Chemistry, Chapter 4

Chemistry, Chapter 4 - [perchlorate salts are soluble II...

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I. Net Equations a. Only strong  soluble  electrolytes are written as ions . i. Seven strong acids:  H2SO4 (aq) [sulfuric acid], HNO3 (aq) [nitric acid],  HClO3 (aq) [chloric acid], HClO4 (aq) [perchloric acid], HCl (aq)  [hydrochloric acid], HBr (aq) [hydrobromic acid], HI (aq) [hydroiodic acid] ii. Three strong soluble bases:  Na(OH) (aq) [sodium hydroxide], KOH (aq)  [potassium hydroxide], Ba(OH)2 (aq) [barium hydroxide] iii. All soluble salts. b. Solubility Rules i. All Na+ [sodium], K+ [potassium], NH4+ [ammonium] salts are soluble. ii. All NO3- [nitrate], C2H3O2- [acetate], ClO3- [chlorate], ClO4- 
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Unformatted text preview: [perchlorate] salts are soluble. II. Types of Reactions that Essentially Go to Completion a. Precipitation reactions b. Gas-forming reactions c. Acid/base neutralization d. Reduction/oxidation III. Solution Concentrations a. Molarity (M) = (moles solute)/(Liters solution) b. M = (moles)/liter or moles = M*L *In writing net equation for reaction: A) Write molecular equation and balance it. B) Then use rules to obtain resulting net equation (indicates driving force of reaction)....
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This note was uploaded on 03/27/2008 for the course CHEM 103 taught by Professor Wendt during the Fall '07 term at University of Wisconsin.

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