Ch 11.2

Card Set Information

Author:
DesLee26
ID:
199570
Filename:
Ch 11.2
Updated:
2013-02-21 22:51:06
Tags:
CHM 112
Folders:

Description:
Units of Concentration
Show Answers:

Home > Flashcards > Print Preview

The flashcards below were created by user DesLee26 on FreezingBlue Flashcards. What would you like to do?


  1. What is concentration?
    amount of solute present in a given amount of solution
  2. What are hte three types of percent?
    • %...
    • - w/v
    • - v/v
    • - w/w
  3. Explain % w/v
    mass of components/ total volume of solution x 100
  4. Explain % v/v
    Volume of component/ total mass of solution x 100
  5. Explain % w/w
    mass of component/ total mass of solution x 100
  6. What are parts per million
    • mass of component / total mass of soluiotn x 10^5
    • = % w/w x 10^4
  7. What is 1 ppm equal to?
    • =1 g of component/ 1,000,000 grams of solutioin
    • = 1 mg of component/ 1 kg of solution
  8. What is mole fraction?
    Moles of A/ Total number of moles
  9. What is molarity?
    Moles of solute/ Liter of Solution
  10. What is molality?
    moles of solute/ kg of solvent
  11. Dilution of Solutions:
    V1C1=V2C2
  12. Factors affecting solubility
    • temp
    • presure
    • surface area of solid solute
    • stirringĀ 
    • polarity
  13. Most substances become more __ as temperature rises, although the exact relationship is often __ and __.
    • soluble
    • complex
    • nonlinear
  14. Most gases become __ in water as the temperature rises. The concentration units are __ at a gas pressure of 1 atm.
    • less soluble
    • millimoles
  15. Henry's Law
    • the solubility of a gas is proportional to the pressure of the gas over the solution
    • Sg=kPg
  16. What are colligative properties?
    What are some?
    • properties that depend on the number of solute particles in solution but not properties of the solvent
    • 1) vapor pressure lowering
    • 2) boiling point elevation
    • 3) freezing point depression
    • 4) osmotic pressure
  17. Number of solute particles:
    van't Hoff factor: i= moles of particles in solution/ moles of solute dissolved
  18. non-ionic solutes
    1=1
  19. ionic solutes
    i>1
  20. Raoult's Law
    • Psoln=Psolv X solv
    • For a single solute solution, Xsolute=1-X solv
  21. Change in vapor pressure of the solvent (the vapor pressure lowering)
    DeltaP=Psolv x Xsolute
  22. What happens if both components are volatile (have measurable vapor pressures)?
    the vapor pressure has a value intermediate between hte vapor pressure of the two liquids

What would you like to do?

Home > Flashcards > Print Preview