WATER SECTION A Reading Guide

Name______

Date______Period____

A.1 : Measurement and the Metric System

A.2: Foul Water Lab Activity

  1. Know what each of the 3 separation methods are supposed to remove from water
  2. Know what types of things ARE NOT removed via the separation methods we used
  3. Know how distillation works, and what it removes from water

A.3: Water Diary Data Collection

A.4: Water and Health

  1. How many days can you live without food?
  1. How many days can you live without water?
  1. How many liters of water do you need on a daily basis?
  1. “Back in the day”, you could drink from the river. Can you now? Why?
  1. If you had a choice, would you drink from a lake, river, stream, rainwater, or groundwater from a well? Why?
  1. What types of things are associated with “dirty water”?
  1. What do we do to our water before we drink it?

A.5 – Water Uses

  1. Remember the WATER CYCLE?
  2. Evaporation -
  3. Condensation -
  1. How does water use and availability differ between regions of the U.S.? Why are there Regional Differences between the East and the West?
  1. How much water does an average family use per day?
  1. Direct water use –
  1. Indirect water use -

A.6 – BACK THROUGH THE PIPES

  1. Where does the water from your pipes come from originally?
  1. Know difference between surface water, ground water,& aquifers
  1. What is the difference between municipal water supplies and well water?
  1. What is the difference between the HYDROLOGIC CYCLE and the WATER CYCLE?

A.7 – WHERE IS EARTH’S WATER

  1. Draw a pie graph (or other “pictogram”) to illustrate where the water is located on our planet. Include the categories: Oceans, Glaciers & Icecaps, Groundwater, and Lakes / rivers / the atmosphere.
  1. Of the water sources shown above, which ones are usable for human consumption?
  1. Is there enough usable water to go around for all of us?
  1. The three states of water (and matter in general) :

Solids -

Liquids -

Gases -

(THIS INFORMATION IS NOT IN YOUR BOOK DIRECTLY – BUT GIVE IT A SHOT IF YOU KNOW ANY OF IT ON YOUR OWN)

  1. How do these 3 states of matter differ structurally on the molecular level? (Pictures are nice)
  1. How do these 3 states of matter differ in terms of the amount of relative Kinetic Energy they contain? (Pictures are nice again!)

WATER UNIT SECTION B Reading Guide

Name______

Date______Period____

B.1 Physical Properties of Water (pg. 22-24)

  1. Describe and give an example of a Physical Property.
  1. What percentage of the earth is covered with water?
  1. List seven physical properties of water.
  1. Define density
  1. Rank gases, liquids and solids by density
  1. Why does ice float?
  1. What would happen to bodies of lakes and oceans...if ice did not float?
  1. Name the property that causes water erosion.
  1. Define evaporation.
  1. At what temperature does evaporation occur?
  1. What makes water liquid at normal temperatures?
  1. Describe surface tension.
B.2: Mixtures and Solutions (pg. 25-26)

Define and give an example of the following terms:

1.Mixture -

2.Heterogenous -

3.Homogenous -

4.How are water mixtures classified?

Define and give an example of the following terms:

  1. Solutions -
  1. Colloids -
  1. Suspensions –
  1. Solute –
  1. Solvent -
  1. List the three particle sizes in water mixtures in order of decreasing size.
  1. What is an aqueous solution?
  1. Describe the Tyndall effect.
B.3: Mixtures Lab(pg.26-28)
B.4: Molecular View of Water (pg. 28-29)
  1. There are approximately ______know elements found in nature.

Define and give an example of the following terms

  1. Atoms –
  1. Elements –
  1. Compounds –
  1. Molecules –
  1. Chemical bond –
B.5: Symbols, Formulas, and Equations (pg. 30-31)

Define and give an example of the following terms:

  1. Symbols -
  1. Chemical formulas –
  1. Subscripts –
  2. CO2 = _____ CARBON ATOMS

______OXYGEN ATOMS

  1. Coefficients –
  2. Chemical Equations -
  1. Reactants –
  1. Products –
  1. The Law of Conservation of Matter –
B.6: The Electrical Nature of Water (pg. 31-33)
1.What evidence do you have that elements or atoms have the potential to conduct electricity?

The three basic parts to ANY atom:

PARTICLE / LOCATION / CHARGE / RELATIVE MASS
Proton
Electron
Neutron
  1. Ions –
  2. Cations
  3. Anions
  1. What happens when you get two oppositely charged forces together?
  1. Ionic Compounds –
  1. Polar Compounds –
  • Non – Polar Covalent Molecules -
  • Polar Covalent Molecules -
B.7: Pure and Impure Water (pg. 33-34)
B.8: Water Testing Lab (pg. 34-37)
  1. Precipitate –
  1. Qualitative Test –
  1. Quantitative Test –
  1. Confirming Test –
  1. Reference –
  1. Control –

WATER UNIT SECTION C Reading Guide

Name______

Date______Period____

Section C.1: Solubility

  • Define Solubility –
  • List the factors that do NOT effect how much of a substance can dissolve.
  • List the factors that doeffect how much of a substance can dissolve.
  • Define saturated, unsaturated, and supersaturated solutions
  • Know how to interpret data from a solubility curve

a. If you have a horizontal line of solubility what does that show for the substance graphed?

b. A solubility line with a steep incline tells you what about the relationship of the solute to water?

c. Each point plotted on the solubility line tells you what about that substance?

d. What do points below the line show?

e. Where on a solubility graph would you find a supersaturated solution?

  • What will happen to the Solubility of a Solid in water when the temperature of the water is lowered?
  • In contrast, what will happen to the solubility of a GAS when the temperature of the water is lowered?
  • List the two factors that a gas’s solubility is dependent upon.

Section C.2

  • Know how to express Concentration of solutions in various units:
  • Percent solution (%)
  • pph (parts per hundred)
  • ppt (parts per thousand)
  • ppm (parts per million)

PERCENT SOLUTION = ( g solute / g solution) x 100

a) 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?

b) The concentration of seawater is 3g salt/100g of salt water. What is its concentration in pph.

c) At 26 °C water is saturated with oxygen when 8 mg (0.008grams) of oxygen is dissolved in 1000g of water. What is the concentration of oxygen in ppm?

d) At 20 °C 1000g of water must have 5.4 mg or .0054g of Oxygen for fish to survive. Calculate this concentration in ppm.

e) 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.

Section C.3 – OXYGEN

  • What do all aquatic organisms need to survive?
  • What interferes with the oxygen supply to aquatic organisms?
  • Describe 3 ways oxygen dissolves in water.
  • Describe photosynthesis.
  • List the photosynthesis equation.
  • What is the name of the oxygen - consuming bacteria that aquatic organisms compete with?
  • What do these organisms feed on?
  • When are aquatic creatures at risk?
  • Define DO.
  • How much dissolved oxygen do fish need?
  • Some fish require more oxygen than others…
  • What sort of water does trout live in?
  • What sort of water do catfish live in?

SECTION C.4 – Temperature and solubility of gases

  • Explain the purpose of refrigeration
  • What happens to the oxygen content of water if the temperature of the water increases?
  • If the temperature of the water is raised, what happens to the metabolism of fish?
  • Consider aerobic bacteria, what effect does raising the temperature of water have on aerobic bacteria?
  • Explain what causes a fish kill after a warm spell.
  • What type of pollution would explain a raise in water temperature in Snake River?

C.6 – ACID CONTAMINATION

  • What ion do acids generally release into solution?
  • What are the “BIG FIVE” Common Acids?
  • What ion do bases generally release into solution?
  • What are the “BIG FOUR” Common Bases?
  • What happens when you get an acid together with a base?
  • On the pH scale, what is considered acidic? What is considered basic? What is considered neutral?
  • Where does ACID RAIN come from?
  • Guess what area of the US is responsible for the majority of the ACID RAIN contamination of water sources in Canada?

Section C.7 – IONS & IONIC COMPOUNDS

  • Atoms that are charged are called ?
  • What are + ions called?
  • What are – ions called?
  • How do we write the correct formula for an ionic compound?
  • Write correct formulas for what you get when you:

a)get Na+ ions together with Cl- ions

b)get Ca2+ ions together with Cl- ions

c)get Ca2+ ions together with O2- ions

  • How do we correctly nameionic compounds?

Name the following:

NaCl CaCl2HFKBr Na2S

  • What do we call these funky ions like (SO4)2- ?

C.8 – DISSOLVING IONIC COMPOUNDS

  • What must happen in order for ionic substances to dissolve in a particular solvent?
  • What is it about water that makes it able to dissolve so many things?

C.9 – HEAVY METAL IONS

  • What are the primary essential metals (minerals)?
  • What are the primary “heavy metals”?
  • What do these heavy metals do in our bodies?
  • What are some biological effects of metal poisoning?
  • How do the heavy metals get into our water ?

LEAD

  • Where did the symbol for lead come from?
  • What are some of it’s uses?
  • How might lead have contributed to the fall of the Roman Empire?
  • What is the primary way urban children are exposed to Pb?

MERCURY

  • Where did the symbol for mercury come from?
  • What are some of it’s uses?
  • What physical form of mercury is most dangerous?
  • Where does the highly toxic (CH3Hg)+ come from?
  • Where do you think the term “Mad as a Hatter” comes from?

CADMIUM

  • What are some of it’s primary uses?
  • What sort of biological damage does it cause?
  • What is the primary way Cd enters the body? Is it then excreted?

C.11 – MOLECULAR SUBSTANCES

  • What are the 2 major types of compounds (ways atoms can bond together)?
  • Give an example of each type.
  • How are these two types of bonding different?
  • What are the 2 major types of molecular (covalent) compounds?
  • How are these two types of molecular bonding different?
  • Give an example of each type.

What is one simple rule that can be used to determine the solubility of solutes in solvents?

WATER UNIT SECTION D Reading Guide

WATER PURIFICATION AND TREATMENT

Name______

Date______Period____

D.1: Natural Water Purification

D.2: Water Softening Lab

D.3: Hard Water and Water Softening

D.4: Municipal Water Purification

D.5: Chlorine in Our Water

D.6: You Decide: Chlorination and THMS Activity

  1. Describe the hydrologic cycle.
  2. What are nature’s purest forms of water?
  3. What is contained in natures purest forms of
    water?
  4. Describe the steps in which natures purest
    forms of water lose their relative purity?
  5. What does gravel and sand remove in the
    ground?
  6. List and describe natures three basic steps in
    purifying water.
  7. What is, the best source of "pure" water?
  8. What conditions allow ground water to pick up
    too high a concentration of dissolved minerals?
  9. Hard water contains an excess of which ions?

D.3 HARD WATER AND WATER SOFTENING

  1. What are the classifications of water
    samples?
  1. If you boil water that has HCO3- what forms?
  1. What can be added to water to remove
    calcium, magnesium, and iron III ions?

4.What problems do synthetic detergents
cause?

5. Which ions contribute to algae growth?

6. What products in your home may contribute
to algae growth?

7. Describe a water softener.

8. When water is hard it will not do what?

9. Define water softening.

D.4 – Municipal Water Purification

Pre-Use Water Treatment

Post-Use Sewage Treatment