1 / 18

Chapter 12

Chapter 12. Solutions. Solution. Solution- homogeneous mixture of 2 or more substances in a single phase Substances have to be soluble (dissolvable) “If not part of solution, part of precipitate” Solute- dissolved Solvent- does the dissolving

aretha-reilly
Download Presentation

Chapter 12

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. Chapter 12 Solutions

  2. Solution • Solution- homogeneous mixture of 2 or more substances in a single phase • Substances have to be soluble (dissolvable) • “If not part of solution, part of precipitate” • Solute- dissolved • Solvent- does the dissolving • If both liquid in equal amount, can’t say which is which

  3. Types of solutions • Alloys- Brass (Zn + Cu), Sterling Ag (Ag + Cu) • G in G • G in L • L in L • L in S • S in L • S in S • Examples of each will be discussed

  4. Mixtures • Heterogeneous • Either colloid or suspension

  5. Colloid • Colloid • Middle size particles • 1 nm – 1000 nm • Can’t be filtered • Does not settle out over time • Muddy water • Mayo – oil, water, egg yolk • Tyndall Effect- light scatters, appears “foggy” (movie theater projector light stream)

  6. Suspension • Largest particle size • Particles settle out over time • Over 1000 nm • Can be filtered • Blood- rigor mortis, centrifuge • Milk- layers of cream • Soil- rock layers • Other examples

  7. Electrolytes • Solutes can be electrolytes or nonelectrolytes • Electrolytes- dissolve in water and conduct electricity • Nonelectrolytes cannot conduct electricity • Examples of each • Review of dipoles, van der Waals forces

  8. How to affect rate of dissolution • Increase surface area of solute • Agitate • Heat • What does each do to the solute • Translation

  9. Solution equilibrium • Dissolution and crystallization occur at the same rate • See double arrow (Scarecrow in Wizard of Oz giving directions) • How we push it to one side- Le Chatlier’s Principle

  10. Saturation • Saturated- maximum amount of solute dissolved • Unsaturated- can add more solute • Supersaturated- more than saturated, add one flake and it crystallizes (seeding) • Boil saturated to make supersaturated • Examples

  11. Solute-Solvent interactions • Like dissolves like- polar vs. nonpolar • Hydration- water breaks solute • L + L- immiscible if don’t mix • L + L- miscible if mix • Examples • Increase Pressure, go to L phase

  12. Gases • Henry’s Law- solubility of gas is directly proportional to the partial pressure of gas on liquid surface • Rapid escape of gas from liquid- effervescence • Increase temperature, decrease gas solubility

  13. Liquid and solid • Can’t predict liquid solubility if change temp. • Increase temperature, increase solid solubility • Enthalpy chart of dissolving 2 solids, enthalpy released

  14. Molarity • M = mole solute/L solution • M1V1 = M2V2 • Example problems

  15. molality • m = moles solute/kg solvent • Example problems

  16. Normality • Dissolvable hydrogens/L solution

  17. Mole ratio • X = moles solute/moles solvent

  18. V/V ratio • Volume solute/volume solvent

More Related