1 / 29

Chapter 6: Sports Drink

Chapter 6: Sports Drink. Introductory Activity. What do you think are the benefits of drinking a sports drink while exercising rather than plain water? How are your ideas influenced by the marketing strategies of the companies that sell these drinks?. Section 6.1—Solutions & Electrolytes.

harrisdavid
Download Presentation

Chapter 6: Sports Drink

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 6: Sports Drink

  2. Introductory Activity • What do you think are the benefits of drinking a sports drink while exercising rather than plain water? • How are your ideas influenced by the marketing strategies of the companies that sell these drinks?

  3. Section 6.1—Solutions & Electrolytes What are those “electrolytes” they say you’re replacing by drinking sports drinks? • Explain the process of dissolving • Explain how ionic substances produce electrolytes in water • Distinguish between unsaturated, saturated, and supersaturated solutions

  4. Solutions Solutions are homogeneous mixtures that contain two or more substances called the solute and solvent. The solute is the substance that dissolves. The solvent is the dissolving medium. It is not possible to distinguish the solute from the solvent by appearance. It is also not possible to separate the solute from the solvent by filtration.

  5. Most solutions are liquids, but gaseous and solid solutions exist. The state of the solvent determines the type of solution. In aqueous solutions, the solvent is water.

  6. Solvation • Substances are dissolved by a process called solvation • It is defined as the process of surrounding solute particles with solvent particles to form a solution. • Solvation in water is also called “hydration.”

  7. Steps in Solvation • - Intermolecular attractive forces between solute particles must be broken. • - Intermolecular attractive forces between solvent particles must be broken. • - New intermolecular attractive forces between solute and solvent particles must form

  8. - - O H H + Dissolving Ionic Compounds - + Ionic compound water Water molecules are polar and they are attracted to the charges of the ions in an ionic compound. When the intermolecular forces are stronger between the water and the ion than between the ions, the water “pulls” the ion into solution. + - + - + - + -

  9. - - + O + H H + Dissolving Ionic Compounds - + Ionic compound water As more ions are “exposed” to water molecules, more ions can be “pulled” into solution as well. - - + - + -

  10. - O H H + Dissolving Ionic Compounds - + Ionic compound water + - These ions in the solution allow electricity to be conducted through the solution. - + - + - + -

  11. Electrolytes • When there are free-floating charges in a solution, then it can conduct electricity. • Compounds that produce free-floating ions when dissolved in water are called electrolytes.

  12. + - + Solute, sugar (polar) Solvent, water (polar) - - + - + - + - + - + Dissolving Covalent Compounds Polar covalent molecules are dissolved in the same way—intermolecular forces form between the water and solute. Water “pulls” the solute particles into solution.

  13. + - + Solute, sugar (polar) Solvent, water (polar) - - + - + - + - + - + Dissolving Covalent Compounds However, the polar covalent molecules themselves do not split into charged ions—the solute molecule stays together and just separates from other solute molecules.

  14. Non-electrolytes • When molecules separate from other molecules (breaking intermolecular forces), but free-floating charges are not produced, the solution cannot conduct electricity. • These are called non-electrolytes.

  15. Types of Electrolytes Non-Electrolytes Strong Electrolytes Weak Electrolytes Covalent Compounds Ionic compounds Ionic Compounds No molecules separate—ions are not formed Almost all ions are separated when dissolved in water. Only a few ions are separated when dissolved in water Does not conduct electricity at all when dissolved in water Easily conducts electricity when dissolved in water Conducts electricity slightly when dissolved in water

  16. How to Break up Electrolytes • Leave polyatomic ions intact (including the subscript within the polyatomic ion) • All subscripts not within a polyatomic ion become coefficients • Be sure to include charges on the dissociated ions! Example: Break up the following ionic compounds into their ions KNO3 Ca(NO3)2 Na2CO3

  17. Breaking up Electrolytes • Leave polyatomic ions in-tact (including the subscript within the polyatomic ion) • All subscripts not within a polyatomic ion become coefficients • Be sure to include charges on the dissociated ions! Example: Break up the following ionic compounds into their ions  K+1 + NO3-1  Ca+2 + 2 NO3-1  2 Na+1 + CO3-2 KNO3 Ca(NO3)2 Na2CO3

  18. Misconceptions about dissolving • People often describe something that dissolves as having “disappeared” • Before the solute dissolves, it’s in such a large group of particles that we can see it. • After dissolving, the solute particles are still there—they’re just spread out throughout the solution and are in groupings so small that our eyes can’t see them

  19. Solubility • Solubility is defined as the maximum amount of solute that can dissolve in a given amount of solvent at a particular temperature and pressure.

  20. Solubility Curves • Solubility is usually expressed in grams of solute per 100 g of solvent at a specified temperature. • A graph of solubility vs. temperature is called a solubility curve.

  21. How Much Will Dissolve? • Solubility is affected by temperature. SOLIDS dissolved in water GASES dissolved in water

  22. HOW MUCH WILL DISSOLVE? • For solids in water, generally solubility ________ with temperature. • For gases in water, solubility _________ with temperature.

  23. Saturated Solutions • Solubility curves relate information about saturated solutions. • A saturated solution contains the maximum amount of solute that can dissolve for a given amount of solvent at a specific temperature and pressure.

  24. Saturated solutions • In a saturated solution, as long as the conditions remain constant, the overall amount of dissolved solute remains constant. If more solute is added to a saturated solution, it will . . . • In a saturated solution, if the temperature of the solvent is increased, generally more solid solute will . . .

  25. Unsaturated Solutions • An unsaturated solution is one that contains less dissolved solute for a given temperature and pressure than a saturated solution. • If more solute is added to an unsaturated solution, it will . . .

  26. Supersaturated Solutions • A supersaturated solution contains more dissolved solute than a saturated solution at the same temperature. • Such solutions are unstable. If the solution is disturbed or “seeded”, the excess solute will precipitate out.

  27. How To Make a Supersaturated SolutionExample: Glucose

  28. Supersaturated Solutions

  29. Types of Solutions Super-Saturated Unsaturated Saturated Has more solute than would make a saturated solution dissolved More solute can be dissolved No more solute can be dissolved—it’s “full” In general, if you increase the temperature of a solution, more solid solute will dissolve but less gaseous solute will dissolve.

More Related