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Solutions

Learn about solutions, their composition, and how to separate their components. Discover the process of solvation and ionization and understand why some ionization reactions are endothermic and others are exothermic. Explore different types of solutions and the concept of solubility.

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Solutions

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  1. Solutions A homogeneous mixture containing a solute dissolved in a solvent.

  2. Homogeneous mixtures • Any two samples have the same composition • particles are SO SMALL • atoms, molecules, ions • THEY CAN’T BE SEEN & will pass through a filter So how do you separate the components?

  3. Two or more substances with different boiling points can be separated using fractionaldistillation (ex. Crude oil)

  4. How do substances dissolve in each other?

  5. When a non-polar, organic molecule dissolves it breaks apart into individual molecules. Called solvation, & forms a non-electrolytic solution.

  6. Click the pic.

  7. NaCl separates into ions (called ionization). When the water molecules surround the ions its called hydration & it forms an electrolytic solution.

  8. How will these salts dissociate/ionize? NaCl(s)  Na+(aq) + Cl-(aq) Na2SO4(s)  2Na+(aq)+ SO42-(aq) Pb(NO3)2 (s) Pb2+(aq)+ 2NO3-(aq)

  9. Why are some ionization reactions endothermic and some exothermic????

  10. Forming a solution Occurs in 3 steps • “Expand” the solvent • Overcome the IMF to make room for the solute. +∆H • “Expand” the solute • Separate the solute into ions, atoms or molecules. +∆H • Allow solvent and solute to COMBINE and form sol’n. -∆H ∆Hsol’n = ∆H1 + ∆H2 + ∆H3

  11. Example: NaCl(s)  Na+(aq) + Cl-(aq) ∆H1 = +21kJ/mol REQUIRED to overcome Hydrogen bonding in H2O (IMF) ∆H2= +786kJ/mol REQUIRED to separate the salt into ions ∆H3 = -783 kJ/mol IS RELEASED when ions and polar water molecules attract ∆Hsol’n= +24kJ/mol This is an endothermic change….. Generally unfavorable in the universe. So….why does NaCl dissolve so readily?

  12. Entropy

  13. Types of Solutions • Gas solutions • 2 or more gases or vapors dissolved • ex. AIR • Solid solutions a.k.a alloy • copper + zinc = brass • copper + tin = bronze • Amalgam • An alloy made with mercury

  14. Liquid solutions • liquid, solid or gas dissolved in liquid • 2 liquids that mix = miscible • 2 liquids that don’t mix = immiscible • (aq) water is the solvent • tincture • alcohol is the solvent

  15. water is the universal solvent because it dissolves almost everything

  16. Solubility Rules Like dissolves like • polardissolves polar • non-polardissolves non-polar • Similar IMF will dissolve in each other

  17. Oil and Water

  18. The End

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