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Chemistry 128
lecture
| Question | Answer |
|---|---|
| chemical kinetics | investigation of the rate at which rxns occur |
| rate | how fast a quantity changes w/ time |
| rxn rate | how fast reactants are consumed and products formed |
| rate = | change in quantity/ time elapsed |
| rate law = | k[A][B] |
| method of initial rates | initial rates of rxn is measured w/ several different starting amounts of reactants |
| R-->P rate= | k[R]^x |
| order (0) | stays the same x1 |
| order (1) | doubles x2 |
| order (2) | x4 |
| order (3) | x8 |
| log(a)(b) | loga+logb |
| log a/b | loga-logb |
| log a^b | bloga |
| collision theory | reactant particles must collide, collide w. enough energy to initiate rxn, and have proper orientation |
| increase rate of rxn | temp. add more reactants. |
| exothermic AB+C --> A+BC | means BC is stonger than AB |
| endothermic AB+C--> A+BC | meand AB is stronger than BC |
| catalyst | lower A. E |
| unimolecular | A-->B |
| bimolecular | A+B-->AB or AB+C->ABC |
| termolecular | A+B+C->ABC |
| Arrenhenius acid | substance that donates a proton |
| Arrenhius Base | substance that accepts a proton |
| Monoprotic acid | only 1 proton to donate |
| monoprotic base | can only accept 1 proton |
| polyprotic acid | can donate several protons |
| polyprotic base | can accept several protons |
| Amphiprotic | a substance that acts as both an acid and a base |
| The stronger the acid | the weaker the conjugate base |
| The stronger the base | the weaker the conjugate acid |
| Ka is used to measure | the strength of the acid |
| kb is used to measure | the strength of the base |
| Ka= | Products / Reactants |
| kb= | Products/ Reactants |
| k=kw= | 1.0x 10^-14 @ 25 C |
| pH= | -log[H] |
| pOH= | -log[OH] |
| [H]= | 10^-pH |
| [OH]= | 10^-pOH |
| kw= | [H][OH] |
| pH+pOH= | 14.00 |
| kakb | kw |
| acidic solution pH | less than 7 |
| basic solution pOh | greater than 7 |
| pka= | -logka |
| pkb= | -logkb |
| As acid strength increases | ka increases and pka decreases |
| as base strength increase | kb increases and pkb decreases |
| Reaction direction: k<1 | rxn is left |
| reaction direction: k>1 | rxn is right |
| k= | kakb/kw |
| Cl- | neutral |
| No3- | neutral |
| Br- | neutral |
| ClO4- | neutral |
| Na, Ca, k, ba | neutral |
| diprotic: ka1kb2= | kw |
| diprotic: ka2kb1= | kw |
| triprotic:ka1kb3= ka2kb2= ka3kb1= | kw |
| Lewis acid | electron pair acceptor |
| lewis base | electron pair donor |
| buffer | resist pH change when acid or base is added both. must be an acid and a base that do not react with each other. usually conjugate acid-base pair |
| Hendersen-Hasselbach equation | pH=pka+log(base/acid) |
| buffer should have pka close to | ph |
| indicators | weak acid or base whose acidic &basic forms are different colors (loss or gain of a proton) |
| solubility | is a continuum |
| solubility | how many moles/grams dissolve in a given amount of water |
| precipitation will begin when.. | Q=ksp |
| Ksp is solubility of solution | 18.2 or appendix J |
Created by:
threasa.hicks
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