1. 1 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 7 Lecture Outline Prepared by Jennifer N. Robertson-Honecker West Virginia University

2. 2 Solutions Introduction Thus far we have focused on pure substances— elements, covalent compounds, and ionic compounds. Most matter we come into contact with is a mixture of two or more pure substances. A heterogeneous mixture does not have a uniform composition throughout the sample. A homogeneous mixture has a uniform composition throughout the sample.

3. 3 Solutions Introduction Solutions consist of two parts: The solute is the substance present in a lesser amount. The solvent is the substance present in a larger amount. An aqueous solution has water as the solvent. A solution is a homogeneous mixture that contains small particles. Liquid solutions are transparent. A colloid is a homogeneous mixture with larger particles, often having an opaque appearance.

4. 4 Solutions Introduction Three different types of solutions: a solution of gases (O 2, CO 2, and N 2 ) an aqueous solution of NaCl (a solid in a liquid) Hg(l) dissolved in Ag(s) (a liquid in a solid)

5. 5 Solutions Introduction A substance that conducts an electric current in water is called an electrolyte. A substance that does not conduct an electric current in water is called a nonelectrolyte. NaCl(aq) dissociates into Na + (aq) and Cl − (aq) H 2 O 2 does not dissociate

6. 6 Solubility General Features Solubility is the amount of solute that dissolves in a given amount of solvent. It is usually reported in grams of solute per 100 mL of solution (g/100 mL). A saturated solution contains the maximum number of grams of solute that can dissolve. An unsaturated solution contains less than the maximum number of grams of solute that can dissolve.

7. 7 Solubility Basic Principles Solubility can be summed up as “like dissolves like.” Most ionic and polar covalent compounds are soluble in water, a polar solvent.

8. 8 Solubility Basic Principles Small neutral molecules that can hydrogen bond to water are water soluble. Ethanol can hydrogen bond to water.

9. 9 Solubility Basic Principles Nonpolar compounds are soluble in nonpolar solvents (i.e., like dissolves like). Octane (C 8 H 18 ) dissolves in CCl 4 because both are nonpolar liquids that exhibit only London dispersion forces. octaneCCl 4 octane + CCl 4

10. 10 Solubility Basic Principles When solvation releases more energy than that required to separate particles, the overall process is exothermic (heat is released). When the separation of particles requires more energy than is released during solvation, the process is endothermic (heat is absorbed).

11. 11 Solubility Temperature Effects For most ionic and molecular solids, solubility generally increases as temperature increases. By dissolving a solid in a solvent at high temperature and allowing it to cool slowly, a supersaturated solution can be made. A supersaturated solution contains more than the predicted maximum amount of solute at a given temperature. In contrast, the solubility of a gas decreases with increasing temperature.

12. 12 Solubility Pressure Effects Henry’s law: The solubility of a gas in a liquid is proportional to the partial pressure of the gas above the liquid. The higher the pressure, the higher the solubility of a gas in a solvent. closed can of soda higher CO 2 pressure higher CO 2 solubility open can of soda lower CO 2 pressure lower CO 2 solubility

13. 13 Concentration Units Weight/Volume Percent Concentration The concentration of a solution tells how much solute is dissolved in a given amount of solution. Weight/volume percent concentration, (w/v)%, is the number of grams of solute dissolved in 100 mL of solution. Weight/volume percent concentration Weight/volume percent concentration (w/v)% = volume of solution (mL) x100% mass of solute (g)

14. 14 Concentration Units Weight/Volume Percent Concentration For example, vinegar contains 5 g of acetic acid in 100 mL of solution, so the (w/v)% concentration is 5 g acetic acid 100 mL vinegar solution x 100% = 5% (w/v)

15. 15 Concentration Units Volume/Volume Percent Concentration Volume/volume percent concentration Volume/volume percent concentration (v/v)% = volume of solution (mL) x 100% For example, if a bottle of rubbing alcohol contains 70 mL of 2-propanol in 100 mL of solution, then the (v/v)% concentration is 70 mL 2-propanol 100 mL rubbing alcohol x 100% = 70% (v/v) volume of solute (mL)

16. 16 Concentration Units Using a Percent Concentration as a Conversion Factor Sample Problem 7.4 A saline solution used in intravenous drips contains 0.92% (w/v) NaCl in water. How many grams of NaCl are contained in 250 mL of this solution? Step [1] Identify the known quantities and the desired quantity. 0.92% (w/v) NaCl solution 250 mL known quantities ? g NaCl desired quantity

17. 17 Concentration Units Using a Percent Concentration as a Conversion Factor Step [2] Write out the conversion factors. 100 mL solution 0.92 g NaCl or 0.92 g NaCl 100 mL solution Choose this one to cancel mL. Step [3] Solve the problem. 250 mLx 0.92 g NaCl 100 mL solution =2.3 g NaCl Answer Milliliters cancel.

18. 18 Concentration Units Parts Per Million When a solution contains a very small concentration of solute, it is often expressed in parts per million. Parts per million mass of solute (g) mass of solution (g) x 10 6 or volume of solute (mL) volume of solution (mL) x 10 6 ppm =

19. 19 Concentration Units Molarity Molarity is the number of moles of solute per liter of solution, abbreviated as M. moles of solute (mol) liter of solution (L) moles of solute (mol) liter of solution (L) Molarity = M =

20. 20 Concentration Units Molarity HOW TO Calculate Molarity from a Given Number of Grams of Solute Example Calculate the molarity of a solution made from 20.0 g of NaOH in 250 mL of solution. Step [1] Identify the known quantities and the desired quantity. 20.0 g NaOH 250 mL solution known quantities ? M (mol/L) desired quantity

21. 21 Concentration Units Molarity HOW TO Calculate Molarity from a Given Number of Grams of Solute Step [2] Convert the number of grams of solute to the number of moles. Convert the volume to liters if necessary. Use the molar mass to convert grams of NaOH to moles of NaOH (molar mass 40.0 g/mol). 20.0 g NaOHx 1 mol 40.0 g NaOH =0.500 mol NaOH Grams cancel.

22. 22 Concentration Units Molarity HOW TO Calculate Molarity from a Given Number of Grams of Solute Convert milliliters of solution to liters of solution using a mL–L conversion factor. 250 mL solutionx 1 L 1000 mL =0.25 L solution Milliliters cancel.

23. 23 Concentration Units Molarity HOW TO Calculate Molarity from a Given Number of Grams of Solute Step [3] Divide the number of moles of solute by the number of liters of solution to obtain the molarity. moles of solute (mol) 0.500 mol NaOH V (L) 0.25 L solution =2.0 M Answer =M =

24. 24 Concentration Units Molarity Molarity is a conversion factor that relates the number of moles of solute to the volume of solution it occupies. To calculate the moles of solute, rearrange the equation for molarity: moles of solute (mol) = M x V(L) To calculate the volume of the solution, rearrange the equation for molarity: moles of solute (mol) M moles of solute (mol) M V(L) =

25. 25 Concentration Units Molarity Sample Problem 7.8 What volume in milliliters of a 0.30 M solution of glucose contains 0.025 mol of glucose? Step [1] Identify the known quantities and the desired quantity. 0.30 M 0.025 mol glucose known quantities ? V(L) desired quantity

26. 26 Concentration Units Molarity Step [2] Divide the number of moles by molarity to obtain the volume in liters. moles of solute (mol) M 0.025 mol glucose 0.30 mol/L = 0.083 L solution Answer V(L) =

27. 27 Concentration Units Molarity Step [3] Use a mL–L conversion factor to convert liters to milliliters. 0.083 L solution x 1000 mL 1 L =83 mL glucose solution Liters cancel.Answer

28. 28 Concentration Units Molarity Since the number of grams and moles of a substance is related by the molar mass, we can convert a given volume of solution to the number of grams of solute given its molarity.

29. 29 Dilution Dilution is the addition of solvent to decrease the concentration of solute. The solution volume changes, but the amount of solute is constant. moles of solute (mol) = molarity (M) x volume (V) initial valuesfinal values M 1 V 1 = M 2 V 2

30. 30 Dilution Sample Problem 7.11 How many milliliters of a 4.0% (w/v) solution must be used to prepare 250 mL of a 0.080% (w/v) solution? Step [1] Identify the known quantities and the desired quantity. C 1 V 1 = C 2 V 2 initial values final values ? V(L) desired quantity C 1 = 4.0% (w/v) C 2 = 0.080% (w/v) V 2 = 250 mL known quantities

31. 31 Dilution Step [2] Write the equation and rearrange it to isolate the desired quantity, V 1, on one side. C 1 V 1 = C 2 V 2 Step [3] Solve the problem. V 1 = (0.080%)(250 mL) 4.0% =5.0 mL dopamine solution Answer V 1 = C 2 V 2 C 1 Solve for V 1 by dividing both sides by C 1.

32. 32 Osmosis The membrane that surrounds living cells is a semipermeable membrane. Semipermeable membranes allow water and small molecules to pass across, but ions and large molecules cannot. Osmosis is the passage of water and small molecules across a semipermeable membrane from a solution of low solute concentration to a solution of higher solute concentration.

33. 33 Osmotic pressure is the pressure that prevents the flow of additional solvent into a solution on one side of a semipermeable membrane. Osmosis

34. 34 Focus on the Human Body Osmosis and Biological Membranes Two solutions with the same osmotic pressure are said to be isotonic. Solutions isotonic to the body: a 0.92% (w/v) NaCl solution a 5.0% (w/v) glucose solution isotonic solution

35. 35 A hypotonic solution has a lower osmotic pressure than body fluids. The concentration of particles outside the cell is lower than the concentration of particles inside the cell. Water diffuses into the cell, so the cell swells and eventually bursts. For red blood cells, this swelling and rupture is called hemolysis. hypotonic solution Focus on the Human Body Osmosis and Biological Membranes

36. 36 A hypertonic solution has a higher osmotic pressure than body fluids. The concentration of particles outside the cell is higher than the concentration of particles inside the cell. Water diffuses out of cell, so the cell shrinks. This process is called crenation. hypertonic solution Focus on the Human Body Osmosis and Biological Membranes

37. 37 Focus on Health Medicine Dialysis In the human body, blood is filtered through the kidneys by the process of dialysis. In dialysis, water, small molecules, and ions can pass through the semipermeable (dialyzing) membrane; only large biological molecules like proteins and starch molecules cannot. This allows waste products like urea to be removed from the bloodstream and eliminated in the urine.

38. Focus on Health Medicine Dialysis When a person’s kidneys are incapable of removing waste products from the blood, hemodialysis is used.