Modern Chemistry Chapter 14

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Modern ChemistryChapter 14

• Acids Bases

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Section 1Properties of Acids Bases

• Aqueous solutions of acids taste sour.
• Acids change the color of acid-base indicators.
• Some acids react with active metals and release
  hydrogen gas.
• Acids react with bases to produce salts and
  water.
• Acids conduct electricity (electrolytes).

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Common acids

• Name some items with a sour taste, and it is
  usually an acid or has an acid as an ingredient.

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Binary Acids

• A binary acid is an acid that contains only
  hydrogen and one of the more electronegative
  elements. (group 17 elements primarily)

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Binary Acid Nomenclature

• Naming binary acids
• The name of a binary acid begins with the prefix
  hydro.
• The root of the name of the second element
  follows this prefix.
• The name then ends with the suffix ic.
• HF hydrofluoric acid
• HCl hydrochloric acid
• HBr hydrobromic acid
• HI hydroiodic acid
• H2S hydrosulfuric acid

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Acid Nomenclature Practice

• Write the formula for the following binary acids
• 1) hydrochloric acid
• 2) hydroiodic acid
• Name the following binary acids
• HBr(aq)
• H2S(aq)
• HF(aq)

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Oxyacids Nomenclature

• An oxyacid is an acid that is a compound of
  hydrogen, oxygen, and a third element, usually a
  nonmetal.
• Nomenclature of an oxyacid.
• Determine the name of the polyatomic ion combined
  with the hydrogen.
• If the name of the ion ends with ate, replace
  it with ic and add the word acid.
• If the name of the ion ends with ite, replace
  it with ous and add the word acid.
• For example for HNO3, NO31- nitrate, so the
  name of the acid is nitric acid.
• Also for HNO2, NO21- nitrite, so the name of
  the acid is nitrous acid.

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Acid Nomenclature Practice

• Name the following oxyacids
• H2SO4 (aq)
• H2SO3 (aq)
• HClO (aq)
• HClO2 (aq)
• HClO3 (aq)
• HClO4 (aq)
• HC2H3O2 (aq)

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Acid Nomenclature Practice

• Write the formula for the following acids
• phosphoric acid
• phosphorous acid
• nitrous acid
• nitric acid

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Common Industrial Acids

• Sulfuric acid (H2SO4) is the most commonly
  produced industrial chemical and is used in
  petroleum refining, metallurgy, and is used in
  the production of fertilizer, metals, paint, dye,
  paper detergents. It is also used in car
  batteries.

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Common Industrial Acids

• Nitric acid (HNO3) stains proteins (like those in
  your skin) yellow. It is used in the manufacture
  of explosives, plastics, and pharmaceuticals.

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Common Industrial Acids

• Phosphoric acid (H3PO4) is used primarily in the
  manufacture of fertilizers and animal feed. It
  is also used as a flavoring for beverages.

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Common Industrial Acids

• Hydrochloric acid (HCl) is the acid produced by
  the stomach for digestion. It is also called
  muriatic acid and is used to clean masonry and
  maintain the acidity of swimming pools.

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Common Industrial Acids

• Acetic acid (HC2H3O2) is the active ingredient in
  vinegar and is produced by the fermentation of
  certain plants. It is used as a flavoring agent,
  a preservative, and as a fungicide. It is also
  used in the manufacture of plastics.

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Properties of Bases

• Aqueous solutions of bases taste bitter.
• Dilute aqueous solutions of bases feel slippery.
• Bases change the color of acid-base indicators.
• Bases react with acids to produce salts water.
• Bases conduct electricity (electrolytes).

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Base Nomenclature

• All bases contain the hydroxide (OH) ion.
• Most bases also contain a metallic ion.
• The number of hydroxide ions is determined by the
  charge of the metal ion.
• Na OH- ? NaOH
• Ca2 OH- ? Ca(OH)2
• Al3 OH- ? Al(OH)3

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Base Nomenclature

• Naming bases is VERY difficult.
• Name the cation.
• Add hydroxide.
• Ba(OH)2 barium hydroxide
• NH4OH ammonium hydroxide
• KOH potassium hydroxide

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Arrhenius Acids Bases

• An Arrhenius acid is a chemical compound that
  increases the concentration of hydrogen, H
  (hydronium, H3O) ions in an aqueous solution.
• An Arrhenius base is a chemical compound that
  increases the concentration of hydroxide (OH-)
  ions in an aqueous solution.

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Acid Base Strength

• A strong acid is one that ionizes completely in
  an aqueous solution.
• A weak acid is an acid that releases few hydrogen
  ions in an aqueous solution.
• A strong base, like a strong acid, is one that
  completely dissociates to produce hydroxide ions
  in an aqueous solution and acts as a strong
  electrolyte.
• A weak base is a weak electrolyte that produces
  few hydroxide ions and is usually not very
  soluble in water.
• Do section review questions 1 through 5 on page
  476.

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Cross-Disciplinary Connection

• Read the Cross-Disciplinary Connection entitled
  Acid Water-A Hidden Menace on page 477.
• Answer the three questions at the end of the
  article.

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Section 2Acid-Base Theories

• Bronsted-Lowry acid is a molecule or ion that is
  a proton (H) donor.
• Bronsted-Lowry base is a molecule or ion that is
  a proton acceptor.
• A monoprotic acid can donate only one proton (H)
  per molecule.
• A polyprotic acid can donate more than one proton
  per molecule.
• diprotic acid can donate 2 protons, such as H2SO4
• triprotic acid can donate 3 protons, such as H3PO4

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Lewis Acids Bases

• A Lewis acid is an electron pair acceptor.
• A Lewis base is an electron pair donor.

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Section 3Acid-Base Reactions

• A conjugate base is the species that remains
  after a Bronsted-Lowry acid gives up a proton.
• A conjugate acid is the species that is formed
  when a Bronsted-Lowry base gains a proton.
• For the reaction HF H2O ? F- H3O
• the F- is the conjugate base and the H3O is the
  conjugate acid.

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Neutralization Reaction

• A neutralization reaction is the reaction between
  an acid and a base to produce a salt and water.
• HCl NaOH ? NaCl H2O
• neutralization is the reaction of a hydronium
  (H3O) and a hydroxide (OH-) ion to form a water
  molecule.
• H3O OH- ? 2 H2O
• A salt is an ionic compound composed of a cation
  from a base and an anion from an acid.
• Na Cl- ? NaCl

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Acid Rain

• Gaseous byproducts of industrial processes enter
  the atmosphere and combine with water to produce
  an acid that the falls as acid rain.
• SO2 H2O ? H2SO3
• SO3 H2O ? H2SO4
• NO H2O ? HNO2
• NO2 H2O ? HNO3

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Modern Chemistry Chapter 14 Test Review

• 35 multiple choice questions
• properties of acids and bases (9)
• definition, naming identification of binary and
  oxyacids (5)
• determining formulas of oxyacids from their names
  (3)
• names and uses of the common industrial acids
  sulfuric, nitric, hydrochloric, phosphoric, and
  acetic (6)
• definitions and identification of Arrhenius acids
  bases (3)
• definitions of weak strong acids (1)
• identify diprotic triprotic acids (2)
• definition of Bronsted-Lowry acids bases (2)
• definition of Lewis acids bases (2)
• definition of conjugate acids bases (2)