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Chapter 16: MIXTURES

. Chapter 16: MIXTURES. This lecture will help you understand:. Most Materials are Mixtures The Chemist’s Classification of Matter Solutions Solubility Soaps and Detergents Softening Hard Water Purifying the Water We Drink Wastewater Treatment. Most Materials are Mixtures.

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Chapter 16: MIXTURES

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  1. . Chapter 16: MIXTURES

  2. This lecture will help you understand: • Most Materials are Mixtures • The Chemist’s Classification of Matter • Solutions • Solubility • Soaps and Detergents • Softening Hard Water • Purifying the Water We Drink • Wastewater Treatment

  3. Most Materials are Mixtures • Pure substance A material consisting of only one type of element or compound.

  4. Most Materials are Mixtures • Pure substance A material consisting of only one type of element or compound. • Mixture A collection of two or more pure substances.

  5. Most Materials are Mixtures • Pure substance A material consisting of only one type of element or compound. • Mixture A collection of two or more pure substances. —can be separated by physical means

  6. Most Materials are Mixtures

  7. The Chemist’s Classification of Matter

  8. The Chemist’s Classification of Matter • Pure materials consist of a single element or compound.

  9. The Chemist’s Classification of Matter • Pure materials consist of a single element or compound. • Impure materials consist of two or more elements or compounds.

  10. The Chemist’s Classification of Matter • Pure materials consist of a single element or compound. • Impure materials consist of two or more elements or compounds. • Mixtures may be heterogeneous or homogeneous.

  11. The Chemist’s Classification of Matter • In heterogeneous mixtures, the different components can be seen as individual substances.

  12. The Chemist’s Classification of Matter • In heterogeneous mixtures, the different components can be seen as individual substances. • In homogenous mixtures, the composition is the same throughout.

  13. The Chemist’s Classification of Matter

  14. The Chemist’s Classification of Matter • Homogeneous mixtures

  15. The Chemist’s Classification of Matter • Homogeneous mixtures • Solution: all components in the same phase.

  16. The Chemist’s Classification of Matter • Homogeneous mixtures • Solution: all components in the same phase. • Suspension: different components in different phases.

  17. The Chemist’s Classification of Matter CHECK YOUR NEIGHBOR Is the air in your house a homogeneous or a heterogeneous mixture? A. Homogeneous, because it is mixed very well. B. Heterogeneous, because of the dust particles it contains. C. Homogeneous, because it is all at the same temperature. D. Heterogeneous, because it consists of different types of molecules.

  18. The Chemist’s Classification of Matter CHECK YOUR ANSWER Is the air in your house a homogeneous or a heterogeneous mixture? A. Homogeneous, because it is mixed very well. B. Heterogeneous, because of the dust particles it contains. C. Homogeneous, because it is all at the same temperature. D. Heterogeneous, because it consists of different types of molecules.

  19. Solutions • Solution: A homogenous mixture consisting of ions or molecules • Solvent: The major component of a solution.

  20. Solutions • Solution: A homogenous mixture consisting of ions or molecules • Solvent: The major component of a solution. • Solute: The minor components of a solution.

  21. Solutions • Solution: A homogenous mixture consisting of ions or molecules • Solvent: The major component of a solution. • Solute: The minor components of a solution. • Saturated: Said of a solution in which no more solute will dissolve.

  22. Solutions • Concentration: A measure of the amount of solute dissolved in solution.

  23. Solutions • Concentration: A measure of the amount of solute dissolved in solution. Solute Concentration = Solution

  24. Solutions • Concentration: A measure of the amount of solute dissolved in solution. Solute Concentration = Solution “concentrated”

  25. Solutions • Concentration: A measure of the amount of solute dissolved in solution. Solute Concentration = Solution

  26. Solutions • Concentration: A measure of the amount of solute dissolved in solution. Solute Concentration = Solution “dilute”

  27. Solutions • Concentration: A measure of the amount of solute dissolved in solution. • Mole: A super-large number, 6.02  1023, used to measure numbers of atoms or molecules, a.k.a. Avogadro’s number.

  28. Solutions • Concentration: A measure of the amount of solute dissolved in solution. • Mole: A super-large number, 6.02  1023, used to measure numbers of atoms or molecules, a.k.a. Avogadro’s number. The formula mass of a substance expressed in grams contains one mole.

  29. Solutions • Concentration: A measure of the amount of solute dissolved in solution. • Mole: A super-large number, 6.02  1023, used to measure numbers of atoms or molecules, a.k.a. Avogadro’s number. Substance Formula Mass The formula mass of a substance expressed in grams contains one mole. Carbon, C 12 Oxygen, O2 32 Carbon dioxide, CO2 44 Sucrose, C12H22O11 342

  30. Solutions Sucrose, C12H22O11 = 342 g/mole

  31. Solutions CHECK YOUR NEIGHBOR Water, H2O, has a formula mass of 18. How many moles of water are there in 18 grams of water? A. 0.5 moles • 1 mole • 9 moles • 18 moles

  32. Solutions CHECK YOUR ANSWER Water, H2O, has a formula mass of 18. How many moles of water are there in 18 grams of water? A. 0.5 moles • 1 mole • 9 moles • 18 moles

  33. Solutions CHECK YOUR NEIGHBOR How many grams of water, H2O, are there in 2 moles of water? A. 1 gram • 9 grams • 18 grams • 36 grams

  34. Solutions CHECK YOUR ANSWER How many grams of water, H2O, are there in 2 moles of water? A. 1 gram • 9 grams • 18 grams • 36 grams

  35. Solutions • Molarity: A unit of concentration expressed in moles solute per liter of solution.

  36. Solutions • Molarity: A unit of concentration expressed in moles solute per liter of solution. Moles of Solute Molarity = Liters of Solution

  37. Solutions • Molarity: A unit of concentration expressed in moles solute per liter of solution. • ppm: A unit of concentration expressed in milligrams solute in liters of solution. • Molarity: A unit of concentration expressed in moles solute per liter of solution. • ppm: A unit of concentration expressed in milligrams solute in liters of solution.

  38. Solutions • Molarity: A unit of concentration expressed in moles solute per liter of solution. • ppm: A unit of concentration expressed in milligrams solute in liters of solution. • Molarity: A unit of concentration expressed in moles solute per liter of solution. • ppm: A unit of concentration expressed in milligrams solute in liters of solution. 1 part solute 1 milligram solute 1 ppm = = 1,000,000 parts solution 1 liter solution

  39. Solubility • Solubility: The ability of a solute to dissolve in a solvent.

  40. Solubility • Solubility: The ability of a solute to dissolve in a solvent. • Soluble: Said of a solute that has appreciable solubility.

  41. Solubility • Precipitate: Solute that comes out of solution.

  42. Solubility CHECK YOUR NEIGHBOR The amount of oxygen, O2, dissolved in the waters of the arctic ocean is greater, about equal to, or less than the amount of oxygen dissolved in warm tropical waters? A. Greater than • About equal • Less than • It depends

  43. Solubility CHECK YOUR ANSWER The amount of oxygen, O2, dissolved in the waters of the Arctic Ocean is greater, about equal to, or less than the amount of oxygen dissolved in warm tropical waters? A. Greater than • About equal • Less than • It depends Explanation: The solubility of oxygen in water decreases with increasing temperature. As a consequence, cold polar oceans tend to be more fertile than warmer tropical waters.

  44. Chapter 12 Review CHECK YOUR NEIGHBOR By mass, water is 88.88 percent oxygen. So why can’t we breathe water?

  45. Chapter 12 Review CHECK YOUR NEIGHBOR By mass, water is 88.88 percent oxygen. So why can’t we breathe water? Hint: What is the elemental formula for the oxygen we breathe and the chemical formula for water?

  46. Soaps and Detergents • Soaps and detergents have both polar and nonpolar properties.

  47. Soaps and Detergents • Soaps and detergents have both polar and nonpolar properties. • Nonpolar part attracts to the “grime”.

  48. Soaps and Detergents • Soaps and detergents have both polar and nonpolar parts. • Nonpolar part attracts to the “grime”. • Polar part attracts to water.

  49. Soaps and Detergents

  50. Soap and Detergents CHECK YOUR NEIGHBOR Soap attracts “grime” by which type of molecular interaction? A. Dipole–dipole. B. Induced dipole–induced dipole. C. Hydrogen bonding. D. Dipole–induced dipole.

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