Asked by Anon
How many milliliters of a 0.250 M acetic acid solution must be added to 50.0
mL of a 0.750 M NaOH solution to produce a buffer solution with
pH = 4.500 ?
The pH is given by which we can calculate the concentration of [H+]
How do we approach the problem from there?
mL of a 0.750 M NaOH solution to produce a buffer solution with
pH = 4.500 ?
The pH is given by which we can calculate the concentration of [H+]
How do we approach the problem from there?
Answers
Answered by
DrBob222
Use the Henderson-Hasselbalch equation. Get data from the equation and an ICE chart.
millimoles NaOH = M x mL = apprx 38 but you need a bettr answer than that
millimols CH3COOH = x
.......CH3COOH + NaOH ==> CH3COONa + H2O
I........0.......38.........0.........0
add......x.............................
C.......x+0.....-38.........38.....
E........x........0.........38
Substitute the E line into HH equation and solve for x = millimols CH3COOH.
Then M = millimols/mL
YOu know M and mmols of the acid, solve for mL.
millimoles NaOH = M x mL = apprx 38 but you need a bettr answer than that
millimols CH3COOH = x
.......CH3COOH + NaOH ==> CH3COONa + H2O
I........0.......38.........0.........0
add......x.............................
C.......x+0.....-38.........38.....
E........x........0.........38
Substitute the E line into HH equation and solve for x = millimols CH3COOH.
Then M = millimols/mL
YOu know M and mmols of the acid, solve for mL.
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