1 / 9

Chapter 7–Reactions in Aqueous Solution

Chapter 7–Reactions in Aqueous Solution. Electrolytes Writing Chemical Equations for Aqueous Reactions Double Displacement or Exchange Reactions Precipitation Acid-Base Gas Formation Oxidation-Reduction Reactions (Redox) Single Displacement or Replacement Combustion

cody-byers
Télécharger la présentation

Chapter 7–Reactions in Aqueous Solution

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 7–Reactions in Aqueous Solution • Electrolytes • Writing Chemical Equations for Aqueous Reactions • Double Displacement or Exchange Reactions • Precipitation • Acid-Base • Gas Formation • Oxidation-Reduction Reactions (Redox) • Single Displacement or Replacement • Combustion • Synthesis or Combination • Decomposition

  2. Example 1 – Three Ways of Writing Chemical Equations Write balanced molecular, complete ionic, and net ionic equations for the following reactions: • AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq) • H2SO4(aq) + KOH (aq)  H2O(l) + K2SO4(aq)

  3. Solubility Rules for Ionic Compounds • Compounds containing Group IA metals, ammonium, acetates and nitrates are allsoluble. • Most halides (Group 7Al, chlorides, etc.) are soluble. Exceptions include Ag+, Pb2+, and Hg22+ halides. • Most sulfates are soluble. Exceptions include Ba+2, Sr2+, Ag+, Pb2+, and Ca2+ sulfates. • Most hydroxidesinsoluble. Exceptions include hydroxides of Group 1A metals, ammonium, Ca+2, Sr+2, and Ba+2. • Most phosphates, carbonates, chromates, and sulfides are insoluble. Exceptions include those compounds containing Group 1A metals and ammonium. • In addition, allacids are soluble!

  4. Example 2 - Precipitation Write balanced molecular, complete ionic, and net ionic equations for the reactions you would expect to occur when the following reagents are combined. If no reaction occurs, just write NO REACTION after the arrow. a. Li2SO4(aq) + Pb(NO3)2(aq)  b. K3PO4(aq) + NaBr(aq) 

  5. Example 3 - Neutralization Write balanced molecular, complete ionic, and net ionic equations for the reactions you would expect to occur when the following reagents are combined. If no reaction occurs, just write NO REACTION after the arrow. a. HI(aq) + NaOH(aq)  b. H2SO4(aq) + Sr(OH)2(aq) 

  6. Example 4 – Gas Formation Write balanced molecular, complete ionic, and net ionic equations for the reactions you would expect to occur when the following reagents are combined. If no reaction occurs, just write NO REACTION after the arrow. a. HCl(aq) + Na2CO3(aq)  b. HNO3(aq) + KHSO4(aq)  c. NH4Cl(aq) + KOH(aq) 

  7. Activity Series for Metals(and Hydrogen)

  8. Example 5 – Single Displacement Write balanced molecular equations for the reactions you would expect to occur when the following reagents are combined. If no reaction occurs, just write NO REACTION after the arrow. a. Fe(s) + Ni(NO3)2(aq)  b. Au(s) + ZnCl2(aq)  c. Ca(s) + HCl(aq) 

  9. Example 6 – Classifying Reactions Classify each of the following reactions. Note that a reaction may fall into more than one category. • Ca(s) + 2 H2O(l)  Ca(OH)2(aq) + H2(g) • Ba(NO3)2(aq) + K2S04(aq)  BaSO4(s) + 2KNO3(aq) • 2 C2H6(g) + 7 O2(g)  4 CO2(g) + 6 H2O(g) • 2 KClO3(s)  2 KCl(s) + 3 O2(g) • 2 HBr(aq) + Ca(OH)2(aq)  2 H2O(l) + CaBr2(aq) • 2 H2(g) + O2(g)  2 H2O(g)

More Related