Chemistry, Chapter 4

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

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
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- 
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

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)....
View Full Document

Ask a homework question - tutors are online