ksoccer2
Probably a bot.
Joined: 09 Nov 2006
Posts: 1
|
 Posted: Thu Nov 09, 2006 4:14 am Post subject: 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!
|
|
adrian
Regular
Joined: 20 Apr 2006
Posts: 44
Location: Bucharest, Romania
|
| Posted: Fri Nov 24, 2006 7:51 pm Post subject: |
|
|
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.
|
|
