Chem3BTest1

Card Set Information

Author:
Anonymous
ID:
68318
Filename:
Chem3BTest1
Updated:
2011-02-22 23:43:52
Tags:
Chem3BTest1
Folders:

Description:
Chem3BTest1
Show Answers:

Home > Flashcards > Print Preview

The flashcards below were created by user Anonymous on FreezingBlue Flashcards. What would you like to do?


  1. Intramolecular definition +examples
    Within the molecule (ionic, covalent)
  2. Intermolecular
    Between the molecules (van der waals, dipole-dipole, hydrogen)
  3. Atm/Torr
    1 Atm/760 torr
  4. value of R in PV=nRT
    .0821 atm L/mol K
  5. Dalton's Laws of Partial Pressure
    • PT=ΣPi
    • PT=VP+Pi
    • Pi=XiPT (X=mole fraction)
  6. Making a molar solution
    • Obtain volumetric flask
    • Rinse with soapy water
    • Rinse with regular water
    • Rinse 2-3 times with DI water
    • Calculate g solute needed
    • Fill flask 1/2 full with DI water
    • Add correct g of solid using a funnel
    • Cap/shake to dissolve
    • Add DI water to within 1cm of marking
    • Add drop by drop until mark is met
    • Cap/shake
    • Place in storage bottle
  7. PPM and PPB
    1/106 and 1/109 units must be the same (g/g)
  8. Solubility of gas in liquid (related to temperature)
    As temperature increases solubility decreases
  9. Solubility of gas in liquid (related to pressure)
    As pressure increases solubility increases
  10. Colloidal dispersion
    • Homogeneous
    • Small enough to pass through filter
    • Too large for semi-permeable membrane
    • Can be seen with light
  11. Suspensions
    • Heterogeneous
    • Too big for filter
    • Too big for semi-permeable membrane
  12. Colligative properties
    Properties that depend on # of particles, not type of particle
  13. Isotonic values
    • .3 M
    • .9%m/v NaCl
    • 5%m/v Glucose
  14. Shrinking and swelling
    crenation and hemolysis
  15. Solution
    • Homogeneous
    • Can't be filtered
    • Will go through semi-permeable membrane
  16. Standardized
    Determine molarity to +/- .001M
  17. Proof of a reaction?
    • Solid
    • Weak electrolyte (heat)
    • Gas
  18. Arrhenius acid/base
    Produces H+/OH- in solution
  19. Bronstead-Lowry acid/base
    H+ donator/H+ acceptor
  20. H3O+
    Hydronium ion
  21. Conjugate acid/base formula
    HA+B<--->A-+HB
  22. Examples of molecules that are both acids and bases
    • H2O
    • NH3
    • CH3OH
  23. HCl
    stomach acid
  24. H2SO4
    Car batteries, Plant fertilizer
  25. HNO3
    Explosives, Fireworks, Fertilizers
  26. HC2H3O2
    Vinegar, food, plastics
  27. H2CO3
    Carbonated beverages, blood
  28. HF
    etching, art
  29. NaOH
    "Caustic lye," soap, drain cleaner
  30. KOH
    Soap production
  31. NaHCO3
    Antacid, baking soda
  32. NH3
    Detergent, fertilizer, glass cleaner
  33. Litmus colors
    acid - red, base - blue
  34. pH from [H+]
    pH = -log[H+]
  35. pH and pOH relationship formula
    pH + pOH = 14
  36. [H+] from pH
    [H+] = 10-pH
  37. Ka
    Ka = [H+][A-]/[HA]
  38. Larger Kameans...
    stronger electrolyte (more dissociation)
  39. [H3O+] from [OH-]
    [H3O+] = 1.0x10-14/[OH-]
  40. [OH-] from [H3O+]
    [OH-]=1.0x10-14/[H3O+]
  41. Nitrite buffer system
    HNO2 / NaNO2
  42. Acetate buffer
    HC2H3O2 / NaC2H3O2
  43. How does a buffer system maintain pH?
    • weak acid combines with strong base to create H2O and conj. base
    • Conj. base combines with H+
  44. Buffer systems in body
    • H2CO3 / HCO3-
    • H3PO4 / H2PO4- / HPO42- / PO43-

What would you like to do?

Home > Flashcards > Print Preview