CHAPTER 5 Water and Seawater

The Water Planet Water covers about 71% of the Earth’s surface. biosphere – Considering the depth and volume, the world’s oceans provide 99% of the biosphere Total Water on Earth 97% = _______________ 2% = ______________ 1% = _____________ Of that ________ = surface water ________= ground water ________= atmosphere The Water Cycle - The Water Planet Chapter 6 Pages 6-2 to 6-4

The Polar Molecule Water is a simple molecule; = The hydrogen atoms bond to the oxygen atoms with a covalent bond.= Water is Polar = Water’s Unique Properties Chapter 6 Pages 6-5 & 6-6

Water molecules in different states of matter Solid= Liquid= Gas= Fig. 5.5

Changes of state due to adding or subtracting heat Temperature= Calorie=

Unusual thermal properties of H2O H2O has high boiling point = H2O has high freezing point = latent heats of Vaporization/condensation= Melting/freezing=

Fig. 5.6

Unusual thermal properties of H2O Water high heat capacity Amount of heat required to raise the temperature of 1 gram of any substance 1o C Water can take in/lose lots of heat without changing temperature Rocks low heat capacity Rocks quickly change temperature as they gain/lose heat

Global thermostatic effects Moderate temperature on Earth’s surface Equatorial oceans (hot) don’t boil Polar oceans (cold) don’t freeze solid Marine effect Oceans moderate temperature changes day/night; different seasons Continental effect Land areas have greater range of temperatures day/night and during different seasons

Density of water Water is the only substance that Density of water increases as temperature decreases Density of ice is less than density of water From 4oC to 0oC density of water decreases as temperature decreases

Density of water Fig. 5.10

Salinity Total amount of solid material dissolved in water- Traditional definition Typical salinity is 3.5% or 35o/oo or parts per thousand (ppt) = grams of salt per kilogram of waterg/Kg Six elements make up 99% of dissolved solids in seawater Fig. 5.12

The Colligative Properties of Seawater Properties of Pure Water= 1. 2. 3. 4. 5. Colligative properties = Ability to conduct an electrical current. A solution that can do this is called an electrolyte. Decreased heat capacity. Takes less heat to raise the temperature of seawater. Raised boiling point. Seawater boils at a higher temperature than pure fresh water. Decreased freezing temperature. Seawater freezes at a lower temperature than fresh water due to increased salinity. Slowed evaporation. Seawater evaporates more slowly than fresh due to the attraction between ions and water molecules. The Inorganic Chemistry of Water Chapter 6 Pages 6-12 & 6-13

Salinity variations Open ocean salinity 33 to 38 o/oo Coastal areas salinity varies more widely brackish conditions= hypersaline conditions= Salinity may vary with seasons (dry/rain)

Why the Seas Are Salty Source of sea salts = minerals and chemicals on land eroding and dissolving into fresh water flowing into the ocean. Waves and surf appear to contribute by eroding coastal rock. Hydrothermal vents change seawater by adding some materials while removing others. Scientists believe these processes all counterbalance so the average salinity of seawater remains constant. The ocean is said to be in chemical equilibrium. The Inorganic Chemistry of Water Chapter 6 Page 6-17

Processes that add/subtract water from oceans Salinity increases through: Salinity decreases through: Precipitation (rain or snow) Runoff (river flow) Melting icebergs Melting sea ice Evaporation Formation of sea ice

Hydrologic cycle describes recycling of water near Earth’s surface Fig. 5.15

Processes that add/subtract dissolved substances Salinity increases through: Salinity decreases through: Salt spray Chemical reactions at seawater-sea floor interface Biologic interactions Evaporite formation Adsorption River flow Volcanic eruptions Atmosphere Biologic interactions

Residence time and steady state Fig. 5.16

Acidity and Alkalinity pH measures acidity or alkalinity. Pure water = Acids add = Bases add = Acidic solutions have a lot of hydrogen ions, pH value of 0 to less than 7. Solutions that have a lot of hydroxyl ions are considered alkaline. They are also called basic solutions. The pH is 7.1- 14. The Inorganic Chemistry of Water Chapter 6 Pages 6-19 to 6-20

Carbon Cycle The Organic Chemistry of Water Chapter 6 Pages 6-24 & 6-25

Carbonate buffering Keeps ocean pH about same (8.1) pH too high, carbonic acid releases H+ pH too low, bicarbonate combines with H+ Precipitation/dissolution of calcium carbonate CaCO3 buffers ocean pH Oceans can absorb CO2 from atmosphere without much change in pH

Carbonate buffering Fig. 5.18

Surface ocean variation of salinity Polar regions: salinity lower, lots of rain/snow and runoff Mid-latitudes: salinity higher, high rate of evaporation Equator: salinity lower, lots of rain Thus, salinity at surface varies primarily with latitude

Surface ocean variation of salinity Fig. 5.21

Density versus depth Density differences cause a layered ocean Halocline= Thermocline= Pycnocline=

Fig. 5.23

Desalination processes Remove salt from seawater Distillation--most common process Electrolysis Reverse osmosis Freeze separation

Fig. 5.24