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Acids and Bases

Acids and Bases. Chapter 20. Acids. A compound that produces hydrogen ions, H + , when dissolved in water. The defining particle of an acid is the hydronium (H 3 O + ) ion. H + + H 2 O  H 3 O +. Naming of Acids. Binary Acids – H + 1 other element (ex. HCl) Begin with “hydro”

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Acids and Bases

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  1. Acids and Bases Chapter 20

  2. Acids • A compound that produces hydrogen ions, H+, when dissolved in water. The defining particle of an acid is the hydronium (H3O+) ion. H+ + H2O  H3O+

  3. Naming of Acids Binary Acids – H + 1 other element (ex. HCl) • Begin with “hydro” • Use the “root” of the element name • Add the suffix “ic” • HCl = • HBr = • HF = • HI =

  4. Ternary Acids Ternary Acids- H + polyatomic ion (ex HNO3) • don’t use “hydro” • Use polyatomic name without “ending” • Add suffix “ic” if there was an “-ate” • Add suffix “ous” if there was an “-ite” • HNO3 = • HClO3 = • H3PO3 = • H2CO3 =

  5. Strong Acids – completely ionize in a water solution • 3 binary acids: • HCl, HBr, and HI • HCl + H2O  H3O+ + Cl- • Ternary acids: • Number of O atoms - # of H atoms > 2 • HNO3 + H2O  H3O+ + NO3- • Ternary acid examples: • H2SO4 , HClO3 , HNO3

  6. Weak Acids – ionize only slightly in a water solution • All acids not listed earlier are weak acids • # O atoms - # H atoms > 1

  7. Properties of Acids • Sour taste • Corrosive • Change the color of litmus (blue to red) • React with metals to produce H2 gas • Aqueous solutions of acids are electrolytes • React with bases to form water and a salt • Examples: vinegar – acetic acid; lemon juice – citric acid; tea – tannic acid; ant venom – formic acid

  8. Bases • A compound that produces hydroxide ions, OH-, when dissolved in water

  9. Naming of Bases • All bases follow ionic naming rules • Name of the cation, followed by the name of the anion • NaOH = • Ca (OH2) = • KOH =

  10. Strong Bases – completely ionize in water solutions All hydroxides, OH- with Groups 1 and 2 metals (except Be) • NaOH • Mg(OH)2

  11. Weak Bases – ionize only slightly in water solution All bases not listed in previous slides are weak bases • Be(OH)2 • Al(OH)3

  12. Properties of Bases • Bitter taste • Feel slippery • Change color of litmus (red to blue) • Aqueous solutions of bases are electrolytes • React with acids to form water and a salt • Examples – Milk of magnesia (a base that treats problems of excess stomach acid), household cleaning products

  13. Water • The usual solvent for solutions of acids and bases • Sometimes donates hydrogen ions to another ion or molecule and sometimes it accepts hydrogen ions (can act as a Bronsted-Lowry acid or base)

  14. Self-Ionization of Water H2O + H2O H3O+ + OH- http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/animations/H2Oeq.html

  15. Self Ionization of Water • Occurs to a very small extent. • In pure water at 25o C, the concentration of hydrogen ions ([H+]) and the concentration of hydroxide ions ([OH-]) are equal [H+] = [OH-] = 1.0 x 10-7 M

  16. [H+] = [OH-] = 1.0 x 10-14 Min ALL aqueous solutions • As [H+] increase, [OH-] decreases • As [OH-] increases, [H+] decreases

  17. Acidity – Neutral – Basicity  [OH-] Basic solution [H+] < [OH-] Acidic solution [H+] > [OH-] [H+] Neutral solution [H+] = [OH-]

  18. What is the pH scale? • [H+] are often small, so the pH scale is easier to use to represent acidity and basicity • pH range is from 0 to 14

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