Georgia Performance Standards

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Georgia Performance Standards Essential
Questions

• SC7. Students will characterize the properties
  that describe the nature of acids and bases.
• b. Compare, contrast, and evaluate the nature of
  acids and bases
• Arrhenius Acids Bases
• Bronsted-Lowry Acid/Bases

• What are the different definitions of acids
  bases?
• How are acids and bases named?

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Characteristics of Acids

• pH below 7
• Sour to the taste
• Turns blue litmus paper red
• Conducts electricity in aqueous solution
• Stays clear in the presence of phenolphthalein
• Corrosive ('burns' your skin)
• Contains hydrogen ions (H) when dissolved in
  water
• Reacts with bases to form salt and water
• Reacts with metals to form hydrogen gas
• Reacts with carbonates to form carbon dioxide,
  water and a salt

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Characteristics of Bases

• pH above 7
• Soapy feels slippery
• Turns red litmus paper blue
• Turns phenolphthalein pink
• Corrosive ('burns' your skin)
• Many soluble bases contain hydroxyl ions (OH-)
• Reacts with acids to form salt and water

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Examples of Acids Bases

• Acids
• Hydrochloric acidSulfuric acidStomach
  juiceLemonsVinegarApplesOrangesGrapesSour
  milkWhite breadFresh milk

• Bases
• Human salivaDistilled waterBlood
  plasmaEggsSeawaterBoraxMilk of
  magnesiaAmmonia waterLimewaterCaustic soda

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Some Definitions

• Arrhenius
• An acid is a substance that, when dissolved in
  water, increases the concentration of hydrogen
  ions (or hydrominum ions H3O.
• EX HCl H2O ? H3O Cl-
• EX H2CO3 H2O ? H3O HCO3 -
• A base is a substance that, when dissolved in
  water, increases the concentration of hydroxide
  ions (OH-).
• EX NaOH ? OH- Na
• EX NH3 H2O ? NH4 OH -
• Arrhenius definition of acids and bases was
  limited, because it only applied to acids and
  bases in aqueous solutions.

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Some Definitions

• 2. Brønsted-Lowry
• An acid is a proton donor.
• must have a removable (acidic) proton
• A base is a proton acceptor.
• must have a pair of nonbonding electrons

• In a Bronsted- Lowry acid-base reaction protons
  are transferred from one reactant (the acid) to
  another (the base).
• Conjugate acid-base pairs form
• Ex HCl NH3 ?Cl- NH4
• HCl is the proton donor NH3 is the proton
  acceptor
• Ex H2O (l) NH3 (g) ? NH4 OH-
• H2O is the proton donor NH3 is the proton
  acceptor

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A. Acids and Bases
The Bronsted-Lowry Model

• Water acts as a base accepting a proton from the
  acid.
• Forms hydronium ion (H3O)

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Acid/Base Reactions Conjugate Acids and Bases

• The term conjugate comes from the Latin word
  conjugare, meaning to join together.
• Reactions between acids and bases always yield
  their conjugate bases and acids.

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What Happens When an Acid Dissolves in Water?

• Water acts as a Brønsted-Lowry base and abstracts
  a proton (H) from the acid.
• As a result, the conjugate base of the acid and a
  hydronium ion are formed.

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Amphorteric Substances

• If it substance has properties of an acid and a
  base, then it is an amphorteric substance.

• Water is amphoteric it can behave as either an
  acid or as a base
• Ionization of water

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Types of Acids

• A monoprotic acid is an acid that can donate only
  one proton (hydrogen ion) per molecule.
• Ionization does not occur in stages
• Examples HClO4, HCl, HNO3
• A polyprotic acid is an acid that can donate more
  than one proton per molecule
• Ionization occurs in stages
• Examples H2SO4 (diprotic), H3PO4 (triprotic)

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B. Naming Binary Acids

• An acid is a molecule with one or more H ions
  attached to an anion.

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B. Naming Binary Acids
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B. Naming Oxyacids
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B. Naming Oxyacids Acids
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B. Naming Acids Flowchart
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Naming Oxyacids Cont.

• Halogens can form more than two oxyacids.
• The oxyacids with the most oxygen atoms has the
  prefix per, and the one with the least has the
  prefix hypo.
• Naming of elements that form more than 2 oxyacids
• EX ClO- hypochlorite HClO- hypochlorus acid
• ClO2- chlorite HClO2- chlorous acid
• ClO3- chlorate HClO3- chloric acid
• ClO4- perchlorate HClO4- perchloric acid

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Rules for naming bases

• Name cation first and without changing it.
• Add the suffix -hydroxide
• Ex NaOH sodium hydroxide
• Ca(OH)2 calcium hydroxide
• LiOH Lithium hydroxide