2. The Chemistry of Life Water & Mixtures copyright cmassengale

3. Mixtures A mixture is a material composed of two or more elements or compounds that are physically mixed but not chemically combined.

4. Solutions & Suspensions Water is usually part of a mixture.Water is usually part of a mixture. Because so many things dissolve in water, it is called the Universal SolventBecause so many things dissolve in water, it is called the Universal Solvent There are 3 types of mixtures:There are 3 types of mixtures: –Solutions –Suspensions –Colloids copyright cmassengale

5. Solutions A solution is a homogenous mixture in which 1 or more substances are uniformly distributed in another substance

6. Copyright Pearson Prentice Hall Na + Cl - Water When a crystal of table salt is placed in warm water, sodium and chloride ions are attracted to the polar water molecules. Na+ ions will be attracted to WHAT END of the water molecule?

7. Properties of Solutions Ionic compounds disperse as ions in water (+ions & -ions spread out among polar water molecules)Ionic compounds disperse as ions in water (+ions & -ions spread out among polar water molecules) SOLUTESOLUTE –Substance that is being dissolved –Substance dissolved in the solution –Particles may be ions, atoms, or molecules SOLVENTSOLVENT –Dissolving Substance for the solute –Substance in which the solute is dissolved copyright cmassengale Remember that water is the Universal Solvent! (Many things dissolve in it)

8. Aqueous solution (water = solvent) are universally important to living things and are the most common type of solution in nature Tinctures are solution in which the solvent is alcohol is a tincture Ex: iodine tincture

9. Solutions Because solutions are so important for Biology, we will learn a little more about it in detail over the next few slides copyright cmassengale

10. Ions and dissociation Ions are atoms with a positive or negative charge

11. Electrolytes Solutions that conduct electricity are electrolytes (sodium chloride and silver nitrate)

12. Non-electrolytes Non-electrolytes form solutions that do not conduct electricity (sugar, alcohol, benzene)

13. Review Questions What is a solution? What are the two parts of a solution? What are some properties of a solution? What’s the difference between an aqueous solution and a tincture?

14. Effervescence (fizz) The escape of a gas from a liquid is effervescence (example: soda and alka seltzer)

15. Solubility The measure of how much solute can be dissolved in a solvent is solubility

16. What affects solubility? The three main factors that affect solubility are temperature, type and the amount of the solvent

17. Ways to increase dissolving rate In order to increase the rate in which a solution dissolves one could heat the solution, stir it, or crush the solute particles

18. Concentration Solutions can be composed of varying proportions of a given solute in a given solvent --- vary in concentration (measurement of the amount of solute) Concentration of a solution is the amount of solute that is dissolved in a solvent

19. Concentrated vs. dilute A solution with a lot of solute dissolved is concentrated A solution with a little solute dissolved is dilute

20. Types of solutions A saturated solution contains all the solute it can possibly hold An unsaturated solution contains less solute that is possible

21. Supersaturated solution A supersaturated solution can be made to hold more solute than is normal

22. Review Questions Compare a saturated, unsaturated, and a supersaturated solution What is solubility and what are the three factors that affect it? What are three ways to increase the rate in which a solute dissolves? copyright cmassengale

23. Freezing point depression Lowering the freezing point of a solution as a result of the dissolved solute (freezing point depression) Ex: antifreeze in water

24. Boiling point elevation Raising the boiling point of a substance by adding solute (salt in water)

25. Polar vs. non-polar A polar molecule has oppositely charged ends (+ and -) Non-polar molecules have the same charges on its ends (even electrical distribution)

26. Rule for dissolving solutes in a solvent Like solutes dissolve in like solvents (polar in polar, non-polar in non- polar)

27. Water Water is the universal solvent A substance that cannot dissolve in water is usually called insoluble

28. Hard water vs. soft water Hard water contains dissolved metal ions Soft water does not contain dissolved metal ions

29. Review Questions What is the difference between polar and non-polar molecules? What is the general rule for dissolving solutes? What is the difference between hard and soft water? How does a solute affect the freezing point and the boiling point?

30. 29 Water-soluble protein

31. Suspensions Some materials do not dissolve when placed in water but separate into pieces so small that they do not settle out easily.

32. Suspensions A suspension is a heterogeneous mixture in which the solute particles are large enough to be seen (solute is suspended) Substances that don’t dissolve but separate into tiny pieces.Substances that don’t dissolve but separate into tiny pieces. Water keeps the pieces suspended so they don’t settle out.Water keeps the pieces suspended so they don’t settle out. Blood & Cytoplasm are suspensionsBlood & Cytoplasm are suspensions copyright cmassengale

33. Colloid A colloid is a homogeneous mixture that is not a true solution (does not separate, solute remains suspended)

34. Interactions with Non-polar Molecules Water Organizes nonpolar molecules. Nonpolar molecules are hydrophobic (repelled by H 2 O) Repulsion forces these molecules into particular arrangements. Example is the lipid bilayer found in cellular membranes.