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    Add as Friendchapter 13: The Nature of Solutions

    by: Rogers

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    1 : I. The Nature of Solutions(p. 401 - 410, 425 - 433) Ch. 13 & 14 - Solutions
    2 : A. Definitions Solution - homogeneous mixture Solvent - present in greater amount Solute - substance being dissolved
    3 : A. Definitions Solute - KMnO4 Solvent - H2O
    4 : B. Solvation Solvation – the process of dissolving First... Then... solute particles are separated and pulled into solution solute particles are surrounded by solvent particles
    5 : B. Solvation Strong Electrolyte Non- Electrolyte solute exists as ions only solute exists as molecules only Weak Electrolyte solute exists as ions and molecules DISSOCIATION IONIZATION View animation online.
    6 : B. Solvation Dissociation separation of an ionic solid into aqueous ions NaCl(s) ? Na+(aq) + Cl–(aq)
    7 : B. Solvation Ionization breaking apart of some polar molecules into aqueous ions HNO3(aq) + H2O(l) ? H3O+(aq) + NO3–(aq)
    8 : B. Solvation Molecular Solvation molecules stay intact C6H12O6(s) ? C6H12O6(aq)
    9 : B. Solvation “Like Dissolves Like”
    10 : B. Solvation Soap/Detergent polar “head” with long nonpolar “tail” dissolves nonpolar grease in polar water
    11 : C. Solubility concentration
    12 : C. Solubility Solubility maximum grams of solute that will dissolve in 100 g of solvent at a given temperature varies with temp based on a saturated soln
    13 : C. Solubility Solubility Curve shows the dependence of solubility on temperature
    14 : C. Solubility Solids are more soluble at... high temperatures. Gases are more soluble at... low temperatures & high pressures (Henry’s Law). EX: nitrogen narcosis, the “bends,” soda

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