1 / 17

Ch. 13 Solutions

Ch. 13 Solutions. What is a solution? A homogeneous mixture of 2 or more substances in a single phase. What is a substance that is capable of being dissolved? Soluble. What is the substance being dissolved called? Solute The substance that dissolves the solute is called what? Solvent.

leane
Download Presentation

Ch. 13 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. Ch. 13 Solutions • What is a solution? • A homogeneous mixture of 2 or more substances in a single phase. • What is a substance that is capable of being dissolved? • Soluble

  2. What is the substance being dissolved called? • Solute • The substance that dissolves the solute is called what? • Solvent

  3. Homogenous mixture – can’t distinguish the difference in substances • Ex. Tomato juice, pop, vanilla ice cream • Heterogenous mixture – can distinguish the substances in the mixture. • Ex. Stew, salad, chocolate chip ice cream • Video

  4. What is an electrolyte? • A substance that conducts electricity in a solution. • Ex. NaCl in water • A nonelectrolyte is a substance that doesn’t conduct electricity in a solution. • Ex. Sugar in water

  5. What is an alloy? • A solid solution with 2 or more metals mixed together. • Ex. Cu + Sn = Bronze • Ex. Cu + Zn = Brass • Ex. 50% Au + 50% Cu = 12 karat Au • Video

  6. Suspension – is a heterogeneous mixture of a solvent-like substance with particles that slowly settle out. • Ex. Muddy water (separate by a filter) • Video • Colloids – have particles that are intermediate in size between those in solutions & suspension. Don’t settle. • Ex. Milk (Tyndall Effect) • Video

  7. Factors that affect the rate of dissolving • 1. Heat the solvent • 2. Stir/mix the solution • 3. Crush/grind the solution • What is solubility? • The rate at which the solvent dissolves the solute at a given temp. • Video

  8. Solutions • What is a saturated solution? • A solution that can’t take on any more solute and dissolve it. • What is a unsaturated solution? • A solution that can take on more solute. • What is supersaturated solution? • A solution with more solute than a saturated solution. (over saturated) • Video

  9. Polar vs. Nonpolar • “Likes dissolve alike” • A polar molecule dissolves a polar molecule. • Ex. Water and salt (both polar) • Ex. Gasoline and benzene (non polar) • Ex. Water and gasoline don’t mix • Polar & nonpolar

  10. Immiscible are substances that is not soluble in each other. • Ex. Gas & water, oil & water • Miscible are substances that are soluble in each other. • Ex. NaCl & water, gas & benzene

  11. Ethanol & ether both have polar and nonpolar ends on their molecules, thus they are able to dissolve both polar and nonpolar substances. • The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid.  Henry’s Law

  12. Example of Henry’s Law • Gas is released in a carbonated pop bottle when opened because the pressure is less. • What is effervescence? • The rapid escape of a gas from a liquid in which it was dissolved in.

  13. Table 13-4 Solubility vs. Temperature • Concentration of a solution is the measurement of the amount of solute in a given amount of solvent or solution. • Ex. Concentrated O.J. or Conc. HCl • A concentration of a solution can be diluted by adding H2O.

  14. Percent by mass is the number of grams of solute dissolved in 100 g of solution.  Sample Problem 13-1 • Ex. 10 g of NaOH in 90 g of H2O • 10 g of NaOH / 10 g of NaOH + 90 g of H2O X 100% = 10% NaOH (by mass)

  15. Molarity • Molarity is the number of moles of solute in 1 liter of solution. • To find the molarity of a solution you must know the molar mass of the solute. • Molarity (M) = # of moles of solute / # of liters of solution • Example Problem 13-2

  16. Molality • Molality is the concentration of a solution expressed in moles of solute per kilogram of solvent. • Molality (m) = # of moles of solute / mass of solvent (kg) Sample Problem 13-4

  17. Nonvolatile is a substance with little tendency to become a gas under the existing condition. • Ex. A lower freezing point & higher boiling point than water. • Colligative property is a property that depends on the # of solute particles, but is independent of their nature. • Ex. antifreeze

More Related