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56 Cards in this Set
- Front
- Back
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Arrhenius definition of acids |
Acids dissociate in water to form hydrogen ions (H⁺) and anions |
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Arrhenius definition of bases |
Bases dissociate in water to form hydroxide ions (OH⁻) and cations |
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Bonsted Lowry definition of acids |
acids are proton donors |
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Bronsted Lowry definition of bases |
bases are proton acceptors |
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*Know conjugate acid-base pairs |
they differ by only 1 proton an acid has a conjugate base a base had a conjugate acid |
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amphiphrotic |
substance that can act as a bronsted lowry acid and base (ie water) |
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alkalis |
soluble bases that neutralize acids to produce water when dissolved in water, they form OH⁻ ions (ie metal oxides and hydroxides, ammonia, soluble carbonates and hydrogen carbonates |
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salt |
ionic compounds formed when hydrogen of an acid is replaced by a metal or another positive ion formed by reaction of acid with metals or bases |
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acid + metal → |
salt + hydrogen gas |
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spectator ions |
species that are not changed |
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acid + base → |
salt + water |
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neutralization reaction |
acid + base reaction represented by the net equation: H⁺+ OH⁻ → H₂O exothermic |
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enthalpy of neutralization |
enthalpy change that occures when an acid and base react together to form one mole of water |
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acid + carbonate → |
salt + water + carbon dioxide net ionic equations: 2H⁺ +CO₃²⁻ → H₂O +CO₂ |
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effervesence |
gas given off so they visibly produce bubbles acid + carbonate acid + metal |
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acid-base indicators |
changes color reversibly according to the concentration of H⁺ ions in the solution |
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Litmus |
Pinkin acids Bluein alkalis |
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Methyl Orange |
Redin acids Yellowin alkalis |
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Phenolphthalein |
Colorlessin acid Pinkin alkalis |
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Universal indicator |
changes color for each pH |
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acid-base titration |
reacting a measured volume of one solution and adding another to the equivalence point where they exactly neutralize eaech other so the molarity of the other can be found |
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pH calculation formulas |
pH= -log[H⁺] pOH= -log[OH⁻] [H⁺]= 10^pH [OH⁻]= 10^pOH pH+pOH= 14 |
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Equilibrium expression |
H₂O= H⁺ + OH⁻ |
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Equilibrium constant/ ionic product constant of water |
[H⁺][OH⁻]/[H₂O] [H⁺][OH⁻]= 1*10⁻¹⁴ at 298K |
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relationship between H⁺ and OH⁻ |
inverse |
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Strong Acid |
dissociates completely weak conjugate base |
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weak acid |
dissociates partially strong conjugate base |
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strong base |
ionizes fully weak conjugate acid |
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weak base |
ionizes partially strong conjugate acid |
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Equilibrium of weak acids and bases favor |
the left |
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strength is a measure of |
how readily is dissociates in aqueous solution not the same as concentration |
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strong acids examples |
HCl, HNO₃, H₂SO₄ |
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weak bases examples |
LiOH, NaOH, KOH, Ba(OH)₂ |
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strong vs weak properties |
strong have higher concentrations strong have higher conductivity reactions happen faster with stronger acids pH |
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Why is rain naturally acidic (pH 5.6) |
due to the presence of dissolved carbon dioxide which dissolves in water to form weak carbonic acid H₂O + CO₂ ↔ H₂CO₃ ionizes: H₂CO₃ ↔ H⁺ + HCO₃⁻ |
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acid rain |
refers to a solution with a pH below 5,6 meaning it contains other acids main contributors are oxides of sulfur and nitrogen (primary pollutants) acid rain is secondary pollutant produced when these acidic gases dissolve in water |
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Acid deposition |
includes all processes by which acidic components as preciptates or gases leave the atmosphere |
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wet acid deposition |
rain, snow, sleet, hail, fog, mist, dew fall to the ground as aqueous precipitates |
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dry acid deposition |
acidifying particles, gases fall to the ground as dust and smoke, later dissolve in water to form acids |
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How is sulfur dioxide produced |
Producedfrom burning of fossil fuels, particularly coal and heavy oil in power plantsused to generate electricity; also released in industrial processes of smeltingwhere metals re extracted from their ores 90%of sulfur dioxide emissions come from coal it is a colorless gas with a sharp smell |
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equations involving sulfur dioxide |
S + O₂ → SO₂ H₂O + SO₂→ H₂SO₄ 2SO₂ + O₂ → 2SO₃ H₂O + SO₃→ H₂SO₄ |
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Nitrogen monoxide is formed by |
combustion engines where the burning of fuel releases heat that causes nitrogena nd oxygen to combine |
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Equations involving nitrogen monoxide and dioxide |
N₂ + O₂ → 2NO N₂+ 2O₂→ 2NO₂ H₂O + 2NO₂ → HNO₂ + HNO₃ 2H₂O + 4NO₂ + O₂→ 4HNO₃ |
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Impact acid deposition has on materials |
both dry (sulfur dioxide) and wet (sulfuric acid) deposition creates calcium sulfate which erodes structures and causes stress and expansion in the stonework also creates salts which increase the rate of electrochemical corrosion like rust corrodes metals |
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equations about the impact on materials |
2CaCO₃ + 2SO₂ + O₂→ 2CaSO₄ + 2CO₃ CaCO₃ + H₂SO₄ → CaSO₄ + H₂O + CO₂ Fe + SO₂ + O₂ → FeSO₄ Fe + H₂SO₄ → FeSO₄ + H₂ Al₂SO₃ + 6HNO₃ → 2Al(NO₃)₃ + 3H₂O |
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Impact acid deposition has on plants |
Slowergrowth, injury, death Leaching Mg²⁺,plants cannot synthesize chlorophyll and therefore cannot make food Acidrain also releases toxic minerals like Al³⁺ which damage plant roots Drydeposition can clog pores for gas exchange (stomata) |
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leaching |
mportant minerals like Mg²⁺, Ca²⁺, and K⁺ held in soil become soluble and wash away |
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impact acid deposition has on water |
Lakesbecome dead Fishcannot survive under pH5 BelowpH4, rivers are dead since toxic Al3+ leach out from aluminum hydroxide Aluminumions reduce fish's ability to take in oxygen eutrophication |
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eutrophication |
over fertilization of bodies of water can be caused by nitrates from acid rain results in algal blooms leading to oxygen depletion and death of lakes or streams |
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equation involving impact on water |
Al(OH)₃ + 3H⁺ → Al³⁺ + 3H₂O |
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impact acid deposition has on human health |
Acidrain components could react and sulfate or nitrate particles could be inhaled Leadto asthma, bronchitis, and emphysemaIrritationof eyes Al³⁺,Pb²⁺, and Cu²⁺ from the reaction of acid rain on metal structures like pipes isalso a risk |
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responses to acid deposition |
reduction of SO₂ and NO₂ emissions Lowerdemand of fossil fuels Moreefficient energy transfer systems Greateruse of public transportations,switchingto renewable energy sources Restorationof ecosystems by neutralizing the acid: CaO + H₂SO₄→ CaSO₄ + H₂O Ca(OH)₂ + H₂SO₄ → CaSO₄ + 2H₂O |
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how to reduce SO₂ emissions through pre-combustion methods |
Sulfurin metal sulfide can be removed by crushing coal and washing with water Hydrodesulfurization-catalytic process that removes sulfur from refined petroleum products byreacting it with hydrogen to form hydrogen sulfide (highly toxic) Hydrogensulfide can be converted into element sulfur to make sulfuric acid |
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how to reduce SO₂ emissions through post-combustion methods |
Flue-gasdesulfurization can remove 90% of SO2 from flue gas in smoke stacks before itis released into the atmosphere CaO + SO₂ → CaSO₃ CaCO₃ + SO₂ → CaSO₃ + CO₂ 2CaSO₃ + O₂ → 2CaSO₄ |
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how to reduce NO₂ emissions through catalytic converters in vehicles |
Exhaustgases can be controlled by catalytic converters where hot gases are mixed withair and pass over platinum/palladium based catalyst to make harmless products 2CO + 2NO → 2CO₂ + N₂ |
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how to reduce NO₂ emissions through lowering temperature for combustion |
Formationof NO is reduced at lower tempsRecirculationof exhaust gases back into the engine lowers temp |
