Q:

Is it possible for me to derive Avogadro's number? 

To my understanding the mole is the unit used to translate between mass on the atomic level and mass in the macro level, defined as the number of atoms in $12$ grams of Carbon-$12$, which apparently turns out to be $\pu{6.0221409e23}$ atoms, and this was defined as Avogadro's Number. 
How was this number derived?  Is it something I can derive myself?  If I had $12$ grams of Carbon-$12$, how would I be able to deduce that it had $\pu{6.0221409e23}$ atoms? 

A:

To determine Avogadro's number you have to measure the same unit at the atomic and macroscopic scales.  
This was first achieved by Millikan who measured the charge of an electron.  The charge of one mole of electrons was already known and  is a Faraday.  Dividing both, you get Avogadro's number.  
Before that, Josef Loschmidt was the first one to calculate the number of particles in a cubic meter of gas, using the kinetic theory of gases.  
This is, of course, also related to Avogadro's number.  
Avogadro himself did not give any number.  He just stated that equal volumes of different gases at the same pressure and temperature have equal amount of particles.  
A more modern way of doing it is determining the density of an ultra pure element and then determine the number of atoms and their distances in a unit cell with X-ray diffraction.  
So yes, you could, in principle, derive Avogadro's number with pure monocrystalline carbon 12.  You will, however, need very good instrumentation.  
As per the answer to this question on Chemistry SE it might become the other way round.  
The Avogadro number will be absolute (defined, with 0 error) and then the kilogram will be redefined as a function of the number of atoms in a monocrystalline perfect $\ce{^{28}Si}$ sphere. 