Asked by Elle
16.72g of sodium acetate trihydride (MW=136 g/mol) is dissolved in 100mL water. To this, 4.00g glacial acetic acid (Ka=2.2x10-5, MW=60.0 g/mol) is added, and distilled water is added to to the 500mL mark. Find the final pH and the molar concentration of the buffer.
Answers
Answered by
DrBob222
What's wrong with using the Henderson-Hasselbalch equation.
By the way, you mean sodium acetate <b>trihydrate</b>
16.72g/molar mass = moles
moles/L = M (the volume you want to use is 0.5L (and not the 100 ml).
4.00g/molar mass
moles /L = M (again use 0.5L for final volume an not some other number).
Then pH = pKa + log (base/acid)
By the way, you mean sodium acetate <b>trihydrate</b>
16.72g/molar mass = moles
moles/L = M (the volume you want to use is 0.5L (and not the 100 ml).
4.00g/molar mass
moles /L = M (again use 0.5L for final volume an not some other number).
Then pH = pKa + log (base/acid)
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