1 / 27

Chapter 15 Solutions

Chemistry B2A. Chapter 15 Solutions. Mixtures. Mixture: is a combination of two or more pure substances. Homogeneous: uniform and throughout Air, Salt in water. Solution. Heterogeneous: nonuniform Soup, Milk, Blood. Solutions.

skyler
Télécharger la présentation

Chapter 15 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. Chemistry B2A Chapter 15 Solutions

  2. Mixtures Mixture:is a combination of two or more pure substances. Homogeneous: uniform and throughout Air, Salt in water Solution Heterogeneous: nonuniform Soup, Milk, Blood

  3. Solutions Gas in gas (air) solid in solid (alloys) liquid in liquid (alcohol in water) Gas in liquid (cokes) solid in liquid (sugar in water) Solutions Well-mixed (uniform) – single phase homogenous transparent cannot be separated by filter cannot be separated on standing sugar in water

  4. Immiscible: two liquids do not mix. alcohol in water Miscible: two liquids can mix. (in any quantities) Solutions (liquid in liquid) Solvent: greater quantity (water) Solute: smaller quantity (sugar)

  5. Solvent and Solute Polar dissolves polar Nonpolar dissolves nonpolar like dissolves like.

  6. Hydrogen Bonds Between H bonded to O or N (high electronegativity) → +ᵟ and another O or N → -ᵟ H2O High boiling point surface tension

  7. Dissolving Ionic compounds Ions Hydrated by H2O Hydration

  8. electrolyte + - Electrolytes bulb Electrolyte:conducts an electric current. Na+ Cl- Ionization (Dissociation) NaCl → Na+ + Cl- strong electrolytes:molecules dissociate completely into ions (NaCl). weak electrolytes:molecules dissociate partially into ions (CH3COOH). nonelectrolytes:molecules do not dissociate into ions (DI water).

  9. Solvent and Solute All nitrates (NO3-) and acetate (CH3COO-) are soluble in water. Most salts of Na+, K+, and NH4+ are soluble in water. Most chlorides (Cl-) and sulfates (SO42-) are soluble in water. (except AgCl, PbCl2, BaSO4, CaSO4, PbSO4) Most carbonates (CO32-), phosphates (PO43-), Sulfide (S2-), and hydroxides (OH-) are insoluble in water. (except NaOH, KOH, Ba(OH)2, Ca(OH)2, and NH4OH)

  10. Supersaturated:solvent holds more solute that it can normally hold (at a given T). (more than an equilibrium condition) Solutions Saturated:solvent contains or holds all the solute it can (at a given T). maximum solute that solvent can hold (Equilibrium). Unsaturated:solvent can hold more solute (at a given T). Is not the maximum solute that solvent can hold.

  11. T  Solubility  Crystal is formed. T  Temperature and Solutions Solubility:the maximum solute that will dissolve in a given amount of a solvent (at a given T).

  12. T  Solubility  Temperature and Solutions Supersaturated solution Seeding A surface on which to being crystallizing.

  13. Solubility ↓ gas in liquid: T ↑ Global Warming

  14. Pressure and Solutions Henry’s law P  Solubility  (gas in liquid)

  15. Concentration Concentrated solution:large amount of solute is dissolved. Strong Coffee Dilute solution:small amount of solute is dissolved. Weak Coffee

  16. Concentration Concentration:amount of a solute in a given quantity of solvent. 1. Percent concentration: Weight solute (g) × 100 Weight / volume (W / V)% = Volume of solution (mL) Weight solute (g) × 100 Weight / Weight (W / W)% = Weight of solution (g) Volume solute (mL) × 100 Volume / volume (V / V)% = Volume of solution (mL)

  17. Concentration 2. Molarity (M): number of moles solute dissolved in 1 L of solution. moles solute (n) Molarity (M) = volume of solution (L) Molarity × V = number of moles (n) prepare the solution: M, V → n (mol) → m (g)

  18. m (g) Volumetric flask Prepare the solution prepare the solution: M, V → n (mol) → m (g)

  19. Concentration 3. Parts per Million (ppm): g solute ppm = × 106 g solvent Parts per billion (ppb): g solute ppb = × 109 g solvent

  20. Dilution Dilute solution Concentrated solution (Stock solution) Standard solution:a solution with known concentration.

  21. Dilution M1V1 = moles(n) before dilution M2V2 = moles(n) after dilution Mole remains constant. M1V1 = M2V2 % V1 = % V2

  22. Neutralization Reactions We will talk about this in Chapter 16.

  23. Normality We will talk about this in Chapter 16.

  24. Colloids Solutions:diameter of the solute particles is under 1 nm. Colloids:diameter of the solute particles is between 1 to 1000 nm. non transparent, non uniform, large particles, cloudy (milky) But it is a stable system.

  25. Colloids Tyndall effect: You can see the pathway of the light passes through a colloid. (particles scatter light.) emulsion:a mixture of immiscible substances (liquid-liquid). (milk and mayonnaise)

  26. Brownian motion Random motion of colloid particles. Dust Why do colloidal particles remain in solution and do not stick together? 1. Surrounding water molecules prevent colloidal molecules from touching and sticking together. 2. A charged colloidal particle encounters another particle of the same charge, they repel each other.

  27. Suspension suspension:system does not stays stable and settle (> 1000 nm). (sand in water) But it is not a stable system.

More Related