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2.2 Properties of Water
Pages 40 - 43
Goal 1:Explain the polarity of water
molecules
• Polar molecule
– A molecule with slightly charged “poles”
– One end is slightly positive
– Other end slightly negative
– Due to uneven distribution of electrons
• Oxygen end – Many protons has stronger hold on electrons– Slight Negative charge
• Hydrogen ends + “naked” protons+ Slight Positive charge Image: PD on wikipedia
http://commons.wikimedia.org/wiki/Image:H2O_(water_molecule).jpg
• Polarity results in Hydrogen bonds forming
– Type of Van der Waals force
– Weak attraction
– Between hydrogen and a negative atom
Image credit: Qwerter, Michal Manas on Wikipedia commons http://en.wikipedia.org/wiki/Image:3D_model_hydrogen_bonds_in_water.jpg
• Hydrogen bonding between water molecules
Image credit: placbo on Flickr
• Cohesion– Attraction
between SAME molecules
– i.e. water & water
Image credit: Mr. Greenjeans on Flickr
http://www.flickr.com/photos/gaylon/298648625/
• Adhesion
– Attraction between different molecules
– Plants use adhesion and capillary
action in Xylem for water transport
Image credit: ShutterSparks on Flickr
http://www.flickr.com/photos/shuttersparks/1413258875/
Image credit: Luc Viatour on wikipedia commons
http://en.wikipedia.org/wiki/Image:Dew_on_a_Equisetum_fluviatile_Luc_Viatour.jpg
• An excellent example of cohesion and adhesion
• Capillary action– Cohesion– Adhesion– (evaporation)
Image credits: http://www.sciencebuddies.org/science-fair-projects/project_ideas/PlantBio_p033.shtml
Goal 2:Distinguish between a solution
and a suspension
Solution
• Solute = substance that dissolves
• Solvent = substance in which solute dissolves
Image credit: Chris 73 on wikipedia
http://en.wikipedia.org/wiki/Image:SaltInWaterSolutionLiquid.jpg
• Solution characteristics– Dissolving– Compounds
separate– Solute does NOT
settle out
Image credit: hundrednorth on Flickr
http://www.flickr.com/photos/100n30th/4821481/
• Suspension– No dissolving /
separation of compounds
– Settling occurs
Image credit: consumatron on Flickr
http://www.flickr.com/photos/consumatron/2514611795/
Goal 3:Explain acidic and basic
solutions
• Hydrogen Ions and hydroxide ions
– Water molecule will separate to form ions
– pH scale measures H+ ion presence
– Copy equation on pg 42 to see why a water molecule forms one of each ion.
• Hydrogen (H+) ions are associated with acids– Recognize acids by the “H” found in the
compound (often found at beginning or end of chemical formula)
H2SO4
HNO3
H3PO4 HCl
• Hydroxide ions (OH-) are associated with bases– Recognize some bases by the “OH” found in
the compound (other bases steal a “H+” from water and leave behind an “OH-” group)
KOH
Ba(OH)2
NaOH
Ca(OH)2
• Acids– Release hydrogen
ions H+ in solution– Concentration of H+
is high– pH 0 – 7– acidic
Image credit: Lou FCD on Flickr
http://www.flickr.com/photos/loufcd/2870399185/
• Bases– Produces OH- in
solution– Less H+ ions than
pure water– pH 7- 14– basic
Image credit: Lou FCD on Flickr
http://www.flickr.com/photos/loufcd/2870399185/
Concentration of H+ ions changes by
powers of 10
pH =1 has 10x more than pH = 2
pH = 1 has 100x more than pH = 3
More Less
1 2 3 4 5 6 7 8 9 10 11 12 13 14
• Buffers
– Weak acid or base
– Neutralizes strong acids or bases
– Prevents sudden changes in pH