1. Chapter 7: Solutions and Colloids CHE 140

2. CHAPTER OUTLINE 7.1 Physical States of Solutions 7.2 Solubility 7.3 The Solution Process 7.4 Solution Concentrations 7.5 Solution Preparation 7.6 Solution Stoichiometry 7.7 Solution Properties 7.8 Colloids 7.9 Dialysis

3. Solution Terminology solution - a homogeneous mixture of two or more substances, the composition of which may vary within definite limits. solute - the substance dissolved in a solution. solvent - the dissolving medium in a solution. A solution is a solute dissolved in a solvent. In the example of the sugar-water mixture, sugar-water is the solution, sugar is the solute, and water is the solvent.

4. Suspension Terminology If clay is mixed with water, it will not dissolve. Clay particles will be suspended in the water. This is called a suspension. suspension - a heterogeneous mixture Colloids are large suspended particles. They may be homogeneous, but they are not true solutions because the large particles are not dissolved. Examples : mayonnaise, ketchup, mustard

5. Electrolytes electrolyte - a substance whose water solution conducts electricity Examples : acids, bases, salts nonelectrolytes - a substance whose water solution does not conduct electricity

6. Concentrations of Solutions The concentration of a solution depends on the relative amounts of solute and solvent present in a solution. The terms concentrate and dilute are qualitative. This means they only give "what" is present in a solution and not "how much" is present.

7. Percent by Mass Percent by mass of a solute in solution is the number of grams of solute dissolved in 100g of solution. mass of solute % by mass = --------------------------------- x100% mass solute + solvent Find the percent by mass of a solution made by dissolving 10g of sodium hydroxide in 90g of water.

8. Molarity Molarity is the number of moles of solute in one liter of solution. moles of solute Molarity = ----------------------------- liters of solution Find the molarity of a solution made by dissolving 20g of sodium hydroxide in 500mL of solution. How many moles of HCl are present in 0.8 L of 0.5 M HCl solution?

9. Molality molality (m) - an expression of moles of solute in a kilogram of solvent moles of solute molality = ------------------------------------- mass of solvent (kg) A solution consists of 17.1g of sucrose (C 12 H 22 O 11 ) dissolved in 125g of water. Find the molal concentration of this solution. Determine the mass of copper(II) sulfate needed to prepare a 0.25-m solution using 250mL of water. Assignment: Find m for 20g NaOH in 250ml solv

10. Types of Solutions air coke cake rain alcohol and water wet sponge smoke saltwater brass gas in gas gas in liquid gas in solid liquid in gas liquid in liquid liquid in solid solid in gas solid in liquid solid in solid

11. Acids and Bases Acids, bases, and salts are electrolytes, substances whose water solutions conduct electricity. They are uniquely related in that acids react with bases to produce salts and water. The word salt is a derivative of the Latin word sal which means vital compound. Roman soldiers were paid with salt, sal-ary. Salt has long been used to flavor and preserve food and as medicine.

12. The Nature of Acids Acids are present in many foods, especially fruit. All foods which taste sour have some type of acid in them. Some organic acids include; ACID FOOD citric acid lemons malic acid apples lactic acid milk butyric acid rancid butter acetic acid vinegar

13. Properties of Acids 1. Acids donate protons in the presence of bases. HCl monoprotic H 2 SO 4 diprotic H + Cl - + Na + OH -  Na + Cl - + H + OH - 2. Acids contain ionizable hydrogen covalently bonded to a nonmetallic element or polyatomic species. nonmetal......................HCl polyatomic species...H 3 PO 4

14. Properties of Acids 3. Acids taste sour. NEVER USE THE TASTE TEST!!! 4. Acids affect indicators. litmus turns red phenolphthalein remains clear methyl orange turns red 5. Acids neutralize hydroxides. HCl + NaOH  NaCl + H 2 O

15. Properties of Acids 6. Acids react with many metals. Zn(s) + H 2 SO 4 (aq)  ZnSO 4 (aq) + H 2 (g) 7. Acids react with oxides of metals. CuO + H 2 SO 4  CuSO 4 + H 2 O 8. Acids react with carbonates. CaCO 3 + 2HCl  CaCl 2 + H 2 O + CO 2

16. The Nature of Bases Bases are often referred to as hydroxides. The hydroxide ion, OH -, is responsible for most basic or alkaline properties. The basicity of a substance is also referred to as the alkalinity. Name some common household bases. 1. lye4. soap 2. lime5. antacids 3. laxatives6. eggs base - a proton acceptor

17. Properties of Bases 1. Hydroxides of active metals supply hydroxide ions, OH -. Na + OH -  Na + (aq) + OH - (aq) 2. Soluble hydroxides have a bitter taste. NEVER USE THE TASTE TEST!! 3. Solutions of hydroxides feel slippery. 4. Soluble hydroxides affect indicators. red litmus paper turns blue phenolphthalein turns red methyl orange turns yellow

18. 5. Hydroxides neutralize acids. NaOH + HCl  NaCl + H 2 O 6. Hydroxides react with oxides of nonmetals. CO 2 + 2NaOH  Na 2 CO 3 + H 2 O 7. Certain hydroxides are amphoteric; i.e., they take on acid properties in the presence of stronger bases and take on basic properties in the presence of strong acids. Example: Write the formula for aluminum hydroxide which shows acidic properties.

19. Salts A salt is a compound composed of the positive ion of an aqueous base and the negative ion of an aqueous acid. We usually think of table salt, NaCl, when we hear the word salt. There are actually many kinds of salts. Our bodies obtain minerals in the form of salts. For example, with your knowledge of the active metal sodium, what would happen if you tried to eat pure sodium metal? Eating NaCl is much safer!

20. Chemical Equivalents Chemical equivalents are the quantities of substances that have the same combining capacity in chemical reactions. Chemical equivalents are calculated by dividing the molar mass by the total positive charge on the first element in the formula of the compound.

21. Calculating Chemical Equivalents molar mass 1 equiv = ------------------------------ total positive charge Determine the chemical equivalents of each of the following. a. HCl ____________________ b. NaOH __________________ c. H 2 SO 4 __________________

22. Normality Normality, (N), is an expression of gram equivalents of solute per liter of solution. Before calculating normality, the chemical equivalent must be calculated. mass solute 1 equiv 1000 mL N= -------------------- X ---------------- X ------------ vol. soln. eq mass L

23. Sample Problem Find the normality of 300mL of a solution containing 55 grams of calcium chloride.

24. pH The pH of a solution is a numerical representation of the degree of hydronium ion concentration. The term (from French pouvoir hydrogène, "hydrogen power") is defined as the negative logarithm of the concentration of H + ions (protons). pH - the common logarithm of the reciprocal of the hydronium ion concentration 1 pH = log 10 ------------ [H 3 O + ]

25. pH Scale The pH scale is a numerical scale which indicates the acidity or basicity of a substance. A neutral substance, one which has an equal concentration of hydronium and hydroxide ions has a pH of 7 which is half way between 0 and 14. acid base 0---------------------- 7 --------------------- 14

26. Approximate pH of Some Common Materials MATERIALpH gastric juice2.0 lemons2.3 vinegar2.8 soft drinks3.0 apples3.1 tomatoes4.2 bananas4.6 bread5.5 rainwater6.2 milk6.5 pure water7.0 eggs7.8 seawater8.5 milk of magnesia10.5

27. pH of Acids The concentrations of acids is usually given in molarity, M. Since molarity is an expression of Moles / L, the hydronium ion concentration can readily be determined. Find the pH of a 0.001-M HCl solution.

28. pH of Bases 10 -14 [H 3 O + ] = ------------ [OH - ] Find the pH of a 0.01 - M NaOH solution. Find the pH of a 0.001 - M Ca(OH) 2 solution

29. Assignment Find the pH of the following. 1. 0.01- M H 2 SO 4 2. 0.0001- M H 2 S 3. 0.1 - M HCl 4. 0.002 –M NaOH

30. Acid-Base Titration Titration is the progressive addition of an acid to a base to achieve neutralization so the concentration of an unknown solution may be found. The point at which neutralization occurs is known as the end point. Indicators are used for determination of this point. The previously discussed indicators will be used in our titrations.

31. Titration Calculations V A N A = V B N B V A = volume of acid used in mL N A = normality of acid used in N V B = volume of base used in mL N B = normality of base used in N

32. Sample Problem A student performed a titration and determined 20mL of a 1.5-N HCl solution was needed to neutralize 35mL of a NaOH solution of unknown concentration. Determine the normality of the unknown solution.