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Chemistry Week 32 print
Transcript of Chemistry Week 32 print
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Chemistry Monday, April 23rd – Tuesday, April 24th, 2018
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Do-Now: “Ch. 16 CN Part A” 1. Write down today’s FLT 2. Spontaneity of a rxn is determined by ___ and ____. 3. The universe tends towards ____ enthalpy and _____ entropy. 4. What is Gibbs Free Energy? 5. What is the equation for Gibbs Free Energy? 6. ΔG is always spontaneous (or -) when __________ and __________. 7. Take out your planner and ToC
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FLT • I will be able to describe the properties
of acids and bases of a reaction by completing Ch. 16 Notes Part A
Standard HS-PS1-1:PropertiesofElementsHS-ESS2-5:PropertiesofWaterHS-ESS3-4:HumanImpacts
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Ch. 16: Acid-Base Theories
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Introduction
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Introduction • Ions to know:
– OH- = Hydroxide Ion – H+ = Hydrogen Ion = proton – H3O+ = Hydronium Ion
• H3O+ and H+ are often used interchangeably in water because H2O + H+ ßà H3O+
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Acids and Bases
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Acids and Bases • What is an acid? • What is a base?
– Both are necessary for life – Can be found in common substances,
from sodas to soaps
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Acids
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Acids • “Acid” à Latin word acidus, for sour
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Acids • Acids = Increase [H+] in water
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Acids • Properties of Acids:
– Taste sour
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Acids • Properties of Acids:
– Electrolytes (conduct electricity) – May be a strong or weak electrolyte, depending
on the acid
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Acids • Properties of Acids:
– React w/ metals to form H2 gas
HCl(aq) + Mg(s) → MgCl2(aq) + H2(g)
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Acids • Properties of Acids:
– Changes the color of indicators • Ex/ Blue litmus turns red
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Acids • Properties of Acids:
– Neutralization: react w/ bases to form H2O + a salt
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Acids • Properties of Acids:
– Have a pH < 7
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Acids • Properties of Acids:
– React with carbonates and bicarbonates to produce a salt, water, and carbon dioxide gas
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Acids • How do you know if a chemical is an acid?
– Usually (not always) starts with hydrogen – Examples of acids: – HCl (monoprotic) – H2SO4 (diprotic) – H3PO4 (triprotic)
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Effects of Acid Rain on Marble (marble is calcium carbonate)
George Washington: BEFORE acid rain
George Washington: AFTER acid rain
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Acids Neutralize Bases HCl + NaOH → NaCl + H2O
-NeutralizationreactionsALWAYSproduceasalt(whichisanioniccompound)andwater.
-Ofcourse,ittakestherightproportionofacidandbasetoproduceaneutralsalt
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Pair-Share-Respond 1. Describefourpropertiesofacids2. Whatdoesaneutralizationreactionalwaysproduce?
3. Distinguishbetweenthetermsmonoproticanddiprotic
4. WhataretwonamesforH+?
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Naming Acids
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Naming Acids • Binary Acids (hydrogen + another element) • Named as hydro______ic acid • Ex/ • HF = hydrofluoric acid • H2S = hydrosulfuric acid • What would be the names of…
– HBr? – H3P? – HCl?
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Naming Acids • Oxyacids (contain a polyatomic ion) • IF the polyatomic ion ends in –ate, then.. • ________ic acid (no hydro) • Ex/ • HNO3 = nitric acid • H2SO4 = sulfuric acid • What would be the names of…
– H2CO3? – H3PO4?
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Bases
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Bases • “Alkali” à Arabic for the ashes that come
from burning certain plants
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Bases • Bases = increases [OH-] in water
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Bases • Properties of Bases:
– Taste bitter and feel slippery
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Bases • Properties of
Bases: – Change the
color of indicators
– Ex/Red litmus turns blue
Red litmus paper turns blue in contact with a base (and blue paper stays blue).
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Bases • Properties of Bases:
– May be a strong or weak electrolyte in solution
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Bases • Properties of Bases:
– Neutralization - react with acids to form water and a salt
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Bases • Properties of Bases:
– Have a pH > 7
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Bases • How do you know if a chemical is a base?
– Usually (not always) ends with OH- – Examples of bases: – NaOH – Ca(OH)2 – NH3
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Bases Neutralize Acids
Milk of Magnesia contains magnesium hydroxide, Mg(OH)2, which neutralizes stomach acid, HCl.
2 HCl + Mg(OH)2
MgCl2 + 2 H2O Magnesium salts can cause diarrhea (thus they are used as a laxative) and may also cause kidney stones.
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Three Definitions of Acids-Bases (Three Theories)
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Three Acid-Base Theories • Arrhenius • Brønsted-Lowry • Lewis
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Arrhenius Acid-Base Theory
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Arrhenius Acid-Base Theory • Arrhenius Acid = Donates H+ in water • Arrhenius Base = Donates OH- in water • (Increases the concentration of ions in water)
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Arrhenius Acid-Base Theory • Arrhenius Acid = Donates H+ in water • Arrhenius Base = Donates OH- in water
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Arrhenius Acid-Base Theory • What about substances that still are acidic/
basic, but don’t do this?
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Brønsted-Lowry Acid-Base Theory
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Brønsted-LowryAcid-BaseTheory• Brønsted-LowryAcid:Donatesaproton(H+)Brønsted-LowryBase:Acceptsaproton(H+)
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Brønsted-Lowry Acid-Base Theory • Typically the most accepted theory
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Lewis Acid-Base Theory
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Lewis Acid-Base Theory • Lewis Acid = Accepts an e- pair • Lewis Base = Donates an e- pair
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Lewis Acid-Base Theory • Useful with organic chemistry
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Sample Problems • Whichistheacid?Base?
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Sample Problems • Whichistheacid?Base?
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Sample Problems • Whatwillformwhenthefollowingdonate(orlose)aproton?
• HCl
• H2O
• HNO3
• H2SO4
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Sample Problems • Whatwillformwhenthefollowingaccept(orgain)aproton?
• Br-
• H2O
• NO3-
• SO32-
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Pair-Share-Respond 1. WhatisthenameofHCl?2. WhatisthenameofHClO3?3. Describethreepropertiesofbases4. Listthreeacid-basetheories5. DistinguishbetweenanArrheniusbaseandaBrønsted-LowryBase
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Chemistry Wednesday, April 25th – Thursday, April 26th,
2018
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Do-Now: “Ch. 16 CN Part B” 1. Write down today’s FLT 2. List two properties of acids. 3. List two properties of bases. 4. How do the definitionsofArrheniusacid-basesdifferfromBrønsted-Lowrydefinitions?5. Copy the equation: HBr + H2O à Br- + H3O+ 6. Draw arrows between your reactants and products to determine which molecule is your acid, and which is your base. 7. Take out your planner and ToC
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Brainstorm Protocol 1. Thegoalistogeneratethelongestpossiblelist
asagroup2. Whenpromptedtodoso,identifywhowill
providethefirstanswer3. Then,goclockwisetothenextperson.4. Donotskippeopleanddonotsayananswer
forthem.5. OnlysayONEansweratatime6. Quantityoverquality7. Stayontopic8. PencilsmustbedownwhenIsaytimeisup9. Listsmustbeexactlythesame
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FLT • I will be able to calculate the pH and
pOH of a solution given concentrations by completing Ch. 16 CN Part B
Standard HS-PS3-1:Createacomputationalmodeltocalculatethechangeintheenergyofonecomponentinasystemwhenthechangeinenergyoftheothercomponent(s)andenergyflowsinandoutofthesystemareknown
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Ch. 16: The pH Scale
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Recall
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Recall • Acids increase [H+] in water • Bases increase [OH-] in water
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Recall • Acids have a LOW pH • Bases have a HIGH pH
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The pH Scale
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The pH Scale • pH is a measure of how acidic or basic a
solution is • pH = measurement of [H+] • pH à potential of Hydrogen
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The pH Scale • pH can be approximated using indicators
(such as litmus paper) or measured accurately using a pH meter.
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The pH Scale • The pH scale ranges from 0 to 14
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The pH Scale • A soln’ with a pH =7 is neutral • Pure water is neutral • Is tap water neutral?
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The pH Scale • A soln’ with a pH < 7 is acidic • pH of orange juice is ~ 3.3 • pH of lemon juice is ~2 • Which is more acidic?
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The pH Scale • The lower the pH, the more acidic the
soln’ is
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The pH Scale • A soln’ with a pH > 7 is basic • pH of baking soda solution ~8.4 • pH of toothpaste ~10 • Which is more basic?
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The pH Scale • The higher the pH, the more basic the
soln’ is
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The pH Scale • A change of 1 pH is equivalent to a 10x
increase/decrease in acidity • Ex/ pH 1 is ten times as acidic as pH 2 • Ex/ pH 0 is 10 x 10 = 100 times as acidic as
pH 2
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Calculating pH and pOH
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Calculating pH and pOH • Formula given pH/pOH:
pH + pOH = 14
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Example 1 • What is the pOH of a solution if the pH is 5? • Is the solution acidic or basic?
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Ex. 2 • What is the pH of a solution if the pOH is
3.5? • Is the solution acidic or basic?
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Calculating pH and pOH • Formulas given
concentration: pH = -log[H+]
pOH = -log[OH-]
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Ex. 3 • What is the pH of a solution if the [H+] is 1 x
10-6 M? • Is the solution acidic or basic?
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Ex. 4 • What is the pH of a solution if the [H+] is 4 x
10-10 M? • Is the solution acidic or basic?
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Ex. 5 • What is the pH of a solution if the [OH-] is 4 x
10-11 M? • Is the solution acidic or basic?
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Ex. 6 • What is the pH of a solution if the [OH-] is 4.3
x 10-5 M? • Is the solution acidic or basic?
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Calculating pH and pOH • Formulas given pH or pOH:
[H+] = 10-pH [OH-] = 10-pOH
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Ex. 7 • What is the [H+] of a solution with a pH of
5.2.
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Ex. 8 • What is the [OH-] of a solution with a pOH of
8.8.
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Chemistry Wednesday, April 25th – Thursday, April 26th,
2018
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Do-Now: “BrainPOP: Acids & Bases” 1. Write down today’s FLT 2. The pH scale ranges from ____ to ____. 3. Which is more acidic: pH 3 or pH 6? 4. Which is more basic: pH 3 or pH 6? 5. If you have a pH of 3, what is your pOH? 6. What is the pH of a solution if the [H+] is 1.5 x 10-6 M? Show all steps. 7. Take out your planner and ToC
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BrainPOP:Acids&Bases• WatchtheBrainPOPvideo• Afterthevideo,answerthequestionsinyourgroup–everymembermustcopydownthesameanswer
• Thegroupwiththemostcorrectanswersà+5dojopointseach
https://www.brainpop.com/science/matterandchemistry/acidsandbases/
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FLT • I will be able to define strong acids and
weak acids & define the products of an acid-base reaction by completing Ch. 16 CN part C
Standard HS-PS3-1:Createacomputationalmodeltocalculatethechangeintheenergyofonecomponentinasystemwhenthechangeinenergyoftheothercomponent(s)andenergyflowsinandoutofthesystemareknown
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Ch. 16: Acid/Base Strength & Neutralization
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Recall
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Recall • The pH scale ranges from 0-14 • What’s more acidic? • What’s more basic?
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Recall • Brønsted-Lowryacids:
– DonateH+inwater
• Brønsted-Lowrybases:– Accept H+ in water
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Recall • Acids and bases are
electrolytes • This means that they
dissociate into ions in water
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Recall • What if they only dissociate a little bit?
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Electrolytes and Nonelectrolytes • Weakelectrolytes=onlypartiallyionizeWeakelectrolyteshaveonlyafractionofthesolutethatexistsasions(about1%)– Weakacidsandbases;ammonia,aceticacid
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Acid/Base Strength
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Acid/Base Strength • Acids are classified as strong or weak
depending on the degree to which they ionize in water
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Acid/Base Strength • Strong acids = completely ionize in water • Ex/ HCl, HNO3, H2SO4
HCl(g) + H2O(l) à H3O+(aq) + Cl-(aq)
100% ionized
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Acid/Base Strength • Weak Acids = ionize only slightly in water. • Ex/ Ethanoic (acetic) acid CH3COOH(aq) + H2O(l) ßà H3O+
(aq) + CH3COO-(aq)
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Acid/Base Strength • Bases are also classified as strong or weak
depending on the degree to which they ionize in water
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Acid/Base Strength • Strong bases = completely dissociate
into metal ions and OH- ions in water • Ex/ Ca(OH)2, NaOH, KOH
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Acid/Base Strength • Weak Bases = Produce a small amount of
OH- in water • Ex/ Ammonia (NH3)
NH3(aq) + H2O(l) ßà NH4+
(aq) + OH-(aq)
99% NH3 still present, ~1% ionized
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Conjugate Acids & Bases
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TheBrønsted-Lowry Definition• Wecanlabelouracid-basereactionsusingproton-transfer
• Ex1:
HCl(aq)+H2O(l)àH3O+(aq)+Cl-(aq)
• Ex2:
NH3(aq)+H2O(l) ßà NH4+
(aq) + OH-(aq)
Donated(Lost)H+
Donated(Lost)H+
Accepted(gained)H+
Accepted(gained)H+
Acid
Acid
Base
Base
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Conjugate Acids & Bases • In this equation, what is the acid? What is
the base?
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Conjugate Acids & Bases • Note: This is a reversible reaction. The back
reaction is also an acid-base reaction. • Which is the acid and which is the base?
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Conjugate Acids & Bases • Conjugate Acid = formed when a base
gains H+
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Conjugate Acids & Bases • Conjugate Base = formed when an acid
loses H+
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TheBrønsted-Lowry Definition• Wecanlabelouracid-basereactionsusingproton-transfer
• Ex1:
HCl(aq)+H2O(l)àH3O+(aq)+Cl-(aq)
• Ex2:
NH3(aq)+H2O(l) ßà NH4+
(aq) + OH-(aq)
Donated(Lost)H+
Donated(Lost)H+
Accepted(gained)H+
Accepted(gained)H+
Acid
Acid
Base
Base
Conj.acid
Conj.base
Conj.acid
Conj.base
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Try This: • In the equation below, label the acid, base,
conjugate acid, and conjugate base.
HNO3(aq) + CH3OH ßà CH3OH2+
(aq) + NO3-(aq)
Donated(Lost)H+
Acid Conj.base
Base Conj.acid
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Conjugate Acids & Bases • Conjugate Acid-Base Pair Strengths:
– Strong acids/bases form weaker conjugates – Weak acids/bases form stronger conjugates
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Last Tidbits
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Last Tidbits • Amphoteric substances = act as both an
acid or a base
NH3 + H2O ↔ NH41+ + OH1-
base acid c.a. c.b. HCl + H2O ↔ H3O1+ + Cl1-
acid base c.a. c.b.
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Last Tidbits • Neutralization Reaction - a reaction in
which an acid and a base react in an aqueous solution to produce a salt and water:
HCl(aq) + NaOH(aq) à NaCl(aq) + H2O(l)
H2SO4(aq) + 2KOH(aq)à K2SO4(aq) + 2 H2O(l)
– Table 19.9, page 613 lists some salts
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Last Tidbits • Acid + Base à Water + Salt • Properties related to every day:
– antacids depend on neutralization – farmers adjust the soil pH – formation of cave stalactites – human body kidney stones from
insoluble salts
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Pair-Share-Respond 1. Distinguishbetweenstrongandweakacids
2. Distinguishbetweenstrongandweakbases
3. Whatareconjugateacids?4. Whatareconjugatebases?5. Howcanyoudetermineifyourconjugateacid/baseisstrongorweak?