Water and Aqueous Systems

1. Water and Aqueous Systems Chapter 15

2. Water and Its Properties • Water covers about three quarters of Earth’s surface. All life forms that are known to exist are made mostly of water. You will learn about the properties of water and what makes this unique substance essential to life on Earth.

3. 15.1 Water in the Liquid State • Water in the Liquid State • How can you account for the high surface tension and low vapor pressure of water?

4. 15.1 Water in the Liquid State • You could not live without water, nor could all the plants and animals on Earth.

5. 15.1 Water in the Liquid State • A water molecule is polar.

6. 15.1 Water in the Liquid State • Polar molecules are attracted to one another by dipole interactions. The negative end of one molecule attracts the positive end of another molecule.

7. 15.1 Water in the Liquid State • The intermolecular attraction among water molecules results in the formation of hydrogen bonds.

8. 15.1 Water in the Liquid State • Many unique and important properties of water—including its high surface tension and low vapor pressure—result from hydrogen bonding.

9. 15.1 Water in the Liquid State • Surface Tension • The inward force, or pull, that tends to minimize the surface area of a liquid is called surface tension. • All liquids have a surface tension, but water’s surface tension is higher than most.

10. 15.1 Water in the Liquid State • Surface tension makes it possible for this water strider to walk on water.

11. 15.1 Water in the Liquid State • A surfactant is any substance that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension.

12. 15.1 Water in the Liquid State • Vapor Pressure • Hydrogen bonding between water molecules also explains water’s unusually low vapor pressure. Because hydrogen bonds hold water molecules to one another, the tendency of these molecules to escape is low, and evaporation is slow.

13. 15.1 Water in the Solid State • Water in the Solid State • How would you describe the structure of ice?

14. 15.1 Water in the Solid State • As water begins to cool, it behaves initially like a typical liquid. It contracts slightly and its density gradually increases. When the temperature of the water falls below 4˚C, the density of water starts to decrease.

15. 15.1 Water in the Solid State

16. 15.1 Water in the Solid State • Hydrogen bonds hold the water molecules in place in the solid phase.

17. 15.1 Water in the Solid State • The structure of ice is a regular open framework of water molecules arranged like a honeycomb. • When ice melts, the framework collapses, and the water molecules pack closer together, making liquid water more dense than ice.

18. 15.2 Homogeneous Aqueous Systems • An ordinary dill pickle from the deli can be a source of light! Iron or copper electrodes are inserted into the ends of the pickle and connected to a source of alternating electric current. You will learn what kind of solution conducts electricity.

19. 15.2 Solvents and Solutes • Solvents and Solutes • What is the difference between a solvent and a solute?

20. 15.2 Solvents and Solutes • An aqueous solution is water that contains dissolved substances. • In a solution, the dissolving medium is the solvent. • In a solution, the dissolved particles are the solute.

21. 15.2 Solvents and Solutes • A solvent dissolves the solute. The solute becomes dispersed in the solvent. • Solvents and solutes may be gases, liquids, or solids. • Solute particles can be atoms, ions, or molecules.

22. 15.2 Solvents and Solutes • If you filter a solution through filter paper, both the solute and the solvent pass through the filter.

23. 15.2 The Solution Process • The Solution Process • What happens in the solution process?

24. 15.2 The Solution Process • As individual solute ions break away from the crystal, the negatively and positively charged ions become surrounded by solvent molecules, and the ionic crystal dissolves.

25. 15.2 The Solution Process • The process by which the positive and negative ions of an ionic solid become surrounded by solvent molecules is called solvation.

26. 15.2 The Solution Process • Solvation of an Ionic Solid

27. 15.2 The Solution Process • Polar solvents such as water dissolve ionic compounds and polar molecular compounds. • Nonpolar solvents such as gasoline dissolve nonpolar compounds. “Like dissolves like.”

28. 15.2 The Solution Process • Oil and water do not mix.

29. 15.2 Electrolytes and Nonelectrolytes • Electrolytes and Nonelectrolytes • Why are all ionic compounds electrolytes?

30. 15.2 Electrolytes and Nonelectrolytes • An electrolyte is a compound that conducts an electric current when it is in an aqueous solution or in the molten state. • All ionic compounds are electrolytes because they dissociate into ions.

31. 15.2 Electrolytes and Nonelectrolytes • The bright glow shows that sodium chloride is a strong electrolyte because nearly all the dissolved sodium chloride exists as separate Na+ and Cl– ions.

32. 15.2 Electrolytes and Nonelectrolytes • A weak electrolyte conducts electricity poorly because only a fraction of the solute in the solution exists as ions.

33. 15.2 Electrolytes and Nonelectrolytes • A compound that does not conduct an electric current in either aqueous solution or the molten state is called a nonelectrolyte.

34. 15.2 Hydrates • Hydrates • How do you write the formula for a hydrate?

35. 15.2 Hydrates • A compound that contains water of hydration is called a hydrate. • In writing the formula of a hydrate, use a dot to connect the formula of the compound and the number of water molecules per formula unit.

36. 15.2 Hydrates • A sample of blue CuSO4·5H2O is heated.

37. 15.2 Hydrates • Blue crystals of CuSO4·5H2O crumble to a white anhydrous powder that has the formula CuSO4.

38. 15.2 Hydrates

39. 15.2 Hydrates • To determine what percent of a hydrate is water, first determine the mass of the number of moles of water in one mole of hydrate. Then determine the total mass of the hydrate. The percent by mass of water can be calculated using this equation.

40. 15.1 Sample Problem 15.1 15.1

41. 15.3 Heterogeneous Aqueous Systems • In 1996, American astronaut Shannon Lucid shared a gelatin dessert with her Russian crewmates. Gelatin is a heterogeneous mixture called a colloid. You will learn more about the characteristics of colloids and a related mixture called a suspension.

42. 15.3 Suspensions • Suspensions • What is the difference between a suspension and a solution?

43. 15.3 Suspensions • A suspension is a mixture from which particles settle out upon standing. • A suspension differs from a solution because the particles of a suspension are much larger and do not stay suspended indefinitely.

44. 15.3 Suspensions • Suspensions are heterogenous because at least two substances can be clearly identified.

45. 15.3 Colloids • Colloids • What distinguishes a colloid from a suspension and a solution?

46. 15.3 Colloids • A colloid is a heterogeneous mixture containing particles that range in size from 1 nm to 1000 nm. The particles in a colloid are spread throughout the dispersion medium.

47. 15.3 Colloids • Colloids have particles smaller than those in suspensions and larger than those in solutions.

48. 15.3 Colloids

49. 15.3 Colloids • The Tyndall Effect • The scattering of visible light by colloidal particles is called the Tyndall effect.

50. 15.3 Colloids • Particles in colloids and suspensions reflect or scatter light in all directions. Solutions do not scatter light.