chemistry sm-1232 week 7 lesson 1
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Chemistry SM-1232 Week 7 Lesson 1. Dr. Jesse Reich Assistant Professor of Chemistry Massachusetts Maritime Academy Fall 2008. Class Today. YES class on Friday Chapter 13 HW due, quiz due Today Chapter 14: Acids and Bases. Acids. Properties include: Sour taste Dissolve many metals - PowerPoint PPT PresentationTRANSCRIPT
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Chemistry SM-1232Week 7 Lesson 1
Dr. Jesse ReichAssistant Professor of Chemistry
Massachusetts Maritime AcademyFall 2008
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Class Today• YES class on Friday• Chapter 13 HW due, quiz due• Today Chapter 14: Acids and Bases
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Acids• Properties include:• Sour taste• Dissolve many metals• Turn litmus paper red• Can have strong smells
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Typical Acids• Sulfuric Acid• Nitric Acid • Acetic Acid• Carboxylic acids• Citric Acid• Malic Acid• Hydrochloric Acid• What’s common to all acid names?
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Bases• Properties:• Bitter taste• Feel slippery• Turn litmus paper blue• Some have strong smells
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Typical Bases• Sodium hydroxide• Potassium hydroxide• Magnesium hydroxide• Sodium bicarbonate• Sodium sulfate• Lithium phosphate• (ammonia)• What are common pieces to base names?
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Acid and Base Definitions
• 1: Arrhenius Definition• Acid: produces H+ ions in aqueous solutions,
also just called protons• Base: produces OH- ions in aqueous solutions
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Arrhenius acid• HCl H+ + Cl-• H2SO4 2H+ + SO4
2-
• H3PO4 3H+ + PO43-
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Hydronium ion• H+ when in water reacts with water to make
an hydronium ion
• H+ + H2O H3O+
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Arrhenius Base• A compound that produces OH- ions when
dissolved in water.
• NaOH Na+ + OH-
• Mg(OH)2 Mg2+ + 2OH-
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Typical Bases• NaOH, sodium hydroxide• KOH, potassium hydroxide• NaOCH3, Soidum methoxide• Calcium Carbonate
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Bronsted-Lowry Definition
• This definition rests on the transfer of H+ ions.• Bronsted acid is a proton H+ donor• Bronsted base is a proton H+ acceptor
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Acid Example
• HCl + H2O H3O+ + Cl-
• H2SO4 +2 H2O 2H3O+ + SO42-
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Base• NH3 + H2O NH4+ + OH-
• NaOH Na+ + OH-
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Amphoteric• Water is amphoteric because it can act like an
acid or base.• HCl + H2O H3O+ + Cl-
• NH3 + H2O NH4+ OH-
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Conjugate Acid-Base Pairs
• NH3 + H2O NH4+ + OH-
• Base, acid conjugate acid, conjugate base
• On the left NH3 gained it’s a base
• H2O gave H+ it’s a base
• On the right, now NH4+ has an H+ to give so it’s
the conjugate acid• OH- lost the H+ so now it’s the conjugate base
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Acid Base Reactions• Neutralization• Acid Reactions• Base Reactions
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Neutralization• Most common reaction!• For Arrhenius acid Base Reactions:• Acid + Base = Water + Salt
• For Bronstead acid base reactions:• AcidH+ + Base- conjugate base- + conjugate acid+
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Arrhenius Acid base Reactions
• HCl + NaOH H2O + NaCl
• H2SO4 + 2 KOH 2 H2O + K2SO4
• Label the acid, base, salt and water
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Bronstead Acid-Base Reactions
• HCl + NH3 NH4+ + Cl-
• Label the acid, base, conjugate acid, and conjugate base
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Fancy Neutralization
• HCl + NaHCO3 H2CO3 + NaCl
• H2CO3 H2O + CO2
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Acid Reactions• Acids eat metals• 2HCl + Mg H2 + MgCl2
• H2SO4 + Zn H2 + ZnSO4
• 2HCl + Fe H2 + FeCl2
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Acids eat oxides• 2HCl + K2O 2 KCl + H2O• 2HBr + MgO H2O + MgBr2
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Base Reactions• Bases dissolve a few metals• 2 NaOH + 2Al + 6H2O 2NaAl(OH)4 + 3 H2
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Work over break• 14.4-14.7 copy example problems. They are a
pain. They will take time. Plan for it. Be sure to read in chapter 14 up through page 509.