CHEM 210 1st Edition Lecture 15Outline of Last Lecture I. Migration of Ions in a SolutionII. Determining Moles of Ions in Aqueous SolutionsIII. Writing Equations for Aqueous Ionic ReactionsOutline of Current Lecture IV. PrecipitatesV. Soluble Ionic CompoundsVI. Insoluble Ionic CompoundsVII. Strong/Weak Acids and BasesCurrent LectureWhen looking at a chemical equation, and a solid produces from two or more aqueous solutions, it is called a precipitate. (aq) + (aq) (s)Soluble Ionic Compounds are compounds that dissolve in water or aqueous solutions.- Groups 1A in the periodic table and NH4+ are all soluble.- Common nitrides, acetates, and most perchlorates are soluble.- Chlorides, bromides, and iodides are soluble, except those of Ag+, Pb 2+, Cu+, and Hg.Insoluble Ionic Compounds are compounds that cannot dissolve in water or aqueous solutions.- All common metal hydroxides, except those of group 1A in the periodic table, and larger members of group 2A, beginning with Ca+, are insoluble.- Common carbonates and phosphates, except those of group 1A and NH4+ are insoluble.- Common sulfides, except those of group 1, group 2 and NH4+ are insoluble.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.There are also strong/weak acids and bases in chemistry.Strong acids include;- HCl (hydrochloric acid)- HNO3 (nitric acid)- HBr (hydrobromic acid)- H2SO4 (sulfuric acid)- HI (hydroiodic acid)- HClO4 (perchloric acid)Weak acids are;- CH3COOH (acetic acid)- HF (hydrofluoric acid)- HN02 (nitrous acid)Strong bases include;- NaOH (sodium hydroxide)- KOH (potassium hydroxide)- Ba (OH)2 (barium hydroxide)Weak bases are;- NH3 (ammonia)- CH3NH2 (methylamine)- C5H5N
View Full Document