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# UOP - CHEM 027 - Class Notes - Week 3

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UOP - CHEM 027 - Class Notes - Week 3

##### Description: These notes cover basic concepts and definitions
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Chapter 17 Properties of Solutions  17.1 Solution Composition  Molarity: the number of moles of solute per liter of solution.   Mass percent: the percent solute by mass in the solution
Mass Percent = (grams of solute/grams of solution) x 100

Mole Fraction: it’s the ratio of the # of moles of a given component to the total number of moles of
solution

𝐴 =   𝑋 𝐴 = 𝑛 𝐴 𝑛 𝐴 + 𝑛 𝐵
17.2 Thermodynamics of Solution Formation

Solubility rules: Like dissolves like

Forming liquids Steps
1.  Expand solute
2.  Expand Solvent
3.  Combine these two

Enthalpy of solution: sum of energies used in expanding both solute and solvent.

Vitamins are divided into 2 categories: fat soluble and water soluble.

Pressure can increase the solubility of a gas.

Henry’s Law is the relationship between gas pressure and the concentration of a dissolved gas.
P = 𝑘
𝐻 𝑥  The law states that the amount of gas dissolved in a solution is directly proportional to the pressure of
the gas above the solution

Solid dissolving occurs more rapidly at higher temperatures and the amount of solid that dissolves
increases/decreases w increasing temperature

When temperature increases, gases become more soluble in nonaqueous solvents.

Volatile solutions tend to go from solution to vapor phase rather quickly.

Adding a nonvolatile solute to a solvent makes the solvent less likely to evaporate.

𝑅𝑎𝑜𝑢𝑙𝑡 𝑠 𝐿𝑎𝑤 𝑋 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 𝑃 𝑠𝑜𝑙𝑣𝑒𝑛𝑡
X-solvent is the mole fraction of the solvent and P solvent is the vapor pressure of the solution.

Any solution that obeys Raoult’s law is an ideal solution.

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##### Description: These notes cover basic concepts and definitions
2 Pages 21 Views 16 Unlocks
• Notes, Study Guides, Flashcards + More!
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