The Chemistry of Acids and Bases

1. The Chemistry of Acids and Bases

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3. Acids and Bases: Molar SolutionsAt the conclusion of our time together, you should be able to: Define molarity Make a solution with a given molarity Determine the molarity of a given solution

4. Some Definitions A solution is a homogeneous mixture of 2 or more substances in a single phase. The larger constituent is usually regarded as the SOLVENT and the others as SOLUTES.

5. Some Definitions The units are moles per Liter. Specifically, it’s moles of solute per Liter of solution. Abbreviated as mol/L or M. The word Molarity.

6. Some Definitions Moles measureamount of solute usually in grams Molaritymeasuresmoles of solute per Liter of solution.

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8. moles solute ( M ) Molarity = liters of solution Concentration of Solute The amount of solute in a solution is given by its concentration.

9. moles solute ( M ) Molarity = liters of solution Concentration of Solute Therefore: x both sides by Liters = MV = moles = grams/molar mass

10. x g NaCl 58.44 g NaCl PROBLEM: Using grams/molar mass = MV.Handout #1 = 1 M x 1 L = 58.44 g NaCl

11. x g NaNO3 85.00 g NaNO3 PROBLEM: Using grams/molar mass = MV.Handout #2 = 0.5 M x 1 L = 42.5 g NaNO3

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13. Acids and Bases: Molar SolutionsLet’s see if you can: Define molarity Make a solution with a given molarity

14. x g H2SO4 98.09 g H2SO4 PROBLEM: Using grams/molar mass = MV.Backside #1 = 2.50 M x 1 L = 245 g H2SO4

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16. Acids and Bases: Molar SolutionsAt the conclusion of our time together, you should be able to: Define molarity Make a solution with a given molarity

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18. x g Ca(OH)2 74.10 g Ca(OH)2 PROBLEM: Using grams/molar mass = MV.Backside #4 = 0.100 M x 0.100 L = 0.741 g Ca(OH)2

19. Preparing Solutions • Determine the mass of solute. • Place in the appropriate volumetric flask. • Add deionized water and swirl until solute is dissolved. • Add water to the mark on the neck of the flask. • Stopper and mix thoroughly.

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21. Stoichiometry: Molar SolutionsLet’s see if you can: Define molarity Make a solution with a given molarity

22. moles solute ( M ) Molarity = liters of solution Concentration of Solute Therefore: MV = moles = grams/molar mass

23. Acids and Bases: Molar SolutionsAt the conclusion of our time together, you should be able to: Define molarity Make a solution with a given molarity Determine the molarity of a given solution

24. moles solute ( M ) Molarity = liters of solution Concentration of Solute Therefore: MV = moles = grams/molar mass Now let’s use this formula to solve another type of problem:

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26. x 1 mol AgNO3 169.88 g AgNO3 PROBLEM: Mr. T accidentally dropped 15.14 g of silver (I) nitrate into 100.0 mL of deionized water. Rather than throw the solution away, help him by determining its molar concentration so that he can label it and still use it.. 15.14 g AgNO3 = M x 0.100 L = 0.8912 M AgNO3

27. x 1 mol KI 166.00 g KI PROBLEM: Molarity Problems #2 249 g KI = M x 0.5 L = 3 M KI

28. How Would You Make this 3M Solution?? • Measure 249 g of KI • Place in a 0.500 L volumetric flask. • Add deionized water and swirl until solute is dissolved. • Add water to the mark on the neck of the flask. • Stopper and mix thoroughly.

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30. Acids and Bases: Molar SolutionsLet’s see if you can: Define molarity Make a solution with a given molarity Determine the molarity of a given solution

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32. Exit Quiz #1 • 1. Calculate the molarity if 0.75 mol of NaCl in placed in 300.0 mL of water. • 2. Calculate the number of moles and grams of HCl if there is 12.2 mL of 2.45 M HCl solution.

33. 0.75 mol NaCl X mol HCl x 36.46 g HCl 1 mol HCl = X M x 0.3000 L • 1. Calculate the molarity if 0.75 mol of NaCl in placed in 300.0 mL of water. • 2. Calculate the number of moles and grams of HCl if there is 12.2 mL of 2.45 M HCl solution. = 2.5 M NaCl = 2.45 M x 0.0122 L = 0.0299 mol HCl 0.0299 mol HCl = 1.09 g HCl

35. Entrance Quiz #2 • 1. Calculate the molarity if 0.50 mol of KBr in placed in 750 mL of water. • 2. Calculate the number of moles and molarity of HCl if there is 12.2 mL with 2.45 g of HCl in solution.

36. 0.50 mol KBr 0.0672 mol HCl x 1 mol HCl 36.46 g HCl = X M x 0.75 L • 1. Calculate the molarity if 0.50 mol of KBr in placed in 750 mL of water. • 2. Calculate the number of moles and molarity of HCl if there is 12.2 mL with 2.45 g of HCl. = 0.67 M KBr 2.45 g HCl = 0.0672 mol HCl = X M x 0.0122 L = 5.51 M HCl

37. Stoichiometry: Molar SolutionsAt the conclusion of our time together, you should be able to: Define molarity Determine the molarity of a given solution Make a solution with a given molarity Dilute a given solution to a new molarity

38. moles solute ( M ) Molarity = liters of solution If the Amount (moles) of Solute #1 = #2 M1V1 = moles and M2V2 = moles Therefore if moles of solute are constant: M1V1 = M2V2 And Using the Formula:

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40. PROBLEM #1: Using M1V1 = M2V2 0.150 M NaOH x 0.125 L = M x 0.150 L = 0.125 M NaOH

41. PROBLEM #5: Using M1V1 = M2V2 2.40 M KCl x 0.500 L = 1.00 M KCl x X L = 1.20 L Therefore: 0.700 L needs to be added

42. Stoichiometry: Molar SolutionsLet’s see if you can: Define molarity Determine the molarity of a given solution Make a solution with a given molarity Dilute a given solution to a new molarity

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44. How much water do I need to add to 250 mL of 3.0 M HCl to dilute it to 1.0 M HCl? 3.0 M HCl x 0.250 L = 1.0 M HCl x L = 0.75 L Total, therefore 0.50 L

45. Name ________Class Period _____ Clicker Number Name ________Class Period _____ Clicker Number "Making Molar Solutions A1" (10 points) Make 50.00 mL of a 0.100M BaCl22H2O solution. • __________ grams mass of solute needed • __________ Instructor initials (one point)

46. What are the products of the reaction? Balance the equation. Write the balanced molecular, complete ionic and net ionic equations below. Place the precipitate on the 3rd line of the first row of lines. (5 points) ________ + ________  ________ + ________ ___ ____ + ___ ____  ______ + ___ ____ •   ____ + ___  _____ • What is this the best molar ratio based on the stoichiometry? Should you have put all 50.00 mL of each reactant together to form the most product? Circle yes or no. (2 points) ____________ : ____________ Yes No

47. Preparing Solutions • Determine the mass of solute. • Place in the appropriate volumetric flask. • Add deionized water and swirl until solute is dissolved. • Add water to the mark on the neck of the flask. • Stopper and mix thoroughly.

49. PROBLEM: Dissolve 5.00 g of NiCl2•6 H2O in enough water to make 250 mL of solution. Calculate the Molarity. Step 1: Calculate moles of NiCl2•6H2O Step 2: Calculate Molarity [NiCl2•6 H2O ] = 0.0841 M

50. x 1 mol H2C2O4 90.04 g H2C2O4 USING MOLARITY What mass of oxalic acid, H2C2O4, is required to make 250. mL of a 0.0500 M solution? moles = M•V X g H2C2O4 = 0.0500 x 0.250 L = 1.13 g H2C2O4