Posted by **Anonymous** on Wednesday, October 23, 2013 at 11:03pm.

A 30 mL sample of .165 M propanoic acid is titrated with .300M KOH. Calculate the pH at each volume of added base: 0 mL, 5 mL, 10, equivalence point, one-half equivalence point, 20 mL, 25 mL. Use calculations to make a sketch of the titration curve.

- chemistry -
**DrBob222**, Wednesday, October 23, 2013 at 11:28pm
eq pt.

mL acid x M acid = mL KOH x M KOH

Solve for mL KOH.

0 mL:

.........HPr ==> H^+ + Pr^-

I......0.165.....0.....0

C.........-x......x....x

E.......0.165-x...x....x

Ka = (H^+)(Pr^-)/(HPr).

Substitute from the E line and solve for x = (H^+), then convert to pH.

For additions up to but not including eq pt use the Henderson-Hasselbalch equation.

For the eq pt the pH is determined by the hydrolysis of the salt. (salt) = (Pr^-) = (0.165 x 30 mL)/(total mL) where total mL = 30 + mL to eq pt. I will call this 0.1 M but you need to do it more accurately

........Pr^- + HOH ==> HPr + OH^-

I......0.1..............0.....0

C........-x.............x.....x

E......0.1-x............x.....x

Kb for Pr^- = (Kw/Ka for acid) = (x)(x)/(0.1-x). Solve for x = (OH^-) and convert to pH.

For all points past the eq pt it will be excess OH^-.

mols base = M x L

mols acid to eq pt = ?

excess OH^- = difference.

(OH^-) = mols OH excess/total L.

Then convert to pH.

- chemistry -
**Sam Dowen**, Tuesday, November 22, 2016 at 8:09pm
2.8?

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