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44 Cards in this Set

  • Front
  • Back

Half life calculation for first order

T 1/2= 0.693/k


Ln [A]=-kt +ln[A]0

List strong acids

HCl, H2SO4, HNO3, HClO4


All others are weak with intermediates, how do

With intermediates, how do you tell which step is the rate determining step with graphs?

One with the highest energy transition state

At equilibrium:

-rate of the forward and reverse reactions are equal


-concentrations have stopped changing BUT NEVER EQUAL!!!

pH vs. pKa

pH -measures the concentration of H3O in a solution


-describes solution


pKa- is a measure of the strength on an acid


-describes acid

Archenius Equation: Calculating Eact graphically

ln(k)= ln(A)+(-Eact/R)(1/T)


y =b + m x


R=8.314


M=(-Eact/R)

Calculating Ka and Kb for conjugate pair

(Ka)(Kb)= 1*10^-14

Half life for zero order

[A]=-Kt+[A]0


t1/2- [A]0/2k

Old DeltaG formula

DeltaG=deltaH-TdeltaS

Calculating Kat another temp

ln (K1/K2= -Eact/ R((1/T1)-(1/T2))


R=8.314

At 25 degrees C,


Kw= 1*10^-4 so,

(Ka)(Kb)=14


pKa+pKb=kw

Equilibrium constant and deltaG are related by:

DeltaG= -RT ln(k)


DeltaG @same temp


R=8.314


T=temp of (k)


k=Value of ka at t

pH and POH equations

pOH=-log [OH-]

a reaction would be slightly thermodynamically favorable, but occur very quickly if it has a ___

-small negative Delta G


-Low activation energy

A reaction would be very thermodynamically favorable, but occur very slowly if it has a ___

-Negative DeltaG


-High activation energy

Weak acids

-donate some protons


- Dissociates sometimes


-ionizes some

Strong acids

-Donates all protons


-Dissociates completely


-ionizes completely

Proceeds to equal

Implies a system that has never been at equilibrium responding to a stress and re-reaching equilibrium

How to find Activation energy for an intermediate reaction

difference between reactants and the energy of the highest transition state

inc in value of k=???


When does K change and when does it not change?

-favor in the products


-K does not depend on inc. or dec. of products or reactants but does depend on temp

Not an actual acid

-Donates nothing


-dissociates nothing


-ionizes nothing

Ka and Kb represents

Ka= Adid strength


Kb=base strength

What range is


1 stonger weak


2 weaker weak


and


3 really weaker weak acids in

110^-2


2 10^-8


3 10^-8

large Ka vs small Ka

inc. Ka, stronger acid


strong acids have infinite #s


~~~~~~~~~~~~~~~~~~~~~~~~~


Dec. Ka, weaker- Regular #s

pKa

is often used to indicate the acid strength instean of Ka (P) means -log

Higher the Ka the___ the pKa


The lower the pKa, the ___ the acid

lower


lower

strength of base is measured by ___

its desire to accept protons


-stronger base--->greater desire



CONJUGATE OF A WEAK ACID WILL ALWAYS BE A WEAK BASE

vice versa

can calculate the concentration depending on 3 things

1. whether the solute is an acid/ base


2. Whether it is a strong/weak (base or acid)


3. Concentration of the base/ acid

When an alkali metal is dissolved in water the solution is ___

basic

when the HCl salt is dissolved in H2o the solution is ___

acidic

When is a metal ion an "Acid"?

When it has a +2 or +3 charge

small x assumptions

assuming a small number can just be x as long as it is lower than 5%

list the strong base

OH-


-all others are weak

when an acid is added to water

-inc H3O+, shift to left


-dec. in OH-


[H3O+]> 1*10^-7, [OH-]<1*10^-7

adding base to water

-bases inc. [OH-}


-Shifts to the left


-[H3O+]<1*10^-7, [OH-]> 1*10^-7

How to calculate K from the graph

Find numbers on graph when it stops charging and fill into equation

DeltaG=0

-at breaking point


-not favorable to go in either direction


-system is already at equilibrium

DeltaG>o

-Non-spontaneous


-fav. in reverse reaction

DeltaG<0

-spontaneous


-Fav in forward reaction

In all aqueous solutions:


1. [H3O+][OH]=???


2. pH=pOH=???

1. =14


2. =7

The pH depends on the same three things that [H3O+] and [OH-] depend on:

1. whether the solute was and acid or a base


2. whether it was a strong or weak acid/base


3. The concentration of the acid/base

General statement: The rate law for each elementary step in a mechanism can be predicted from equation for that step

Note: This is not true for overall equations/reactions

No reaction or very little reaction, would be observed for reactions that have ___

-Positive DeltaG's


-Really high activation energies