buffer solutions help!

[ksoccer2]

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!

[adrian]

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.