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16 Cards in this Set
- Front
- Back
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Solution
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A homogeneous mixture; can be liquids, solids, or gases
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Molarity
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Number of moles per of solution (mol/L)
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Mass percent
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(grams of solute) / (grams of solution) X 100%
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Mole Fraction
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n(A) / n(A) + n(B)
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Molality
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(molesof solute) / (kilograms of solvent)
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3 steps to creating a liquid solution
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1) (ENDOTHERMIC) expand solute - break it up into indiviual components
2) (ENDOTHERMIC) expanding the solvent - overcoming intermolecular forces in the solvent to make more room for the solute 3) (EXOTHERMIC) allowing the solute and solvent to interact to form the solution |
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ΔH
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ΔH(soln) = ΔH(1) + ΔH(2) + ΔH(3)
positive ΔH = endothermic (energy absorbed) negative ΔH = exothermic (energy released) |
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ΔH(hyd)
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ΔH(2) + ΔH(3)
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Standard enthalpy of solution
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sum of ΔH(1) andΔH(hyd)
ΔH(soln) = ΔH(1) + ΔH(hyd) |
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Gibbs free energy
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ΔG = ΔH - TΔS
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Driving force of "like dissolves like"
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ΔS(soln)
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Supercritical fluid
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when a substance s heated beyond its critical temperature
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Fat-Soluble
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Fat soluble (vitamins A, D, E, K) are non polar and composed mostly of carbon and hydrogen atoms, similar electronegativities making it virtually nonpolar, dissolves in body fat which is also nonpolar
*HYDROPHOBIC* |
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Water-Soluble
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Water soluble (Vitamins B and C) has many polar O-H and C-O bonds making it polar
*HYDROPHILIC* |
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Henry's Law
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the amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the solution
P=kC or P=k(h)x C=concentration of gas in mol/L k=L atm/mol P=partial pressure x=mole fraction k(H)=Henry's law constant |
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Thermal pollution
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**SOLUBILITY OF A GAS IN WATER DECREASES WITH INCREASING TEMPERATURE**
1) water is used as a coolant 2) returned to its natural source - water is less dense so floats on top and allows for less oxygen absorption - returned water contains less oxygen required for aquatic life |
