buffer solutions help!
 

ok the buffer solution we made contained 3.3g of sodium acetate trihydrate, 46mL of DI water, and 4.0mL of 6.0M HC2H3O2. From there we only took a 19mL sample and now I have to find how many mL of HCl would be needed to destroy 19mL of the buffer system........I have no idea on how to go about solving this!

Destroying with HCl means reacting all sodium acetate.
3.3g=0,024 moles sodium acetate.
We will assume that the final buffering solution have 50mL.
Therefore 19 mL involve 19/50*0.024=0.009 moles. we need 0.009 mole of HCl.
May I approximate to 0.01 mole? Thank you.
Now, HCl is at your choice. Pure HCl is gaseous, then we need an aqeuous solution.
The most concentrated solution is around 36%, but I believe we will use more appropriate 0.1N (or 0.1M) solution. The amount will be around 100 mL.
Hope no math mistakes.