In: Chemistry
Calculate the pH at the equivalence point in titrating 0.110 M solutions of each of the following with 8.0×10−2 MNaOH. chlorous acid (HClO2) benzoic acid (C6H5COOH)
Ans- HClO2 -- Ka = 1.1 x 10^-2
At the equivalence point you have an aqueous solution of NaClO2. If
you started with 10.0 mL of 0.110 M HClO2:
mmoles HClO2 = M HClO2 x mL HClO2 = (0.110)(10.0) = 1.1 mmoles
HClO2
The reaction between HClO2 and NaOH is in a 1:1 mole ratio: HClO2 +
NaOH ==> NaClO2 + H2O.
All of the HClO2 will be converted to NaClO2.
1.00 mmoles HClO2 x (1 mmole NaOH / 1 mmole HClO2) = 1.00 mmoles
NaOH
1.00 mmoles NaOH x (1 mL NaOH / 8.0×10−2 mmoles NaOH) =
1.25*10-3 mL NaOH used in the titration. The final
volume is then 10.0 mL + 1.25*10-3 mL = 10 mL.
M NaClO2 = mmoles NaClO2 / mL solution = 1.00 / 10 = 0.1 M NaClO2
at the equivalence point.
The salt solution will be basic (i.e. it was made using a STRONG
BASE and a weak acid). So ClO2- ion will ionize as follows:
Molarity . . . . .ClO2- + H2O <==> HClO2 + OH-
Initial . . . . . . 0.1 0 0
Change . . . . . . .-x . . . . . . . . . . . . . . . .x . . . .
.x
Equilibrium . .0.1-x . . . . . . . . . . . . . x . . . . .x
Kb ClO2- = Kw / Ka HClO2 = (1.0 x 10^-14) / (1.1 x 10^-2) = 9.1 x
10^-13
Kb = [HClO2][OH-] / [ClO2-] = (x)(x) / (0.1-x) = 9.1 x 10^-13
Because Kb is so small, we can neglect the -x term to simplify the
math.
x^2 / 0.1 = 9.1 x 10^-13
x^2 = 9.1 x 10^-14
x = 3.01 x 10^-7 = [OH-]
pOH = -log [OH-] = -log (3.01 x 10^-7) = 6.52
pH = 14.00 - pOH = 14.00 - 6.52 = 7.4
(b) C6H5COOH -- Ka = 6.5 x 10^-5
Like the first problem, C6H5COOH and NaOH will react in a 1:1 mole
ratio and at the equivalence point the concentration of C6H5COONa
will equal 0.1 M. The ICE chart will look the same, too.
Kb C6H5COO- = Kw / Ka C6H5COOH = (1.0 x 10^-14) / (6.5 x 10^-5) =
1.5 x 10^-10
Kb = [C6H5COOH][OH-] / [C6H5COO-] = (x)(x) / (0.1-x) = 1.5 x
10^-10
Again, we can neglect the -x term to get
x^2 / 0.1 = 1.5 x 10^-10
x^2 = 1.5 x 10^-11
x = 3.87x 10^-6 = [OH-]
pOH = -log3.87x 10^-6 = 5.41
pH = 14 - pOH = 8.59