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Chemistry (181)
CHM 113 (103)
Ron Briggs (24)
Lecture

Electrolytes & Acids/Bases

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Department
Chemistry
Course
CHM 113
Professor
Ron Briggs
Semester
Fall

Description
 Precipitation Reaction: Replacement reacting in which a solid precipitate is formed in a solution  Dissociation: Break up of soluble ionic compounds into ions in solution o Solubility: The ability of a substance (the solute) to dissolve in the solvent  Solubility Rules tell us which compounds are soluble o Appendix J of lab manual & Pg 121 of textbook  Electrolyte: Solution of ions that conducts and electric current o Strength depends on how many ions are formed in the solution  Strong electrolytes: Nearly 100% dissociation (Many ions)  More ions=Stronger electrolyte solution o Al(NO ) 3 3aCl o Al(NO ) 3 3 4 ions, NaCl has 2 ions  Examples: Any soluble ionic compound in H O 2  Strong acids  Strong bases  Weak electrolytes: Only some dissociation (Few ions)  Weak acids  Weak bases  Non-electrolytes: No dissociation (No ions)  Molecular/covalent bonded compounds o H O2  Hydrocarbons o Unless a weak/strong acid/base  Ionic Equations:  What happens when Pb(NO ) (a3) and NaI (aq) are mixed together in a solution? o Determine the ions that form when mixed together 2+ -  Pb(NO )3 2q) →+b (aq)+-O (aq) 3  NaI(aq) →Na (aq)+I (aq) o Predict new possible products  New combinations: Na +NO →NaNO - 2+ - 3 3  Pb +I→PbI 2 o Write
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