<p>UNIT 1-C INVESTIGATING THE CAUSE OF THE FISH KILL Section C.1 1. Define solubility - THE MAXIMUM AMOUNT OF SOLUTE THAT WILL DISSOLVE IN A GIVEN AMOUNT OF SOLVENT – AT A GIVEN TEMPERATURE. - EX. – SUGAR IN WATER AT 25C – SOLUBILITY IS 15g SUGAR / 100 g WATER</p><p>2. List the two factors that do not effect how much of a substance can dissolve? </p><p>- EVERYTHING DISSOLVES TO SOME EXTENT - THINGS THAT READILY DISSOLVE = SOLUBLE - THINGS THAT HARDLY DISSOLVE AT ALL = INSOLUBLE</p><p>3. Define saturated, unsaturated, and supersaturated solutions - SATURATED = THE SOLVENT HOLDS AS MUCH SOLUTE AS IT CAN - UNSATURATED = SOLVENT CAN HOLD MORE SOLUTE - SUPERSATURATED = UNSTABLE SITUATION CREATED WHERE SOLVENT HOLDS MORE SOLUTE THAN IT SHOULD</p><p>4. Know how to interpret data from a SOLUBILITY CURVE – Some help on Your Turn pg. 44 – (use figure 18, pg.42)</p><p>- What is the solubility of KNO3 at 80C? - At what temperature will the solubility of dissolved oxygen be 10 mg / 1000 mg of water ?</p><p>- How much KNO3 will dissolve in 200 g of water at 80C?</p><p>5. If you have a horizontal line of solubility what does that show for the substance graphed? </p><p>6. A solubility line with a steep incline tells you what about the relationship of the solute to water? </p><p>7. Each point plotted on the solubility line tells you what about that substance? </p><p>8. What do points below the line show? </p><p>9. Where on a solubility graph would you find a supersaturated solution? </p><p>10. What will happen to the solubility of a solid in water when the temperature of the water is lowered? </p><p>11. In contrast, what will happen to the solubility of a GAS when the temperature of the water is lowered?</p><p>12. List the two factors that a GAS’S solubility is dependent on? SECTION C.2 Concentration – a quantitative measurement of solute in a certain amount of solvent EXAMPLE – the concentration of sugar in a water solution – given in PERCENT SOLUTION = </p><p>( g solute / g solution) x 100</p><p>- PERCENT SOLUTION also called pph - Can also have ppt, and ppm solution concentrations</p><p>1) Another way to tell the concentration of a solution is by using percentage. What would be the % concentration of a solution containing 10 grams of salt dissolved in 90 grams of water? What would the concentration be in pph? In ppt? In ppm?</p><p>2) The concentration of seawater is 3g salt/100g of salt water. What is its concentration in pph. Show work and units______</p><p>3) At 26 °C water is saturated with oxygen when 8 mg(.008grams) of oxygen is dissolved in 1000g of water. What is the concentration of oxygen in ppm? Show work______</p><p>4) At 20 °C 1000g of water must have 5.4 mg or .0054g of Oxygen for fish to survive. Calculate this concentration in ppm. Show work and units 5) A solution which has .00005 g of lead ion dissolved in 1000g of water is considered dangerous to human health. Calculate the concentration in ppm Show work and units C.3 – OXYGEN What do aquatic organisms need to survive? </p><p>What interferes with the oxygen supply to aquatic organisms? </p><p>Describe how oxygen dissolves in water. </p><p>Describe photosynthesis. </p><p>List the photosynthesis equation.</p><p>What is the name of the oxygen - consuming bacteria that aquatic organisms compete with? </p><p>What do these organisms feed on? </p><p>When are aquatic creatures at risk? </p><p>Define DO. </p><p>The amount of dissolved oxygen that fish needs is? </p><p>Some fish require more oxygen than others What sort of water does trout live in? What sort of water do catfish live in? C.3 – OXYGEN - Every animal requires O2 for Aerobic respiration - Organisms that live in water get O2 dissolved in water, NOT the O in H2O - 3 ways O2 can become dissolved in the H2O - Direct contact w/ the atmosphere - Aeration – water “churned w/ air” - Photosynthesis of aquatic plants</p><p>6CO2 + 6H2O C6H12O6 + 6O2</p><p>- Aerobic bacteria use up O2 - Live off of wastes – natural or otherwise - Lots of “food” for bacteria = population explosion - Less O2 for other aquatic animals</p><p>- Dissolved Oxygen levels below 4 ppm = fishies die</p><p>C.4 – TEMPERATURE AND SOLUBILITY OF GASES - High temperatures = increased metabolism of fishies - Increased metabolism = more O2 use - Lower temperatures = decreased metabolism - Decreased metabolism = less O2 use - O2 gas solubility decreases at higher temperatures - Fish kills often happen in the summer! - High water temperature can be caused naturally – or by man – thermal pollution C.4 – TEMPERATURE AND SOLUBILITY OF GASES</p><p>As water temperature INCREASES, what happens to the solubility of gases?</p><p>Besides temperature, what other factor effects the solubility of gases?</p><p>If the temperature of the water increased 10 C what happens to chemical reactions of the fish? </p><p>Explain the purpose of refrigeration.</p><p>When water temperatures increase what happens to the temperature of the fish? </p><p>If the temperature of the water is raised, the fish's chemical reactions are what?</p><p>The fish now require what, since the temperature of the water is increased? </p><p>Consider aerobic bacteria, what effect does raising the temperature of water have on aerobic bacteria? </p><p>Explain what causes a fish kill after a warm spell. </p><p>What type of pollution would explain a raise in water temperature in Snake River? C.6 – ACID CONTAMINATION</p><p>ACIDS - Usually have a H+ that can be easily released into solution - H usually written first (i.e. HCl, H2SO4, H3PO4, HC2H3O2, H2CO3, HNO3) - Examples of uses ?</p><p>BASES - Usually have an OH- that can be easily released into solution - OH usually written last (i.e. NaOH, Ca(OH)2, Mg(OH)2, KOH) - Examples of uses?</p><p>- ACIDS and BASES can get together to make neutral solutions pH SCALE –tells us how to classify substances as ACIDIC, BASIC, or NEUTRAL</p><p> pH SCALE goes from 0 – 14 0 – 7 = ACIDIC 7 = NEUTRAL 7 – 14 = BASIC</p><p>Q. Where does ACID RAIN come from?</p><p>Q. Guess what area of the US is responsible for the majority of the ACID RAIN contamination of water sources in Canada? C.7 – IONS & IONIC COMPOUNDS Atoms that are charged are called ?</p><p>What are + ions called?</p><p>What are – ions called?</p><p>What do you get when you put positive ions and negative ions together to have a net charge of 0?</p><p>When we write formulas for IONIC COMPOUNDS, we always write the cations first, and anions last Example – NaCl CaCl2</p><p>When we name IONIC COMPOUNDS – 1. name the cation just like the element 2. drop the last few letters of the anion and add “ide” ending Example NaCl = Sodium Chloride CaCl2 = Calcium Chloride HF = ? KBr = ? Na2S = ?</p><p>2- Q. - What do we call these funky ions like (SO4) ? C.8 – DISSOLVING IONIC COMPOUNDS</p><p>Q. What must happen in order for ionic substances to dissolve in a particular solvent?</p><p>Q. What is it about water that makes it able to dissolve so many things?</p><p>C.9 – HEAVY METAL IONS Q. – What are the primary essential metals (minerals)?</p><p>Q. – What are the primary “heavy metals”?</p><p>Q. – What do these heavy metals do in our bodies?</p><p>Q. – What are some biological effects of metal poisoning? Q. – How do the heavy metals get into our water ?</p><p>LEAD</p><p>Q. – Where did the symbol for lead come from?</p><p>Q. - What are some of it’s uses?</p><p>Q. – How might lead have contributed to the fall of the Roman Empire?</p><p>Q. – What is the primary way urban children are exposed to Pb? MERCURY</p><p>Q. – Where did the symbol for mercury come from?</p><p>Q. – What are some of it’s uses?</p><p>Q. – What physical form of mercury is most dangerous?</p><p>+ Q. – Where does the highly toxic (CH3Hg) come from?</p><p>Q. – Where do you think the term “Mad as a Hatter” comes from? </p><p>CADMIUM</p><p>Q. – What are some of it’s primary uses?</p><p>Q. – What sort of biological damage does it cause?</p><p>Q. - What is the primary way Cd enters the body? Is it then excreted? C.11 – MOLECULAR SUBSTANCES</p><p>- There are 2 major types of compounds - IONIC – held together by (+) and (–) charged particles attracted to one another (i.e. NaCl) - MOLECULAR – held together by the sharing of electrons (i.e. H2O) - There are 2 major types of MOLECULAR COMPOUNDS - POLAR – unequal sharing of electrons (i.e. CH3OH) - NON-POLAR - equal sharing of electrons (i.e. N2)</p><p>Q. – What is one simple rule that can be used to determine the solubility of solutes in solvents? </p>