In: Chemistry
A 45.00 -mL sample contains
0.754 g of
KHC8H4O4, known as
KHP . This sample is used to standardize an NaOH solution.
At the equivalence point, 43.30 mL of NaOH have
been added.
Ka(
HC8H4O4-)
= 3.9E-6
a) What was the concentration of the NaOH?
b) What is the pH at the equivalence point?
Answer –
We are given, mass of KHC8H4O4 = 0.754 g , volume = 45.00 mL = 0.045 L
First we need to calculate the moles of KHC8H4O4
Moles of KHC8H4O4 = 0.754 g / 204.22 g.mol-1
= 0.00369 moles
[KHC8H4O4] = 0.00369 moles / 0.045 L
= 0.0820 M
a) At the equivalence point , moles of KHC8H4O4 = moles of NaOH
So, moles of NaOH = 0.00369 moles
Concentration of the [NaOH] = 0.00369 moles / 0.04330 L
= 0.0853 M
b) pH at the equivalence point
at the equivalence point, moles of KHC8H4O4 = moles of NaOH
so,
KHC8H4O4 (aq) + NaOH (aq) ----> NaKC8H4O4 (aq) + H2O
0.00369 0.00369 0.00369
Moles of NaKC8H4O4 (aq) = moles of KC8H4O4- (aq) = 0.00369 moles
Total volume = 45 + 43.30 = 88.30 mL
So, [KC8H4O4- (aq)] = 0.00369 mole / 0.0883 L
= 0.0418 M
Now we need to put ICE table
KC8H4O4- (aq) + H2O --------> KHC8H4O4 (aq) + OH-
I 0.0418 M 0 0
C -x +x +x
E 0.0418-x +x +x
We need to calculate Kb from Ka
We know, Ka * Kb = 1*10-14
So, Kb = 1*10-14 / 3.9*10-6
= 2.56*10-9
So, Kb = [KHC8H4O4(aq)] [OH-] / [KC8H4O4-(aq)]
2.56*10-9 = x *x / 0.0418-x
We can neglect x in the 0.0418-x, because Kb value is too small
So,
2.56*10-9 * 0.0418 = x2
x = 1.035*10-5 M
x = [OH-] = 1.035*10-5 M
so, pOH = -log [OH-]
= - log 1.035*10-5 M
= 4.98
So, pH = 14-pOH
= 14 – 4.98
= 9.02