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Gen Chem Chapter 4 Week 5

by: Zaida Gomez

Gen Chem Chapter 4 Week 5 1341

Marketplace > Texas State University > Chemistry > 1341 > Gen Chem Chapter 4 Week 5
Zaida Gomez
Texas State

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These notes will cover part of chapter 4. - aqueous solution properties - electrolytes - rules for solubility
General Chemistry I
No professor available
Class Notes
General Chemistry
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This 1 page Class Notes was uploaded by Zaida Gomez on Tuesday October 11, 2016. The Class Notes belongs to 1341 at Texas State University taught by a professor in Fall. Since its upload, it has received 4 views. For similar materials see General Chemistry I in Chemistry at Texas State University.


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Date Created: 10/11/16
Chapter4 General Properties of Aqueous Solutions - Are homogenous mixtures of 2 substances - Substance in the greater quantity is solvent - Substance in the smaller quantity is usually called a solute Electrolytes Solutions that conduct electricity are called electrolytic (always ionic) and contains electrolytes Nonelectrolytes They don’t conduct electricity called nonelectrolytic and contains nonelectrolytes Reactions The ability for an aqueous solution to form is due to + - region on water to stabilize the ionic charge (called solvation) Strong Electrolyte Ionic compound that completely dissociates in solution (randomly dispursed) Metal, nonmetal will either stay as a precipitate or dissolve Weak Electrolyte Ionic compound only partially dissociates in solution Precipitation Reactions Precipitate- insoluble solids formed by the reaction of two solutions Soluble- substance dissolved into solvent Insoluble- does not dissolve into solvent Rules for Solubility 1. Alkali Metal and Ammonium are ALWAYS soluble 2. Nitrate and Acetate are ALWAYS soluble 3. Halogen is ALWAYS soluble (exceptions- Ag+, Hg2 2+, Pb 2+) 4. Sulfate is ALWAYS soluble (exceptions- Sr 2+, Ba 2+, Hg 2+, Pb 2+) 5. Hydroxide and Sulfide are always INSOLUBLE (exceptions- rule 1, Ca 2+, Sr 2+, Ba 2+) 6. Carbonate and Phosphate are always INSOLUBLE (exception is rule 1) Precipitation Reactions Steps to write/balance a precipitation reaction 1. Determine ions present in reactants 2. Write chemical formulas of products by combining the cation from 1 reactant with the anion of another, using the ionic charge to determine the subscripts in the chemical formulas 3. Check the water solubilities of the products. For a precipitation reaction to occur, at least one product must be insoluble in water 4. Balance the equation


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