(Unit 2): Chem 11.3-11.4

• In the dissolution process: Endothermic (delta H>0) rupturing of ___-___ and ___-____ interactions (___ interactions)

  solute-solute, solvent-solvent, cohesive
• In the dissolution process: Exothermic (delta H<0) formation of ___-___ interactions (___interactions)

  solute-solvent, adhesive
• In the dissolution process: Gets lots of ___ from forming a mixture

  entropy
• In the dissolution process: Happens if delta Gdiss = delta__diss-Tdelta___ <0

  H, S
• Delta Hdiss = delta Hrupture + delta Hformation can be...

  endothermic or exothermic
• What are electrolytes?

  ions in a solution when dissolved
• Strong electrolytes dissociate ___ upon dissolving. Solutions are usually very good...

  100%, electrical conductors
• Weak electrolytes do not ___ ___. Solutions are usually...

  Completely dissociate, poor conductors
• The solubility of a solute is defined as...

  the maximum concentration of solute that will stay in the solution
• Solubility depends on the...


  identities of the solvent and solute, temperature, and for gases pressure
• Saturated solutions are defined as...

  have as much solute dissolved as possible
• You can recognize a saturated solution of a solid in a liquid because...

  some solid remains
• Unsaturated solutions are defined as...

  solutions can dissolve more of the solute
• Supersaturated solutions are defined as...

  containing more dissolved solute than a saturated solution
• Supersaturated solutions are ___. Slight disturbances can cause the solute...


  unstable, to precipitate out
• Miscible is defined as...


  Describes liquids that can be mixed in any ratios
• Immiscible is defined as...

  describes liquids that do not remain mixed (ex: oil and water)
• Solubility of gases ___ with ___ in ___. Solids generally ___

  decrease, increase, temperature, opposite
• Solubility of ___ compounds in water a balance between ___ ___ and ion dipole attractions in water.

  ionic, ionic attractions,
• ___ groups that are polar or can form H-bonds ___ water solubility

  molecular, increase
• What is the equation for molality?

  moles of solute / kilograms of solvent
• What is the equation for mole fraction?

  moles of component / total moles of mixture
• Does molality depend on temperature?

  No
• What is the equation for molarity?

  moles / L solution
• Freezing Point Depress Equation: delta Tf = -/Kf/mi. How do you rearrange it to solve for m?


  m = delta Tf / -/kf/i
• Freezing Point Depress Equation: delta Tf = -/Kf/mi. How do you rearrange it to solve for i?

  i = -delta Tf / -(Kf) * (m)
• Vapor pressure lowering: Pa = Xa Px*. How do you rearrange to solve for Xa

  Xa = Pa / Px
• If k is small, what can you do when calculating in RICE table

  Can rewrite the bottom equation without the x's
• What is the 5% rule in chemistry?

  answer is okay if x<5% of the smallest number if it is added to or subtracted from
• If you can't always approx, what do you do

  Use the quadratic formula
• How do you check your answer by using Q?

  Q=answer/Initial change from original ICE table
• little k =

  Aexp(-ea/RT)
• Big K =

  kf(forward)/kr(reversed)
• Delta G reversed =

  -DeltaG4
• DeltaG=


  -RTInK
• For gases, do you use kp or kc

  kp(partial pressure)
• For liquid or multiphase, do you use kp or kc


  kc(concentration)