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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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michelecul michelecul
wrote...
11 years ago
You wish to prepare 100 mL (TOTAL volume!) of a buffer solution that is .025 M in carbonic acid, pH 7.25.  You have solid H2CO3 and solid NaHCO3.  Calculate how many grams of H2CO3 and HCO3- you need to prepare this solution.

I'm pretty sure you use henderson-hasselbach, but am still really confused!  Thanks!
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wrote...
#1
11 years ago
7.25=6.36 +log (base/acid)
0.89= log (base/acid)
7.76=base/acid
base=(7.76/8.76) *0.025M/0.1L=0.2214M NaHCO3
acid=(1/8.76) * 0.025M/0.1L=0.0285M H2CO3
Need 0.1L*0.025M NaHCO3=  0.0025 moles NaHCO3
Convert that number of moles of NaHCO3 to grams and you should be good to go.  (0.0025 * molar mass of NaHCO3)

Check my math on all this, we're probably taking the same level class.
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