1 / 45

Understanding Solutions: Solubility, Dissolving, Concentration

Explore the world of solutions, solubility rules, factors affecting solubility, concentration measurements, colligative properties, and heterogeneous mixtures. Learn about acids, bases, and salts as electrolytes and their characteristics. Enhance your knowledge in chemistry.

eldridgek
Download Presentation

Understanding Solutions: Solubility, Dissolving, Concentration

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/Acid & Bases Chapter 15 & 19

  2. Solution are homogenous mixtures. • Solutions are made up of 2 things: • A solute & a solvent. • Water is the most common solvent in liquid solutions.

  3. Dissolves in a solvent Example: Sugar in water Will not dissolve in a solvent Example: Sand is insoluble in water. Soluble & Insoluble

  4. Two liquids that are soluble in one another Example: Antifreeze & water Acetic acid & water Two liquids not soluble in one another Example: Oil & vinegar Oil & water Miscible & Immiscible

  5. What gets dissolved. The lesser amount of substance in a solution. Example: Sugar Salt What things dissolve in. The greater amount of substance in a solution. Example: Water Ethanol Solute & Solvent

  6. Solvation • Rules: • Like dissolves like. • Polar dissolves polar. • Nonpolar dissolves nonpolar.

  7. Solvation of salt cont… • Formula units break apart & ions become attracted to charges of the water molecules.

  8. Solvation of salt

  9. Solvation of sugar (covalent) • In polar molecules, water molecules have a stronger attraction to the polar molecules than they have to each other.

  10. “What can affect solubility?” Two factors that affect rates of solutions. • Temperature • Pressure

  11. Surrounding solute particles with solvent particles. Breaking apart. “Dissolving” Hydration Particles coming together. Dehydration Solvation & Crystallization

  12. Max amount of solute dissolves in a solvent at a temp/pres. Ex: Concentrated or strong tea Less solute is dissolved than saturated. It can dissolve more. Ex: Diluted or weak tea Saturated & Unsaturated

  13. Factors that affect solubility 1. Temperature: • For solids- ↑ temperature, ↑ solubility • For gases- ↑ temperature, ↓ solubility 2. Pressure: • For gases in liquid- ↑ pressure, ↑ solubilty

  14. Super saturated solution- a solution that contains more solute than saturated solutions at the same temp/pressure

  15. http://www.youtube.com/watch?v=D1PDE5OawuI&edufilter=iaYy5cltW5JHB2qLmddDPghttp://www.youtube.com/watch?v=D1PDE5OawuI&edufilter=iaYy5cltW5JHB2qLmddDPg

  16. Henry’s Law- at a given temperature, solubility of a gas in a liquid is directly proportional to the pressure of a gas above the liquid. • Example: a soda

  17. 15.2 Solution Concentration • How much solute is dissolved in a specific amount of solvent is concentration

  18. Describing concentration • Qualitative: • Concentrated or diluted

  19. Describing concentration • Quantitative: • Percent by volume • Molarity (M) • Molality • Normality

  20. Molarity: (M)(mol/L)= moles of solute liters of solution

  21. Example 1 • A 100.5 mL intravenous solution contains 5.10 g of glucose (C6H12O6). What is the molarity of this solution? • Hint: glucose molar mass is 180. g/mol. • Practice 1-3

  22. 15-3 Colligative Properties of Solutions • Physical properties that are affected by the number of particles and not by their identity are colligative properties.

  23. Examples of colligative properties include: • 1. vapor pressure lower • 2. boiling point elevation • 3. freezing point depression • 4. osmotic pressure

  24. Solutions: • Solutes will not settle out • Will not scatter light • Cannot filter

  25. 15-4 Heterogeneous Mixtures • Suspensions: • Settles out • Scatters light • Can be separated by filtering • Are large particles (>1000 nm) • Examples: muddy water, fine sand in water

  26. Colloids: • Don’t settle out • Scatters light • Can’t be filtered • Medium to small sizes (<1000 nm) • Examples: milk

  27. Brownian motion is the random movement of colloid particles. • Causes collision of particles preventing them from settling.

  28. Tyndall effect: • Particles scatter light • Can be seen in suspensions & colloids • Examples: ray of light through fog or smoke

  29. Acid & Bases Chapter 19 • Acids, bases, & salts are electrolytes because they conduct electrical current. • An indicator is a compound that changes color to indicate the presences of an acid or base.

  30. Characteristics of acids • Sour taste • Reacts with metals • Neutralizes bases • affects indicators • turns blue litmus red/pink • keeps phenolphthalein colorless • turns methyl orange red

  31. Common Acids: • Citric acid- in citrus fruits • (Lemons, oranges, etc) • Acetic acid- vinegar • Malic acid- apple • Butyric acid- sour butter • Lactic acid- sour milk; builds up in muscles during exercise.

  32. Industrial acids: • Sulfuric acid- (H2SO4) most manufactored chemical in US; fertilizers • Phosphoric acid- (H3PO4) fertilizers; detergents • Nitric acid- (HNO3) fertilizers; explosives • Hydrochloric acid- (HCl) used to “pickle” steel (remove surface impurities)

  33. Review: Naming acids • 1. Binary acids- (only 2 elements) “hydro________ic acid” • Ex. HBr • Ex. H2S • 2. Oxyacids- (has polyatomic ions) “________ic acid” • Ex. HClO3 • Ex. H2SO4

  34. Characteristics of Bases • tastes bitter • feels slimy • affects indicators • pink litmus turns blues • phenolphthalein turns bright pink • methyl orange turns yellow

  35. Common Bases: • Ammonia- (NH3) cleaning agent • Lye- (NaOH) draino • Milk of magnesia- (Mg(OH)2) laxative • Lime- (Ca(OH)2) mortar for bricks, foul lines on fields

  36. What is pH? • pH is the negative logarithm of H+1 ion concentration • pH= -log[H+] • pH range- 014 • pH scale: acids  0-6.99, neutral  7, base  7.01-14

  37. Example 2 • What is the pH of a solution with the concentration [H+]= 1.0 x 10-7 M? • Practice 4. What is the pH of [H+]=1.0x10-2? 5. What is the pH of [H+]=3.0x10-6? pOH? 6. What is the pOH of [OH-]=8.2x10-6?

  38. Ex. 3 What is the concentration (Molarity) of H+ of an acidic solution with the pH of 3.20? • Practice: • 7. Calculate the concentration of H+ of an acidic solution with the pH of 6.55.

  39. Neutralization • Neutralization Reaction- reaction between an acid & base to produce a salt & water • Salt- made of the positive ion (from base) & the negative ion (from acid) • Example: • Mg(OH)2 + HCl  • Practice: • H3PO4 + Ca(OH)2 • Al(OH)3 + H2SO4 

  40. Acid is the sub. containing H Base is the sub. containing OH Ex. HCl & NaOH Acid is the sub. that loses the H+ Base is the sub. that gains the H+. involves conj. acid & bases H2O + NH4+ NH3 + H3O+ Arrhenius vs Bronted-Lowry

  41. Practice: • Identify the following Bronsted-Lowry acids & bases. • HC2H3O2 +H2O  H3O+ + C2H3O2-

  42. Anhydrides are compounds that can become acids or bases when water is added. • Ex. Which is the anhydride? • CO2 + H2O  H2CO3 • Practice. Which is the anhydride? • CaO + H2O Ca(OH)2 • H2O + SO2  H2SO4

More Related