1 / 45

Solutions

Solutions. Chapter 14. Common Solutions. Chemical solutions encountered in everyday life: air coffee tap water gasoline shampoo cough syrup orange soda Gatorade. Solutions. . . . the components of a mixture are uniformly intermingled (the mixture is homogeneous ). A Solute.

maegan
Download Presentation

Solutions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Solutions • Chapter 14

  2. Common Solutions • Chemical solutions encountered in everyday life: • air coffee • tap water gasoline • shampoo cough syrup • orange soda Gatorade

  3. Solutions • . . . the components of a mixture are uniformly intermingled (the mixture is homogeneous).

  4. A Solute • dissolves in water (or other “solvent”) • changes phase (if different from the solvent) • is present in lesser amount (if the same phase as the solvent)

  5. A Solvent • retains its phase(if different from the solute) • is present in greater amount (if the same phase as the solute)

  6. Figure 14.1: When solid sodium chloride dissolves, the ions are dispersed randomly throughout the solution

  7. Aqueous Solutions • Aqueous solutions are solutions in which water is the solvent. • Aqueous solutions are the most common type of solution.

  8. Some Properties of Water • Water is able to dissolve so many substances because: • Water is “bent” or V-shaped. • The O-H bonds are covalent. • Water is a polar molecule. • Hydration occurs when salts dissolve in water.

  9. Water is a polar molecule because it is a bent molecule. The hydrogen end is + while the oxygen end is -, Delta () is a partial charge--less than 1.

  10. Polar water molecules interact with the positive and negative ions of a salt, assisting in the dissolving process. This process is called hydration.

  11. Solubility • The general rule for solubility is: • “Like dissolves like.” • Polar water molecules can dissolve other polar molecules such as alcohol and, also, ionic substances such as NaCl. • Nonpolar molecules can dissolve other nonpolar molecules but not polar or ionic substances. Gasoline can dissolve grease.

  12. Miscibility • Miscible -- two substances that will mix together in any proportion to make a solution. Alcohol and water are miscible because they are both polar and form hydrogen bonds. • Immiscible -- two substances that will not dissolve in each other. Oil and vinegar are immiscible because oil is nonpolar and vinegar is polar.

  13. Figure 14.6: An oil layer floating on water

  14. Structure & Solubility • Like dissolves like. • Hydrophobic --water-fearing. Fat soluble vitamins such as A, D, E, & K. • Hydrophilic --water-loving. Water soluble vitamins such as B & C. • Hypervitaminosis--excessive buildup of vitamins A, D, E, & K in the body.

  15. Solubility • How does the rule “Like dissolves like.” apply to cleaning paint brushes used for latex paint as opposed to those used with oil-based paint?

  16. Common Terms of Solution Concentration • Saturated - when a solution contains as much solute as will dissolve at that temperature. • Unsaturated - when a solution has not reached its limit of solubility. • Supersaturated - when a solution has more of the solute dissolved than it normally would --very unstable.

  17. Common Terms of Solution Concentration • Stock - routinely used solutions prepared in concentrated form. • Concentrated - relatively large ratio of solute to solvent. (5.0 M NaCl) • Dilute - relatively small ratio of solute to solvent. (0.01 M NaCl)

  18. Qualitative -- general and relative. dilute concentrated Quantitative -- mathematically defined. Mass % -- biology Molarity -- most solutions in chemistry Normality -- chemical titrations Molality -- molar mass, freezing point depressions, & boiling point elevations Solution Composition

  19. Mass % • Mass (weight) percent =

  20. Mass % Calculations • If 1.00 g of ethanol is added to 100.0 g of water, what is the mass % of the ethanol?

  21. Mass % Calculations • Cow’s milk typically contains 4.5 % by mass of the sugar lactose, C12H22O11. Calculate the mass of lactose present in 175 g of milk. • Mass % = • mass of solute = (mass %)(mass of solution)/(100%) • mass of solute = (4.5 % lactose)(175 g)/(100%) • mass of solute = 7.9 g lactose

  22. Molarity • Molarity (M) = moles of solute per volume of solution in liters:

  23. Molarity Calculations • If 1.00 g of ethanol is dissolved in enough water to make 101 mL of solution, what is the molarity of the solution?

  24. Molarity Calculations • Calculate the molarity of a solution prepared by dissolving 11.5 g of solid NaOH in enough water to make 1.50 L of solution. • (11.5g NaOH/1.50L)(1 mol NaOH/40.00g NaOH) • = 0.192 M NaOH

  25. Molarity Calculations • Calculate the molarity of a solution prepared by dissolving 1.56 g of gaseous HCl into enough water to make 26.8 mL of solution. • (1.56g HCl/26.8mL)(1mol/36.5g)(1000mL/1L) = 1.59 M HCl solution

  26. Molarity Calculations • How many moles of nitrate ions are present in 25.00 mL of a 0.75 M Co(NO3)2 solution? • (25.00mL)(1L/1000mL)(0.75mol Co(NO3)2/1L) • (2 mol NO3-/1 mol Co(NO3)2) = 3.8 x 10-2 mol NO3-

  27. Molarity Calculations • Typical blood serum is about 0.14M NaCl. What volume of blood contains 1.0 mg of NaCl? • (1.0mg NaCl)(1g/1000mg)(1mol/58.45g)(1L/0.14mol) = 1.2 x 10-4 L blood serum

  28. Molarity Calculations • A chemist needs 1.00 L of an aqueous 0.200 M K2Cr2O7 solution. How much solid potassium dichromate must be massed to make this solution? • (1.00L)(0.200mol K2Cr2O7/L)(294.2g/1mol) = 58.8 g K2Cr2O7

  29. Standard Solution • A standard solution is a solution whose concentration is accurately known. • A volumetric flask is used to make a standard solution.

  30. Steps involved in making a standard solution.

  31. Dilution of Stock Solutions • When diluting stock solutions, the moles of solute after dilution must equal the moles of solute before dilution. • moles of solute before dilution = moles of solute after dilution • Stock solutions are diluted using either a measuring or a delivery pipet and a volumetric flask.

  32. Steps to dilute a stock solution.

  33. Dilution Calculations • What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.10 M H2SO4 solution? • (0.10mol H2SO4/1L)(1.5L)(1L/16mol)(1000mL/1L) • = 9.4 mL conc H2SO4

  34. Dilution Calculations • What volume of 12 M HCl must be taken to prepare 0.75 L of 0.25 M HCl? • (0.75L)(0.25mol HCl/L)(1L/12mol)(1000mL/1L) = 16 mL conc. HCl

  35. Steps For Solving Solution Stoichiometry Problems • 1. Write the balanced reaction. • 2. Calculate moles of reactants. • 3. Determine limiting reactant. • 4. Calculate moles of required reactant/product. • 5. Convert to grams or volume, as required.

  36. Precipitation Calculations • When aqueous solutions of Na2SO4 & Pb(NO3)2 are mixed, PbSO4 precipitates. Calculate the mass of PbSO4 formed when 1.25 L of 0.0500 M Pb(NO3)2 & 2.00 L of 0.0250 M Na2SO4 are mixed. • 1. Pb(NO3)2(aq) + Na2SO4(aq) ----> PbSO4(s) + 2NaNO3(aq) • 2. (1.25L)(0.0500mol Pb(NO3)2/L) = 0.0625 mol Pb(NO3)2 • (2.00L)(0.0250mol Na2SO4/L) = 0.0500 mol Na2SO4

  37. Precipitation CalculationsContinued • 3. (0.0625mol Pb(NO3)2)(1mol Na2SO4/1mol Pb(NO3)2 = • 0.0625 mol Na2SO4 • Na2SO4is the limiting reactant. • 4. (0.0500mol Na2SO4)(1mol PbSO4/1mol Na2SO4) • (303.3g/1mol) = 15.2 g PbSO4

  38. Neutralization Reactions • Acids and bases react to neutralize each other and form a salt and water. This type of reaction is called a neutralization reaction. • HCl(aq) +NaOH(aq) ----> NaCl(aq) + HOH(l)

  39. Acid-Base Calculations • What volume of a 0.100 M HCl solution is needed to neutralize 25.0 mL of 0.350 M NaOH? • HCl(aq) + NaOH(aq) ----> HOH(l) + NaCl(aq) • (25.0mL)(0.350mol NaOH/1L)(1mol HCl/1mol NaOH)(1L/0.100mol) = 87.5 mL HCl solution

  40. Normality • Acid-Base Equivalents = (moles) (total (+) charge) • N = M ( total (+) charge)

  41. Normality Calculations • .250 M H3PO4 =______N • N = M(total(+) charge) • N = (0.250)(3) • N = 0.750 N H3PO4

  42. Normality Calculations • A solution of sulfuric acid contains 86 g of H2SO4 per liter of solution. What is its normality? • (86g H2SO4/1L)(1mol/98.0g) = 0.88 M H2SO4 • N = M(total (+) charge) • N = (0.88M)(2) • N = 1.8 N H2SO4

  43. Normality Stoichiometry Calculations • What volume of a 0.075 N NaOH solution is required to react exactly with 0.135 L of 0.45 N H3PO4? • Na = 0.45 N • Va = 0.135 L • Nb = 0.075 N • Vb = ? NaVa = NbVb Vb = (NaVa)/Nb Vb = (0.45N)(0.135L)/(0.075N) Vb = 0.81 L NaOH

More Related