Inorganic Chemistry Exam 2

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  1. Bronsted Acid
    Proton Donor
  2. Bronsted Base
    Proton Acceptor
  3. Kw =
    [H3O+] [OH-] = 1x10^-14
  4. pH =
    -log [H3O+]
  5. Borderline of acids and bases for concentration of [H3O+]
    1x10-7
  6. Ka =
    [H3O+] [A-] / [HA]
  7. Amphiprotic
    Acts as an Acid and a Base
  8. Binary Acid Strength going down a group
    • Increase in Acid Strength
    • 2
  9. Binary Acid Strength strength going across a period
    • Increase going right
    • 3
  10. Binary Acid - Predominance Diagram
    • Must be given the pKa. When given the left side is the most protonated side.
    • 4
  11. Oxoacids - Differs in Number Oxo Groups
    • 8-5p
    • 5
  12. Oxoacids - Differs in Charge
    • pKa + 5
    • 6
  13. Oxoacids - Differs in central atom
    • Most electronegative atom attracts more electrons, more acidic
    • 7
  14. Oxoacids - Predominance Diagrams
    • You do not need a pKa value. It can be determined using oxo group rule, and charge rule.
    • 8
  15. Adding Cation to Water - Very Strongly Acidic
    -pKa
    -precipitate
    -what happens to pH
    -s & p
    -d
    -f
    8
  16. Adding Cation to Water - Strongly Acidic
    -pKa
    -precipitate
    -what happens to pH
    -s & p
    -d
    -f
    8
  17. Adding Cation to Water - Moderately Acidic
    -pKa
    -precipitate
    -what happens to pH
    -s & p
    -d
    -f
    8
  18. Adding Cation to Water - Moderately Acidic
    -pKa
    -precipitate
    -what happens to pH
    -s & p
    -d
    -f
    8

Card Set Information

Author:
DianaKarlova
ID:
311161
Filename:
Inorganic Chemistry Exam 2
Updated:
2015-11-09 06:48:31
Tags:
Inorganic Chemistry
Folders:
Inorganic Chemistry
Description:
Inorganic Chemistry Exam 2 Review Questions: Acids, Bases
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