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CHEM 132 FINAL
| Question | Answer |
|---|---|
| what does enthalpy combine | internal energy and work (total heat content of the system) |
| how is enthalpy a state function? | it describes the state of a system |
| what is heat? | a description of change. the path that the change takes can change the heat transferred |
| what is true at constant pressure with heat and enthalpy? | q = delta H |
| what is hess's law? | regardless if the multiple stages/steps of a rxn, the total enthalpy change for the rxn is the sum of all changes |
| what is true for work if volume is constant? | no work is done |
| difference between delta G and delta G naught | delta G: spontaneity of a rxn delta G naught: free energy change of a rxn at STP |
| what is true about delta G when delta H < 0 and delta S < 0? | -delta G < 0 at low temps (spontaneous) -delta G > 0 at high temps |
| what is true about delta G when delta H < 0, delta S > 0? | delta G <0 at any temp (spontaneous) |
| what is true about delta G when delta H > 0, delta S > 0? | -delta G < 0 at high temps (spontaneous) -delta G > 0 at low temps |
| what is true about delta G when delta H > 0, delta S < 0? | delta G > 0 at any temp (non-spontaneous) |
| molar solubility | moles of dissolved solute/L of saturated solution (units are usually in M) |
| how to tackle solubility problems | -write out dissociation rxn and Ksp expression -if question gives gram solubility, convert to molarity |
| polyatomic ions (5 you don't know) | NH4+, CO3 2-, NO2- (nitrite), PO4 3-, SO3 2- (sulfite) |
| acids | proton donor. after donating, it becomes a conjugate base. since it loses positive charge, it becomes negatively charged |
| bases | proton acceptor. after accepting, it becomes a conjugate acid. since it gains positive charge, it's now positively charged. |
| start of titration curve | only weak acid/weak base in solution, Ka/Kb dictates pH |
| halfway point titration curve | half of the weak acid/base has been neutralized by the addition of strong base/acid/turned into conj. base/acid. [HA] = [A-]. pH = pKa, acid dictates pH |
| equivalence point of titration curve | all acid/base has been neutralized by addition of strong base/acid. only conj. base/acid remains, Kb/Ka dictates pH |
| what does a strong acid/base react with in titrations? | weak acid/base in solution, NOT WATER |
| how do strong bases/acids react? | stoichiometrically. find the limiting reagent, tells what's leftover in solution |
| what to do if there's leftover weak acid/base in solution | use ICE table to find pH |
| what to do if there's leftover strong acid/base in solution | they fully dissociate, no ICE table needed |
| what is a buffer composed of? | weak conj. acid/base pair |
| how to make a buffer? | salt and titration |
| what is the buffer capacity? | the amount of acid or base that can be added before the pH changes drastically (greater concentration, greater buffer capacity) |
| how to approach buffer problems (4 steps) | 1) determine what rxn is happening 2) use HH equation to figure out [] of buffer components 3) acid will react with conj. base (will dec.), making acid (will inc.) 4) if asking for pH, use Ka and ICE table |
| what is an alt. question asked for buffers? | make a buffer with a specific pH, and give a list of possible reagent (take in account TOTAL VOLUME when calculating molarity) |
| rate of rxn depends on... | how often molecules collide, colliding at the right angles, how much energy for collisions, etc. |
| what do rate laws tell us? | gives us info about how we can speed up/slow down rxns |
| order of the rxn | tells us how dependent the rate of the rxn is on the [ ] of the reactant |
Created by:
madalynes