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© University of South Carolina Board of Trustees Spaghetti Science What happens somewhat before a pot of water boils? ●Bubbles form on sides of the pot.

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Presentation on theme: "© University of South Carolina Board of Trustees Spaghetti Science What happens somewhat before a pot of water boils? ●Bubbles form on sides of the pot."— Presentation transcript:

1 © University of South Carolina Board of Trustees Spaghetti Science What happens somewhat before a pot of water boils? ●Bubbles form on sides of the pot.

2 © University of South Carolina Board of Trustees Chapt. 12 Solutions Sec. 3 Does Higher Temperature Increase Solubility?

3 © University of South Carolina Board of Trustees Solubility Experiments

4 HeatX Heat + X (s) + solvent X (sol) © University of South Carolina Board of Trustees Effect of Temperature on Solubility X Heat + X (s) + solvent X (sol)  H pos. (endothermic)  Temp.  Temp.,  Solubility    Temp. = add heat X Heat + X (s) + solvent X (sol)    

5 XHeat X (s) + solvent X (sol) + Heat © University of South Carolina Board of Trustees Effect of Temperature on Solubility  H neg. (exothermic)  Temp.  Temp.,  Solubility    Temp. = add heat X X (s) + solvent X (sol) + Heat    

6 © University of South Carolina Board of Trustees Example Problem What happens somewhat before a pot of water boils? ●Bubbles form on sides of the pot. ●N 2 /O 2(gas)  N 2 /O 2(sol) + heat ●Nitrogen and oxygen have a negative enthalpy of solution (exothermic). ●Gas solubility is decreasing. Draw a conclusion about the enthalpy of solution of air.

7 © University of South Carolina Board of Trustees Chapt. 12 Solutions Sec. 3 Does Higher Pressure Increase Solubility?

8 © University of South Carolina Board of Trustees Pressure and Solubility ●Gases  Pressure,  Solubility ●Liquids little effect ●Solidslittle effect

9 © University of South Carolina Board of Trustees Pressure and the Solubility of Gases Doubling the pressure ______ the solubility of gases. doubles Henry’s Law m = k P Conc. in solution Pressure of gas Henry’s Law Constant (table) (partial) (in a mixture) (William) (1803)

10 © University of South Carolina Board of Trustees Example Problem If the atmospheric CO 2 level is 0.03 mole %, how many grams of CO 2 will be dissolved in 1 L of water at 20  C?

11 © University of South Carolina Board of Trustees Henry’s Law Constants in Water (molal/atm) Gas0 o C20 o C40 o C60 o C CO x x x x10 -2 C 2 H x x x He4.22 x x x x10 -4 N x x x x10 -4 O x x x x10 -4

12 © University of South Carolina Board of Trustees Chapt. 12 Solutions Sec. 4 Colligative Properties

13 © University of South Carolina Board of Trustees Adding a nonvolatile solute to a pure solvent causes: lower vapor pressure higher boiling point lower freezing point osmotic pressure Colligative Properties

14 © University of South Carolina Board of Trustees Adding a nonvolatile solute to a pure solvent causes:  lower vapor pressure  P = P  x  sol  lower vapor pressure  P = - P  x  sol higher boiling point lower freezing point osmotic pressure Colligative Properties

15 © University of South Carolina Board of Trustees Vapor Pressure Lowering Benzene pure 0.02 mol frac 0.04 mol frac 0.06 mol frac 0.08 mol frac

16 © University of South Carolina Board of Trustees Boiling Point Elevation Benzene pure 0.02 mol frac 0.04 mol frac 0.06 mol frac 0.08 mol frac

17 © University of South Carolina Board of Trustees Adding a nonvolatile solute to a pure solvent causes: lower vapor pressure  P = - P  x  sol  higher boiling point  T = + k b x m sol lower freezing point osmotic pressure Colligative Properties

18 © University of South Carolina Board of Trustees Example Problem Find the molar mass of a solute, if a solution of 1.33 g of the compound dissolved in 25.0 g of benzene has a boiling point of o C.

19 © University of South Carolina Board of Trustees Adding a nonvolatile solute to a pure solvent causes: lower vapor pressure  P = - P  x  sol  higher boiling point  T = + k b x m sol lower freezing point osmotic pressure Colligative Properties Mole-Meter


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