Ions in Solution
- Structure of Ionic Compounds (overhead fig 3.13)
- Solvation of Ionic Compounds (overhead fig 3.15)
- KMnO4 ( , Internet© Saunders, 1997)
- Strong and Weak Acids & Bases, CD-ROM 4-7 & 4-8 (overhead table 4.1)
4.6 Precipitation Reactions
- potassium chromate and lead nitrate produces lead chromate and potassium nitrate( ,Internet© Saunders, 1997)
)
K2CrO4 (aq)
+ Pb(NO3)2 (aq)
- > PbCrO4 (s) + 2 KNO3 (aq)
- lead nitrate and potassium iodide produces lead iodide and potassium nitrate( Internet© Saunders, 1997)
Pb(NO3)2 (aq) + 2 KI (aq)
-> PbI2 (s) + 2 KNO3 (aq)
- silver nitrate and sodium chloride produces silver chlroide and sodium nitrate( Internet© Saunders, 1997)
AgNO3 (aq) + NaCl aq) - > AgCl (s) + NaNO3 (aq)
- iron (III) Ions + Sodium hydroxide produces iron (iii) hydroxide and sodium ions( Internet)
Fe3+ (aq) + 3 NaOH (aq) - > Fe(OH)3 (s) + 3 Na1+(aq)
- Solubility Rules
4.7 Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations
4.8 Acid-Base and Gas-Evolution Reactions
- Definitions of acids and bases
- Arrhenius definition (in water only)
- Acids, produce H+ in water solution: HCl (aq) -> H+(aq) + Cl-
- Bases, produce OH- in water solution: NaOH(aq) -> Na+ + OH-
- Bronsted-Lowry Acids and bases (more general definition)
- Acids are proton donors in a chemical reaction
- HCl (g) + H2O -> H3O+ + Cl-
- Acid + Base -> Base + Acid
- Bases are proton acceptors in a chemical reaction
- NaOH + H2O -> Na+ + H3O+
- Base + Acid -> Acid + Base
- Common Acids (know names of all strong acids)
- Monoprotic - Single H+
- Polyprotic - more than 1 H+, ie: diprotic, triprotic
- H2SO4 + H2O -> H3O1+ + HSO41-
- HSO41- + H2O -> H3O1+ + SO42-
- Strong acids (dissociate completely)
- Weak acids (partially dissociate, introduce equlibrium)
- Common Bases
- Strong Bases (alkali metal hydroxides)
- Weak bases (ammonia)
- Aqueous Acid-Base Reactions
- Total Equation: HCl(aq) + NaOH(aq) -> H2O(l) + NaCl(aq)
- Ionic Equations
- Dissociation
- HCl (g) -> H+(aq) + Cl-(aq) OR HCl(g) + H2O(l) -> H3O+(aq) + Cl-(aq)
- NaOH -> Na+(aq) + OH-(aq)
- Neutralization (spectator ions): H3O+ + Cl- + Na+ + OH- -> 2 H2O + Na+ + Cl-
- Net Ionic Equation: H3O+ + OH- -> 2 H2O
- Example Reactions
- Magnesium Hydroxide + Nitric Acid
- Total equation
- Ionic Equation
- Net ionic equation
- Sulfuric acid and lithium hydroxide
- Total equation
- Ionic Equation
- Net ionic equation
- Acetic acid and iron (III) hydroxide
- Total equation
- Ionic Equation
- Net ionic equation
- Ammonia (NH3) and water( Internet)
- hydrochloric acid and ammonia produces ammoinum and chloride
- hydrochloric acid and sodium hydroxide produces sodium chloride and water; no indicator
4.9 Oxidation-Reduction Reactions
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Department of Chemistry
Widener University
Chester, PA 19013
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This page has been accessed
times since 5/30/97.
Last Updated Friday, May 25, 2001 1:59:43 PM