1. The Water Planet
Water covers about 71% of the Earth’s surface. Considering the depth and volume, the world’s oceans provide more than 99% of the biosphere – the habitable space on Earth.

2. The vast majority of water on Earth can’t be used directly for drinking, irrigation, or industry because it’s salt water.
This becomes a major political issue
But, the sea provides many other resources such as food, transport by shipping, oil and gas, and recreation.
As big as the ocean is, it’s not always big enough. This has lead to wars
Rivers do not always go where people want them to or people downstream dispute the use of water by people upstream. It’s easy to recognize that if a group upstream pollutes a river or diverts its flow, those downstream may suffer. This is happening in Egypt and Ca.

3. Humans primarily need fresh water
Humans primarily need fresh water. There’s just not as much as we’d like, and not all the sources are accessible.
Plenty of water exists at the poles but it’s frozen and located far from population centers.
We can condense water vapor from the atmosphere by artificial means, but only at an astounding cost.
Most of the fresh water we rely on comes from underground aquifers and rivers

4. As the population increases, so does the need for water.
Part of the solution to meeting this demand lies in understanding what water is, where it goes, and how it cycles through nature.
From the POV of sea life, the oceans are vast. 71% only accounts for the surface area that water covers. When you consider depth and volume, the world’s oceans provide more than 99% of the biosphere – the habitable space on Earth.
On land the habitable space comprises the ground, a few
feet or meters below ground, and rarely more than 30 meters (98 feet) above ground in trees.

5. Some birds and insects fly high in the air, but they do not live there
Some birds and insects fly high in the air, but they do not live there. This is why much of the atmosphere isn’t considered part of the biosphere.
Many whales, fish, and other organisms live midwater, seldom, if ever, nearing the bottom or the shore.
Hydrothermal vents shoot hot, mineral- rich water into the ocean, providing flourishing habitats in the deepest parts of the sea. This makes the entire ocean, which averages 3,730 meters (12,238 feet) deep, part of the biosphere.
While humans need fresh water for drinking, bathing, agriculture, and industry, the oceans provide resources for most life, including human life.

6. The deepest known point in any ocean is the Challenger Deep in the Mariana Trench.
At 10,838 meters (35,558 feet), it’s so deep that if you put Mt. Everest into it, the top would still be more than 1,990 meters (6,527 feet) under water.
This depth creates water pressure of an amazing 8 tons per square inch. That’s about the weight of four automobiles pressing down on an area the size of a typical postage stamp.
The world’s oceans hold more than 1.18 trillion cubic kilometers (285 million cubic miles).

7. The Polar Molecule
Water is a simple molecule; the way it’s held together gives it unique properties.
The hydrogen atoms bond to the oxygen atoms with a covalent bond.
A covalent bond is formed by atoms sharing electrons. This makes water a very stable molecule.

8. A molecule with positive and negative charged ends as polarity and is called a polar molecule.
The water molecule’s polarity allows it to bond with adjacent water molecules.
The positively charged hydrogen end of one water molecule attracts the negatively charged oxygen end of another water molecule.
This bond between water molecules is called a hydrogen bond.

10. The Effects of Hydrogen Bonds
Being a polar molecule, water has these characteristics:
Liquid Water. The most important characteristics of the hydrogen bonds is the ability to make water a liquid at room temperature. Without them, water would be a gas.
Cohesion/Adhesion. Because hydrogen bonds attract water molecules to each other, they tend to stick together. This is cohesion. Water also sticks to other materials due to its polar nature. This is adhesion.

11. Viscosity. This is the tendency for a fluid to resist flow
Viscosity. This is the tendency for a fluid to resist flow. The colder water gets, the more viscous it becomes. It takes more energy for organisms to move through it, and drifting organisms use less energy to keep from sinking.
Surface Tension. A skin-like
surface formed due to the
polar nature of water.
Surface tension is
water’s resistance to objects
attempting to penetrate its
surface.

12. The Effects of Hydrogen Bonds (continued)
Ice Floats: as water cools enough to turn from a liquid into solid ice, the hydrogen bonds spread the molecules into a crystal structure that takes up more space than liquid water, so it floats.
If ice sank, the oceans would be entirely frozen – or at least substantially cooler – because water would not be able to retain as much heat.
The Earth’s climate would be colder – perhaps too cold for life.

13. More visual examples http://www.johnkyrk.com/H2O.html

14. Solutions and Mixtures in Water
A _______ occurs when the molecules of one substance are homogeneously dispersed among the molecules of another substance.
A _______ occurs when two or more substances closely intermingle, yet retain their individuality.

15. Solutions They are made up of 2 parts
Solvent = _______ _______ _______ _______ _______ _______ _______ _______.
Water is a very good solvent due to its polar property
Solute = _______ _______ _______ _______ _______ _______ _______ _______ _______ _______ _______ The molecules of the solute are homogenously dispersed throughout the solvent

16. _______ - homogeneous mixture
_______ - substance being dissolved
_______ - present in greater amount

17. The dissolving (also known as solvation) can occur through:
Dissociation
Nonionic solutions
H-bonds to can occur with some nonpolar compound

18. Mixtures A mixture is generally heterogeneous
The individual particles are easy to see or they settle out and become easier to see.

19. Salts and Salinity
_______ includes the total quantity of all dissolved inorganic solids in seawater.
_______ _______(rock salt or halite) is the most common and abundant sea salt.
It is not the only one. It includes things such as KCl
Scientist’s measure salinity in various ways
expressed in parts per thousand (‰).
Most commonly used because small variation are significant
_______ _______ _______ _______
_______

20. The ocean’s salinity varies from near zero at river mouths to more than _______ in confined, arid regions (_______ _______ _______).
The proportion of the different dissolved salts never change, only the relative amount of water.
The salinity changes when fresh water enters the ocean – such as from a river or from rain – or as water evaporates. For instance, _______ _______ results when fresh water mixes with seawater in estuaries. Brackish water has a salinity of 0.6‰ to 30‰.

21. The salinity of the oceans changes some of water’s physical properties
_______, which is water saturated or nearly saturated with dissolved salt, develops in areas with high evaporation and little inflow of fresh water or where salt domes dissolve at the seafloor, as is common in the Gulf of Mexico.
The salinity of the oceans changes some of water’s physical properties
_______ _______ _______ _______ _______ _______ _______ _______

22. The Colligative Properties of Seawater
_______ _______ are properties of a liquid that may be altered by the presence of a solute and are associated primarily with seawater. Pure water doesn’t have colligative properties. Fresh water, with some solutes, can have _______ _______ to some degree.

23. The colligative properties of seawater include:
Pure water doesn’t have anything dissolved in it, it does not have colligative properties. Colligative properties are associated primarily with seawater.
natural fresh water usually has some quantity of solutes, and can have colligative properties to some degree. The strength of the colligative properties depends on the quantity (concentration) of the solute.
The colligative properties of seawater include:
_______ _______ _______ _______. A solution that can do this is called an electrolyte.
_______ _______ _______ _______ _______. Takes less heat to raise the temperature of seawater.
_______ _______ _______ _______. Seawater boils at a higher temperature than pure fresh water.

24. Decreased freezing temperature
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.
Ability to create osmotic pressure. Liquids flow or diffuse from areas of high concentration to areas of low concentration until the concentration equalizes. Osmosis occurs when this happens through a semi-permeable membrane, such as a cell wall. Because it contains dissolved salts, water in seawater exists in lower concentration than in fresh water.

25. Types Applications salting icy roads making ice cream antifreeze
cars (-64°C to 136°C)
fish & insects

26. The Principle of Constant Proportions
In seawater no matter how much the salinity varies, the proportions of several key inorganic elements and compounds do not change. Only the amount of water and salinity changes.
This constant relationship of proportions in seawater is called the principle of constant proportions.
Almost every known, naturally occurring element, and some man-made ones, exist in the oceans
This principle does not apply to everything dissolved in seawater – only the dissolved salts.
Dissolved salts are called conservative constituents

27. Dissolved Solids in Seawater
Next to hydrogen and oxygen, chloride and sodium are the most abundant chemicals in seawater.

28. Determining Salinity, Temperature, and Depth
If you know how much you have of any one seawater chemical, you can figure out the salinity using the principle of constant proportions.
Chloride accounts for 55.04% of dissolved solids – determining a sample’s chlorinity is relatively easy.
The formula for determining salinity is based on the chloride compounds:
salinity ‰ = x chlorinity ‰
Sample of seawater is tested at 19.2‰ chlorinity:
salinity ‰ = x 19.2‰
salinity ‰ = 34.68‰

29. Most commonly, salinity is determined with a salinometer
Most commonly, salinity is determined with a salinometer. This device determines chlorinity and calculates the salinity based on the water’s electrical conductivity. It is accurate.

30. The primary tool to measure the properties of seawater is the conductivity, temperature, and depth (CTD) sensor. The CTD profiles temperature and salinity with depth.

31. Another less accurate way to determine salinity is with a refractometer.

32. Why the Seas Are Salty
A source of sea salts appears to be minerals and chemicals 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 _______ _______.

34. Salinity, Temperature, and Water Density
Although the ocean’s average salinity is about 35‰, it isn’t uniform.
Precipitation and evaporation have opposite effects on salinity.
Rainfall decreases salinity by adding fresh water.
Evaporation increases salinity by removing fresh water.
Freshwater input from rivers lowers salinity.
Abundant river input and low evaporation results in salinities well below average.

35. Salinity and temperature also vary with depth.
Density differences causes water to separate into layers.
High-density water lies beneath low-density water.
Water’s density is the result of its temperature and salinity characteristics:
Low temperature and high salinity are features of high-density water.

36. Relatively warm, low-density surface waters are separated from cool, high-density deep waters by the thermocline, the zone in which temperature changes rapidly with depth.
Salinity differences overlap temperature differences and the transition from low-salinity surface waters to high-salinity deep waters is known as the halocline.
The thermocline and halocline together make the pynocline, the zone in which density increases with increasing depth.

37. Salinity, Temperature, and Water Density (continued)

38. Acidity and Alkalinity
pH measures acidity or alkalinity.
Seawater is affected by solutes. The relative concentration of positively charged hydrogen ions and negatively charged hydroxyl ions determines the water’s acidity or alkalinity.
It can be written like this:

39. Acidic solutions have a lot of hydrogen ions, it is considered an acid with a 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 higher than 7, with anything over 9 considered a concentrated alkaline solution.

40. Acidity and Alkalinity (continued)
Seawater is fairly stable, but pH changes with depth because the amount of carbon dioxide tends to vary with depth.
Shallow depths have less carbon dioxide with a pH around 8.5.
This depth has greatest density of photosynthetic organisms which use the carbon dioxide, making the water slightly less acidic.

41. Middle depths have more carbon dioxide and the water is slightly more acidic with a lower pH.
More carbon dioxide present from the respiration of marine animals and other organisms, which makes water somewhat more acidic with a lower pH.
Deep water is more acidic with no photosynthesis to remove the carbon dioxide.
At this depth there is less organic activity, which results in a decrease in respiration and carbon dioxide. Mid-level seawater tends to be more alkaline.
At 3,000 meters (9,843 feet) and deeper, the water becomes more acidic again.
This is because the decay of sinking organic material produces carbon dioxide, and there are no photosynthetic organisms to remove it.