Combustion Terminology
_________________________
The process by which cells convert the chemical energy stored in organic molecules (sugars) into energy that cells can use.
_________________________
A chemical reaction that occurs in the presence of oxygen and resulting in the release of energy. Both processes release H2O and CO2
_________________
An organic compound containing only carbon and hydrogen atoms
____________– A substance that releases energy when involved in a chemical reaction (often combustion) or a nuclear reaction
___________ – A substance discharged into the atmosphere or into surface water.
Balancing Chemical Equations
Steps [See Page 156]
1. Balance carbon products 2. Balance hydrogen products 3. Balance oxygen reactants
4. If necessary, make reactant oxygen a whole number by multiplying ALL coefficients by 2.
Oxides of Carbon
________________ – plant matter or agricultural waste from recently living sources used as a fuel or as an energy source.
1. Provide 3 sources of airborne CO2.
2. Describe two carbon sinks (carbon that is removed from the atmosphere and stored)
__________ ____________________ – the ‘capture’ or removal of CO2 from the atmosphere.
__________ ____________________ - a product of the incomplete combustion of a carbon compound.
How can this occur? [Page 158]
Oxides of Sulfur ______________
Once burned, coal can be a source of sulfur
____________
Natural gas that contains greater than 1% hydrogen sulfide.
What is the estimated % of natural gas reserves in Alberta that are sour? [159]
_____________
The release of low quality gas by burning
Which contains less sulfur, coal from Alberta or Eastern coal? [160]
Oxides of Nitrogen
What are the two most common sources of nitrous oxides? [160]
____________ __________
Matter that consists of solids suspended in the atmosphere that comes from natural and human-made sources.
______________________
Summary of Sources of Sulfur and Nitrogen Oxides
Sources of SO2 Sources of NOx
Natural Natural
Hot springs
Volcanic out gassing Forest fires
Human Made Human Made
__________________ power plants
Pulp and paper _______
Refining crude oil Refining oil sands
Refining metals and smelting
Automobiles
Fossil fuel power plants Industrial and home furnaces
Production of ____________
Burning of crops
____________
1.2 THE CHEMISTRY OF ACIDS AND BASES
Empirical Properties of Acids, Bases and Neutral Solutions ________________: a result of an observation
______________ ______________: a solution in which water is the solvent
Apparatus / Test Used to identify an ionic compound, a base or an acid?
Expected Result for a Positive test
Expected Result for a Negative test Conductivity
Meter
Red Litmus Paper Blue Litmus Paper
Magnesium
Solution Red litmus Blue litmus Conductivity Magnesium
HCl HNO3
H2SO4
NaOH Na2CO3
NaCl C6H12O6
Properties of Acids, Bases and Neutral Solutions
Solution Properties
Acid Base Neutral
Types of Deposition
__________________ – industrial emissions that return to the Earth 1. _____deposition
2. ____ deposition
What Makes a Solution Acidic
______________ – the substance whose bonds are broken by a solvent. Acids tend to form _______________ solutions
__________________ – an aqueous solution that conducts an electric current
Acids behave as ________________________, even if their formula suggests that the solute is a molecular compound.
Ionic compound – a chemical substance formed from the mutual attraction of positive and negative _____.
Molecular compound – a chemical substance formed by elements ________ valence electrons.
Dissociation of ionic compounds occurs due to electrostatic attraction between solute and ______
ions
Dissociation – the separation of chemical substances into its individual _____ in a solution
Electrostatic Attraction – a force that acts to ______ oppositely charged objects toward each other.
Arrhenius – proposed that acids contained hydrogen ions [H+
(aq)]and bases contained hydroxide
ions [OH -(aq) ]
Balancing Chemical Equations
CaCl2(aq) Ca2+(aq) + 2Cl-(aq)
n.c = n.c = n.c =
_______________ – the number that is in front of an chemical formula. It indicates the number of moles of the entire formula
_______________ – the superscript behind a ion or polyatomic ion that indicates the charge of the ion
_____________________ - the number of that particular of substance
_____________________ – the total ionic charge of the reactants and products
Na2CO3 (aq) 2Na+(aq) + CO32-(aq)
___________________ –molecular compounds that behave as an ion
Write the balanced equation for the change that occurred with each substance when it was dissolved in water.
a) HCl b) HF c) NaOH c) Na2CO3
BrØnsted – Lowry Acid - Base Reactions
1. Acids dissociate in water. 2. Acids release protons (H+)
3. Protons (H+) bond to water molecules (H 2O)
4. This bond forms a hydronium ion (H3O+)
Acid – a substance that __________ or loses a proton to another substance during a chemical reaction
Base – a substance that accepts or __________a proton from another substance during a chemical reaction
HF(aq) + NH3(aq) F-(aq) + NH4+(l)
Conjugate Acid – an acid __________ in an acid-base reaction when a base accepts or gains a hydrogen ion from another substance
Conjugate Base – a base __________in an acid-base reaction when an acid donates a proton to another substance
Label each part of the following reactions. Complete the reaction when required. H2SO4(aq) + H2O(l) H3O+(aq) + HSO4–(aq)
HCl(aq) + H2O(l)
HNO3(aq) + H2O(l)
1. Strongest Acids are near the top.
2. These will donate a proton to the reactant below it
List the following acids in order of strongest to weakest
HF(aq) H2SO4(aq) HCl(aq) HCO3- (aq) H3PO4(aq) HBb(aq) H3O+ (aq)
Neutralization Reactions
- Reactions that involve acids and bases. These produce a number of products which can include ionic compounds and water.
- The following are 1:1 molar ratios.
HCl (aq) + NaOH (aq)
HCl (aq) + Na2CO3 (aq)
____________– oxygen combining with carbon, sulfur or nitrogen
_____________ – any form of precipitation containing an excess of dissolved acids with a pH of 5.6 or less
_________________ – originating from human activity
Global Sulfur Emissions
The five sources of sulfur emissions are anthropogenic, marine, volcanic, terrestrial and biomass burning.
1. Which is the most common type in the Northern Hemisphere?
pH: a value that represents the concentration of dissolved _________________ ions, H3O+(aq), within a solution
pH Scale
A pH of 7 is considered _______________ A pH of 0 is _____________
A pH of 14 is _________
A pH of 6 has _______ more hydronium ions than a pH of 7 A pH of 5 has ________ more hydronium ions than a pH of 7
Calculation of pH from hydronium concentration
1. Determine the pH of a sample of rainwater that has a hydronium-ion concentration, [H3O+ (aq)], of 1.00 x 10-4 mol/L.
2. A sample of lake water has a hydronium-ion concentration of 2.27 x 10-7 mol/L. Determine the pH of the lake water.
3. Calculate the pH of a sample of water that has a hydronium-ion concentration, [H3O+(aq)], of 1.00 x 10-7 mol/L.
Significant Digits: Special case pH
When writing a pH value the number before the decimal does NOT count as a significant digit.
Only the numbers after the decimal count as significant digits
Calculation of hydronium concentration from pH
1. Calculate the hydronium-ion concentration, [H3O+(aq)] in a shampoo with a pH of 5.72.
2. Calculate the hydronium-ion concentration, [H3O+(aq)] in water with a pH of 7.00.
Practice
1. For each hydronium-ion concentration, calculate the pH. Classify each solution as being acidic, basic or neutral.
a. 0.00100 mol/L b. 2.00 x 10-4 mol/L c. 1.50 x 10-6 mol/L d. 1.35 x 10-4 mol/L e. 1.54 x 10-12 mol/L
2. For each pH value, calculate the hydronium-ion concentration.
a. 7.00 b. 2.98 c. 8.912 d. 13.1
Using pH indicators (Page 12)
Indicators are weak acids.
1. In solution, bromothymol blue is blue. What is the pH range of the solution?
2. In solution, phenolphthalein is colorless. What is the pH range of the solution?
3. In solution, phenol red is red. What is the pH range of the solution?
4. A solution is tested using all of the indicators above. The color changes are as above.
Estimate the pH of the solution?
5. Estimate the hydronium – ion concentration of the solution.
6. In solution, bromocresol green is green. What is the estimated pH range of the solution?
Blending of Indicator Colors
1. Yellow – blue =
2. Red – Yellow =
3. Red – Blue =
Practice: Using pH indicators (Page 12)
1. In solution, litmus is red. What is the pH range of the solution?
2. In solution, thymol blue is orange. What is the pH range of the solution?
3. In solution, orange IV is red. What is the pH range of the solution?
4. A solution is tested using all of the indicators above. The color changes are as above.
Estimate the pH of the solution.
5. Estimate the hydronium – ion concentration of the solution.
Memorization of Common Bases and Acids.
Place the following in order from acidic to basic
Distilled water, bleach, vinegar, stomach acid, baking soda,
Aboriginal uses of indicators
______________: pH range of red (pH 1) to green (pH 13)
Section B1.2 Review
1. Write balanced chemical equations for the reactions between the following substances. For each equation, label the acid, the base, the conjugate acid, and the conjugate base.
a. hydronium ion, H3O+(aq), and hydroxide ion, OH-(aq)
b. ethanoic acid and ammonia
2. Calculate the pH values for each hydronium-ion concentration given. Identify whether the solution is acidic, basic, or neutral.
a. 0.001 25 mol/L b. 2.3 x 10-9 mol/L c. 4.42 x10-13 mol/L d. 5.6 x 10-2 mol/L e. 8.10 x 10-8 mol/L
3. Calculate hydronium-ion concentration for each pH value given. a. 2.14
b. 7.1 c. 9.437 d. 11.00
4. A solution is yellow with thymol blue and blue with bromocresol green. Determine the pH of the solution, then determine the color of the solution using the following indicators.
a. methyl violet b. indigo carmine c. methyl orange d. alizarin yellow R
NAME: _______________________________________ BLOCK: __________ 1.3 The Impact of Acid Deposition on Ecosystems
Sedimentary Rock
- Sedimentary rock includes _____________ gypsum, halite (rock salt) and ______________
- Organic sedimentary rocks are formed by the accumulation of dead plant and animal matter which is then compacted together.
- Sedimentary rock reacts with acids and _______________________
Intrusive Rock
- Intrusive rock is a form of igneous rock which is produced by the hardening of volcanic magma.
- The hardened magma crystallizes into mineral formations which include granite.
- Intrusive rock contains minimal carbonate and therefore _______________________________.
Metamorphic Rock
- Metamorphic rock is a rock in transition between igneous and sedimentary rock.
- This rock has a __________________ to minimize the effects of acids.
The Effects of Prevailing Wind Patterns on Acid Deposition Jet Stream Internet Research
Step 1: Search the Internet for images of daily, monthly, and seasonal patterns of the jet stream. (Website links and within the Website PowerPoint)
Step 2: Draw a line representing an approximate average location for the jet stream across North America.
Step 3: Determine the direction of the winds in areas north and south of the jet stream.
Step 4: Use vector arrows to indicate the direction of the winds on your map for North America and Alberta.
Analysis
1. Define the term jet stream.
2. State the general direction of the jet stream.
3. Explain the effect the jet stream has on weather and climate in western Canada.
4. Comment on the statement, “Wind patterns in Canada and Alberta are always the same.”
5. From your analysis of wind patterns, does Canada’s position in the northern hemisphere ensure that air transported by currents, such as the jet stream, are relatively clean and unpolluted?
Experimental Terminology ______________ Variable
The one part of the experiment that is changed to determine the outcome
______________Variable
The outcome as a result of the manipulated variable
Experimental _____________
Portions of the experiment that are not exposed to the manipulated variable
LAB: Acid Deposition and Its Effect on Simulated Lake Water
Analysis
1. Earlier, you discovered the importance of experimental controls. Identify the cylinders that were experimental controls. Briefly describe their purpose. In some experiments, only one control is used. Why are two control cylinders used in this experiment?
______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________
2. Identify the samples of simulated lake water that were exposed to wet acid deposition, that were exposed to dry acid deposition, and that were not exposed to acid deposition.
______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________
3. Describe the effect that CaCO3(s) had on the simulated lake-water samples. Support your answer using the evidence collected during the experiments and, if possible, a balanced chemical equation.
______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________
4. This demonstration was designed to simulate conditions that could occur in nature. List natural sources of CaCO3(s). Explain how CaCO3(s) could come into contact with lake water to form a chemical system.
______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________ ______________________________________________________________________________
Buffering of Acid Rain
- Limestone contains carbonate [CO32-]
- Carbonate is found in soil and in bodies of water exposed to carbonate
- Carbonate acts as a buffer against the effects of acid rain
Effects of soil composition
Intrusive and metamorphic rocks contain low levels of carbonate. Sedimentary rock contains high levels of carbonate
Which areas of Canada have high buffering capacity? Which areas of Canada have low buffering capacity?
Effects of pH on plants
- Most plants tolerate a small range of pH.
- Soil with a pH below 5.5 reduces available plant nutrients.
- This reduces plant growth.
1. Which plants are best able to withstand acid soil conditions?
2. Which plants are least able to withstand acid soil conditions?
3. Potassium, phosphorous and nitrogen are key ingredients in plant fertilizers. What is the optimum pH that allows these nutrients to be available to plants?
Leaching
- A process during which metals are extracted from soil compounds and released into water.
- Acid rain lowers soil pH and leaches metals such as _____________________________
- Metals are normally found as ionic compounds in the soil. Example: Al(OH)3
- Acid rain causes metals to be released as ions (dissociation).
- These ions are ______________ by plants.
- These ions accumulate in the soil, water and organisms.
Biomagnification
A process that begins with a pollutant accumulating in an organism. A
_________________results in the accumulation of high levels of pollutants in the fat cells of the top consumer
Biomagnification Concentrations
______ -
microgram per gram or 1/1 000 000 of a gram
______ – 1 part per million
What is affected by Acid Rain?
_________ Factors – the living components of an environment
_________ Factors – the physical non-living components of an environment
- _____________________________
- _____________________________
- _____________________________
- _____________________________
Biodiversity
The ____________ of different organisms within an environment
TITRATION LAB:
Chapter 1.4 Quantifying Acid Deposition
_____________Data - a description of a substance that involves a measurement and a numerical magnitude
_____________ – a technique used to determine the concentration of a substance in a solution by adding measured quantities of another substance until an endpoint is reached
Label the Equipment Setup
Indicator Color Change
Phenolphthalein pH range for clear to pink ___________________________
Highlight or circle Key Instructions
1. Get the following pieces of equipment:
Two 50 mL beakers. One 300 mL beaker. One stand and clamp. One biuret.
One 125 mL Erlenmeyer flask One 10.0mL pipette and bulb
2. Label one 50 mL beaker HCl and the other NaOH 3. Label the 250 mL beaker Waste.
4. Set up your equipment as shown in the diagram.
5. Rinse the burette out with the water bottle. Drain into the sink. Repeat. Use the twirl method.
6. Add a small amount of NaOH to the burette. Twirl. Drain into the waste beaker.
7. Place the burette in the clamp as shown in the diagram.
8. Using a funnel, add NaOH into the Burette up to or slightly below the 0.00 mL mark. Record this amount in Table 1. (Next Page)
9. Further trials will NOT require adding NaOH. Simply read the meniscus as your initial reading.
10.Rinse the Erlenmeyer flask with the wash bottle. 11.Add 10.0 mL of HCl to the
Erlenmeyer flask. See the diagram.
12.Add 3 drops of
Phenolphthalein to the Erlenmeyer flask.
13.Place the Erlenmeyer flask on a white piece of paper. 14.Place the flask underneath
the burette nozzle.
15.Swirl!
16.Record final NaOH burette reading in Table 1. Table: 1 Volume of Standard Solution (mL)
Trial InitialVolume of Standard Solution (mL)Final Amount Added
1.
2.
3.
4.
5.
AVERAGE AMOUNT OF
NaOH
17. Pour the Erlenmeyer flask contents into the waste beaker. Rinse the Erlenmeyer flask with the water bottle.
18. Repeat trials (Steps 9 – 16). Meniscus Reading Practice.
Strong and Weak Acids
Strong acids ______________________, producing a maximum number of
hydronium [H3O]+ ions.
These are often used as standard solutions in titration's
Weak acids _____________ completely dissociate.
Strong and weak acids can be determined by reactions with bases.
Equal volumes of strong acids require more moles of base
CAVA = CBVB
Acid
C
A= ?
V
A= 10.0 mL
NaOH – standard solution
C
B= [ ] mol/L label
V
B= [ ] from the titration
C
A= C
BV
BV
AWeak acids require less moles.
A strong acid does ________ necessarily produce a low pH
A small amount of a strong acid in water may only produce a __________________ in pH. A large amount of weak acid can cause the pH to become _________________.
Question: Which is the stronger acid?
a. A solution of HCl(aq) with a pH of 6 b. A solution of H2SO3 (aq) with a pH of 3
Chapter 1.5 Reducing Acid Deposition
___________________ were originally used to reduce local acid deposition. Was this an effective solution? Why?
Fly Ash -
_________________________ of sand and other unburned material that remain suspended in the exhaust gases when pulverized
__________________________
Current Solutions Solution # 1. _______________
________________– a device that uses electric fields to collect fly ash from emissions.
Solution #2. .________________ – a process used to remove one or more components from a mixture of gases by passing it through substances that absorb and separate unwanted
components
_____________________
– a substance used in a chemical process that increases the speed of the reaction is not affected by the process.
Solution # 3.
______________ ____________
- An emission control device used to remove NOx, CO
and hydrocarbons from vehicle exhaust.
_________________________ - the lowest region of
the atmosphere that extends to approximately 18 km
above Earth’s surface; the region of the atmosphere where all weather occurs.
__________________________ – a brownish-red
haze produced by the reaction of UV and the components in combustion. 1.
The production of NO is ___________ released through engine exhaust. 2. The second reaction requires _____ later in the day.
3. The production of ozone occurs ______.
Solution # 4.
______________ – adding a basic compound to soil or a body of water to neutralize acid deposition
Solution # 5
Green and Semi Green Energies
1. ‘Green’ Energy Sources –
2. ‘Semi Green’ Energy Sources –
Solution # 6
