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The Extraordinary Properties of Water

The Extraordinary Properties of Water. Where there’s life……there’s water!!!. H. H. Water. A water molecule (H 2 O), is made up of three atoms --- one oxygen and two hydrogen. O. Water is Polar. Having positively and negatively charged sides. The oxygen end “acts” negative

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The Extraordinary Properties of Water

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  1. The Extraordinary Properties of Water Where there’s life……there’s water!!!

  2. H H Water • A water molecule (H2O), is made up of threeatoms --- one oxygenand two hydrogen. O

  3. Water is Polar • Having positively and negatively charged sides. • Theoxygenend“acts” negative • Thehydrogenend“acts” positive • The term “POLARITY” means the molecule has an uneven distribution of electrons

  4. What are the Properties of Water? The Universal Solvent

  5. Properties of Water • Cohesion • Adhesion

  6. Cohesion – “Co” means“With or Together” • Attraction betweensimilarsubstances (why water is attracted to itself) • Due to Hydrogenbonds

  7. Cohesion • Produces a surface film on water called • surface tension that allows insects to walk on water and leaves to float. • Surface Tension - a measure of the strength of water’ssurface

  8. Adhesion • Attraction of H2O to different substances. • Due to hydrogen bonds • Ex:paper towels soak up water, meniscus in a graduated cylinder.

  9. Adhesion Also Causes Water to … Attach to a silken spider web Form spheres & hold onto plant leaves

  10. Both Cohesion and Adhesion Causes Capillary Action Capillary action gives water the ability to “climb” structures

  11. High Specific Heat • Amount of heat needed to raise the tempof1g of H2O 1° C. • Water has a very HIGHspecific heat. • Crucial in temperature stabilityin living systems to maintain homeostasis.

  12. High Heat of Vaporization • Amount of energy to convert 1g water from a liquid to a gas. • Called vaporization orevaporation

  13. High Heat of Vaporization • As water evaporates, it removes a lot of heat with it (cooling effect). • Ex: evaporation of sweatfrom the body

  14. Water is Less Dense as a Solid • Ice is less denseas a solid than as a liquid – therefore it floats • Other materials contractwhen they solidify, but water expands.

  15. Water is Less Dense as a Solid • Which is ice and which is water? Water Ice

  16. Water is a Solvent • Solvent: any substance that dissolves other substances. • Water is averyversatilesolvent • Other polar substances dissolve easily in water.

  17. Solution • Mixture of 2 or more substances. • Evenly distributed + +

  18. MIXTURE Materials composed of 2 or more elements or compounds that are physically mixed but not chemically combined.

  19. Hydrophilic (“water-loving” ) • substances that dissolve easily in water are known as water soluble. • Examples: salts, polar compounds (sugar).

  20. Hydrophobic(means “water-fearing”) • substances that do not dissolve easily in water separate and are known as insoluble.. • Examples: oils, fats, lipids, waxes. • These substances are non-polar.

  21. Acids, Bases and pH One water molecule in 550 million naturally dissociates into a Hydrogen Ion (H+) and a Hydroxide Ion (OH-) Hydrogen Ion Hydroxide Ion Acid Base H2O  H+ + OH-

  22. The pH Scale • Ranges from 0 to 14 • Measures strength of an acid or base by concentration of H+ ions and OH- ions. • Pure Water has a pH level of 7.

  23. Acids • Substance that contains high concentration of H+ ions. • pH of acids range from 0-6 • Strong acids have a pH of 1-3

  24. Bases • Substance that have lower concentrations of H+ ions thus increasingOH- ions • Bases have a pH value range from 8 to 14. • Strong Bases have a pH of 11 to 14

  25. Buffers • Weak acids or bases that react with strong acids or bases to prevent sharp, sudden changes in pH (neutralization). • Produced naturally by the body to maintain homeostasis Weak Acid Weak Base

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