1. Formula Unit Equation
    an equation for a chemical reaction in which all formulas are written as complete formulas
  2. net ionic equation 
    an equation that results from canceling spectator ions from a total ionic equation
  3. total ionic equation
    an equation for a chemical reaction written to show the predominant form of all species in aqueous solution or in contact with water
  4. Bronsted-Lowry (acid, base, neutral)
    • acid- proton donor
    • base-proton acceptor
    • neutral-salt and water formed; salt has cation charateristics of the base and anion characteristics of the acid
  5. Arrhenius (acid, base, neutral)
    • acid-contains Hydrogen H+ donor
    • base- contains OH-, H+ acceptor
    • neutral-salt and water formed; salt has cation characterisitcs of the base and anion characteristics of the acid
  6. Strong Acids (7)
    • HCl hydrochloric acid
    • HI hydroiodic acid
    • HBr hydrobromic acid
    • HNO3 nitric acid
    • HClO4 perchloric acid
    • HClO3 chloric acid
    • H2SO4 sulfuric acid
  7. Lewis (acid, base, neutral)
    • acid- any species that can accept or share in an electron pair
    • base-any species that can donate or share one or more lone pairs of electrons
    • neutral- coordinate covalent (or dative) bond formation
  8. How to identify acidic, basic and normal salt
    • normal- no ionizable H or OH
    • acidic- salt with unreacted H atoms (ex. NaH2PO4)
    • basic- contains unreacted OH groups (ex. Al(OH)2Cl
  9. Conjagate Acid-Base Pair Concept and example
    • The stronger the acid, the weaker is its conjugate base; the weaker the acid, the stronger is its conjugate base
    • example: weak acid HF dissolves in water. The H+ is accepted by both OH- and F- because F- is a stong base; Hf is only slightly ionized
  10. Three properties of acids and bases
    • Change the colours of indicators
    • React to form salt and water
    • Aqueous solutions conduct electricity because they are ionized
  11. Strong Bases (8)
    • LiOH lithium hydroxide
    • NaOH sodium hydroxide
    • KOH potassium hydroxide
    • RbOH rubidium hydroxide
    • CsOH cesium hydroxide
    • Ca(OH)2 calcium hydroxide
    • Sr(OH)2 strontium hydroxide
    • Ba(OH)2 barium hydroxide
  12. sulfuric acid
  13. Sodium Hydroxide
  14. Barium Hydroxide
  15. Nitric acid
  16. KOH
    Potassium Hydroxide
  17. KHP
    Used to standardize bases; 204.2 grams per mole
  18. THAM, Na2CO3
    Used to standardize acids
  19. Celcius to F
  20. F to C
  21. C to Kelvin
  22. oxalic acid
  23. Boyle's law
    • P1V1=P2V2
    • Constant n, t
  24. Charle's Law
    • V1/T1=V2/T2
    • constant n,p
  25. Combined Gas Law
    • P1V1T2=P2V2T1
    • constant n
  26. 1 atm
    760 mmHg=760 torr
  27. Standard Temp and pressure
    0 C and 1 atm
  28. Standard Molar Volume at STP
    22.414 L/mol
  29. Molecular Weight
  30. Ideal Gas Law
  31. Universal Gas Constant
    R= 0.0821 (L*ATM)/(mol*k)
  32. PV=
    (mass/formula weight)*R*T
  33. Dalton's Law of Partial Pressure
  34. Pressure total

  35. Nitrous oxide
Card Set
Chapter 10 flashcards