PbSO 4

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The solubility rules: Usually NOT Soluble O 2-, OH - Most hydroxides and oxides are insoluble Exceptions: CBS CaO, Ca(OH) 2 SrO, Sr(OH) 2 BaO, Ba (OH) 2 And the always group of Alkali metals and Ammonium

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The solubility rules: Insoluble Ions Not soluble CO 3 2- PO 4 3- SO 3 2- S 2- C 2 O 4 2- CrO 4 2- Exceptions: The things that are always soluble. Group 1A (Alkali Metals) Li 2 CO 3, Na 2 CO 3 etc Ammonium compounds (NH 4 ) 2 CO 3

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Types of reactions Remember net ionic equations?

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Showing everything in the reaction vessel (beaker, well plate, test tube

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Sometimes parts of the equation do nothing but sit and watch. Spectators

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Complete ionic vs. net ionic Sodium sulfate + Barium Chloride react to form Solid barium sulfate and Sodium chloride 2 Na + (aq) + SO 4 2- (aq) + Ba 2+ (aq) + 2 Cl - (aq) BaSO 4 (s) + 2 Na + (aq) + 2 Cl - (aq) NaCl is a strong electrolyte, so it does not combine to form a solid

Slide 18

Stoichiometry in Aqueous Reactions What volume of 0.200 M copper (II) sulfate is required to react with 50.0mL if 0.100 M NaOH? 1) Write the net ionic equation Cu 2+ (aq) + 2 OH - (aq) Cu(OH) 2 (s)

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What volume of 0.200 M copper (II) sulfate is required to react with 50.0mL if 0.100 M NaOH? find the moles of each reactant needed: n OH - = n Cu 2+ =