Busy. Please wait.

show password
Forgot Password?

Don't have an account?  Sign up 

Username is available taken
show password


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.
We do not share your email address with others. It is only used to allow you to reset your password. For details read our Privacy Policy and Terms of Service.

Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.
Didn't know it?
click below
Knew it?
click below
Don't know
Remaining cards (0)
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how

CHEM 126 Chapter 13

CHEM 126 Final

IMAFs on protein - secondary: form shape - tertiary: overall 3D shape ** determines function - quanternary: arrangement of two or more polypeptide chains in protein
IMAFs on DNA - created by nucleic acids, two chains wrapped around each other in a double helix - polar exterior: PO4 groups interact with ion dipole & h bonds - polar interior: N containing bases, interact by dispersion forces - h bonds: keep chains together
colloid - dispersed (solute-like) substance distributed throughout a dispersing (solvent-like) substances - particles are larger than simple molecules but too small to settle out - EX: G-G (all gases) G-L (foam) L-L (milk) S-L (jelly)
Osmotic Pressure (concentration effects) - increases with number of solute particles - OP = (n solute/ v solution) *RT * n = moles of solute, R = gas constant, T = temp, V = volume of solution)
Freezing Point (concentration effects) - decreases with increasing solute particles -∆T f = ∆Kf*M *m = molality, Kf = freezing point depression constant, ∆Tf = Tf solvent - Tf solution - ∆T > 0 -> decrease in freezing point
Boiling Point (concentration effects) - increases when solute particles increase - boiling point elevation: ∆Tb = Kb * m * Kb = boiling point elevation constant, m = molality, ∆Tb = Tb solution - Tb solvent
Vapor Pressure (concentration effects) - decreases with number of particles of solute (more particles -> lower VP) -P solvent (∆P) = X solvent * P0 solvent * X solvent = 1 - X solute ∆P > 0 -> decrease in VP
Parts by Mass (or volume) - Volume of solute (L)/ volume of solution (L) - composition
Mole Fraction - amount of solute (mol)/ (amount of solute (mol) + amount of solution (mol)) -Vapor-Pressure Determination, Composition
Molality - m - amount of solute (mol)/ mass of solvent (kg) - colligative behavior
Molarity - M - (amount of solute (mol)/volume of solution (L)) - moles of solute that would be dissolved in 1 L of a solution - stoichiometry equations & analysis
Henry's Law - determines gas solubility at given pressures - S gas = K h * P gas * s= solubility (mol/L) Kh = Henry's Law Constant, P = pressure
effect of pressure on solubility - increase pressure -> increase GAS solubility - increase pressure -> decrease does not affect solid of liquid solubility
effect of temp on solubility - increase temp -> increase solid solubility - increase temp -> decrease gas solubility
supersaturated - amount dissolved is more than max dissolved possible - unstable solution & will easily seperate out
unsaturated - amount dissolved is less than max dissolved possible
saturated - max amount of dissolved solid - crystallization rate = dissolving rate
sontaneity energy contribution - entropy contribution * help determine if process occurs spontaneously
entropy distribution of energy over larger number of states
∆H equations ∆H solution = ∆H solute + ∆ H solvation/hydration (always < 0) ∆H solvation = ∆H solvant + ∆H mixing ∆H solute = -∆H lattice (always > 0)
Solubility - S - max amount that dissolveds in a fixed quantity of a given solvent at a given temp - excess of solute is present
different types of solution L-S (salt water) L-L (gasoline) G-G (natural gas) G-L (soda) G-S (H2 + Pd) S-S (alloys)
2 substances form a solution? ∆H = exothermic -> unfavorable, will not mix * breaking strong for weak ∆H = endothermic -> favorable & will mix * breaking weak for strong
Created by: ccottrel



Use these flashcards to help memorize information. Look at the large card and try to recall what is on the other side. Then click the card to flip it. If you knew the answer, click the green Know box. Otherwise, click the red Don't know box.

When you've placed seven or more cards in the Don't know box, click "retry" to try those cards again.

If you've accidentally put the card in the wrong box, just click on the card to take it out of the box.

You can also use your keyboard to move the cards as follows:

If you are logged in to your account, this website will remember which cards you know and don't know so that they are in the same box the next time you log in.

When you need a break, try one of the other activities listed below the flashcards like Matching, Snowman, or Hungry Bug. Although it may feel like you're playing a game, your brain is still making more connections with the information to help you out.

To see how well you know the information, try the Quiz or Test activity.

Pass complete!

"Know" box contains:
Time elapsed:
restart all cards