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32 Cards in this Set

  • Front
  • Back
Bronsted/Lowry Base
proton acceptor
Bronsted/Lowry Acid
proton donor
changes from reactants to products and products to reactants, but no net change
colligative properties
Properties that depend only on the number (not the identity) of the solute particle.
Heat of Solution
enthalpy change associated with dissolving a solute in a solution
Freezing Point Depression
Kf=-(delta T)/ (m solute)
Heat of Neutralization
The enthalpy change associated with the neutralization of an acid-base reaction.
Beer's Law
A = absorbance
b=pathlenght of light through sample
The ratio of the intensity of emerging light (Ii) to the intensity of incident light (Io)

Light taken in by a sample

A=-log (%transmittance/100)
The study of light interaction with matter
Redox Reaction
the release and uptake of electrons
Reactants change oxidation states
Equivalence Point
the number of moles of base have completely reacted with the number of moles of acid
specific heat capacity
The amount of heat required to raise the temperature of one gram of substance bye one degree celsius
The study of heat flow into and out of a system
First Law of Thermodynamics
The energy of the universe is constant
Method of initial Rates
a method used to study chemical kinetics

is only concerned with initial rates (the average rate of a reaction over the first few seconds or at most few minutes)
Neutralization Reaction
An acid base reaction
Rate Law
algebraic expression
Relates rates to concentrations

Rate=k[A]ˆm [B]ˆn
Conjugate Acid
The species formed after a proton is added to a base.
Chemical kinetics
determining and studying the rates of chemical reactions
conjugate base
The species formed after an acid loses a proton
Rate of Reaction
expressed in terms of a decrease in any one of the reactants or an increase in any one of the products
end point
when a titration has stopped
hess's law
energy change in a reaction is the same weither it occurs in one step or a series of step wise reactions
an analytical technique

controlled addition of one reactant to another

both reactants are consumed
q=mc delta T
q=heat change (if positive=endothermic)
(if negative=exothermic)
C=specific heat
delta T=change in temperature
Molar Heat Capacity
Specific Heat Capacity x Molar Mass
a gravametric unit (value is set by mass)

moles solute/kg solvent
a gravametric unit (value is set by mass)

(grams x/total mass) x 100
Dulong and Petit's Law
A metal will have a molar heat capacity of about 24.9 J/ (mol x degrees celsius)