Term
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Definition
| a measure of how disordered a system is (randomness) |
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Term
| gibbs free energy (delta G) |
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Definition
| all the useful energy a substance contains |
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Term
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Definition
properties of solutions that depend solely on the number of particles dissolved in the solution. theydo not depend on the kinds of particles dissolved. they are physical properties of the solution.
There are four common types of colligative properties:
Vapor pressure lowering
Freezing point depression
Boiling point elevation
Osmotic pressure |
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Term
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Definition
| maximum amount of solute that can be dissolved in a solvent |
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Term
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Definition
like dissolves like
ex: organic dissolves organic |
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Term
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Definition
| the solubility of a gas in a liquid is proportional to the gas pressure |
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Term
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Definition
| solutions that have equal osmotic pressure |
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Term
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Definition
| substances that affect properties of surfaces |
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Term
| 2nd law of Thermodynamics |
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Definition
| in a spontaneous process, the entropy of the universe increases |
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Term
| 3rd law of Thermodynamics |
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Definition
| absolute entropy = 0 at 0 Kelvin |
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Term
| Gibbs Free Energy equation |
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Definition
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Term
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Definition
the number of electrolytes
N=1 if nonelectrlyte, nonvolatile, organic, or a polymer |
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Term
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Definition
1. delta VP = N(mol solute/total mol)(VP pure)
2. VP mix = VP pure - delta VP |
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Term
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Definition
| rate is equal to the concentration of the reactants raised to the power of its molar coefficients ONLY if it says the word slow. We dont ever care about the product of the slow step. |
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Term
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Definition
| added to a reaction to increase reaction rate, lower the activation energy of a reaction (forward and reverse), provide an alternate pathway or mechanism, are neither gained nor consumed in a reaction, doesnt affect G, H, E, S, or Keq, ONLY Ea, increases the frequency of effective collisions |
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Term
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Definition
| ln(K2/K1)=(Ea/R)((1/T1)-(1/T2)) |
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Term
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Definition
| a state of dynamic balance in which the rates of the forward and reverse reactions are equal, and the net concentrations of the reactants and products no longer change with time |
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Term
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Definition
| ratio of products raised to their coefficients divided by reactants raised the their coefficients. Pure solids and liquids are not included because their chemical activity is 1 |
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Term
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Definition
| same as Kc except only gases appear in the expression, if no gasses Kp=0 |
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Term
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Definition
| a measure of the extent to which a reaction occurs, measure of activity (the effective concentration). Depends of the nature of the reaction and the temperature. |
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Term
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Definition
| energy required to reach the activated complex (transition state) |
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Term
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Definition
| a substance that accepts a share in the pair of electrons, Al, B, Ti, -COOH |
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Term
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Definition
| substance that makes available a pair of electrons for sharing, Na, Li, K, Ca, Nitrogen without a charge |
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Term
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Definition
| the ionization constant of water divided by the ionization constant of a weak base |
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Term
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Definition
| a solution that resists a change in pH, will no have a large change in pH upon addition of a strong acid, weak acid or weak base + salt |
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Term
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Definition
| Point on a titration curve where equal moles of acid and base are added |
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Term
| Henderson Hasselbach equation |
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Definition
pH = -log Ka + log N[salt]/[acid]
used to find the pH of a acidic buffer solution |
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Term
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Definition
| can be either an acid or a base |
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Term
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Definition
| acids that release more than one proton in solution |
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Term
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Definition
| the process of neutralizing an acid with a base to form salt and water |
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Term
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Definition
| the measure of attraction of electrons by an atom from another part of the same molecule |
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Term
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Definition
| method of using an electric current to drive an otherwise non-spontaneous chemical reaction. Electrolysis is commercially highly important as a stage in the separation of elements from naturally-occurring sources such as ores using an electrolytic cell. |
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Term
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Definition
independent of pathway (capital letters)
ex: T (temp) P (pressure) V (volume) |
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Term
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Definition
| dependent on pathway (lower case) |
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Term
| 1st Law of Thermodynamics |
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Definition
| Law of Conservation of Energy: Energy is neither created nor destroyed in chemical reactions and physical changes. The energy of the Universe is constant. Chemical systems tend toward a state of minimum potential energy. |
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Term
| 2nd Law of Thermodynamics |
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Definition
| Chemical systems tend toward a state of maximum disorder. The entropy of universe must increase. |
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Term
| 3rd Law of Thermodynamics |
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Definition
| The entropy of a pure, perfect, crystalline solid at 0 K is zero. |
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Term
| Four factors that affect the rate of reaction |
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Definition
1.nature of reactant
2. concentration
3. temperature
4. presence of a catalyst |
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Term
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Definition
the effect on a solution of two dissolved solutes that contain the same ion.
The presence of a common ion suppresses the ionization of a weak acid or a weak base. |
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Term
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Definition
| A reagent of a known concentration (a standard solution) and volume is used to react with a solution for titration |
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Term
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Definition
| amount of acid = to amount of base |
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Term
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Definition
| the point at which the indicator changes color in a colorimetric titration. |
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Term
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Definition
| If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or total pressure, then the equilibrium shifts to counter-act the imposed change. |
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