A weak acid is titrated with a strong base and the pH is
measured at each...
A weak acid is titrated with a strong base and the pH is
measured at each interval. It the equivalence point is reached when
30 mL of the base has been added, describe how the pKa of the acid
can be determined.
Solutions
Expert Solution
The method is described for any general monoprotic acid HA
dissociation of weak acid ---
HA
H+ + A-
dissociation constant of HA , Ka =
[H+][A-]/[HA]
when concentrations of both HA and A- are equal
then Ka = [H+]
this is also revealed by the henderson equation.
so pH = pKa when weak acid and it's conjugate base
concetrations are same.This occurs at half equivalence point. For
the given problem half equivalence volume of NaOH is 15 ml. so the
pH value corresponding to 15 ml is noted from the plot , Which is
pKa value of the given weak acid.
Multi protic acids dissociations also can be studied by the
same method.
What is the pH of a weak acid strong base titration after each
of the following additions? Ka for HF is 3.5 x 10-4.
a. 10.0 mL of 0.250 M NaOH added to 15.0 mL of 0.400 M HF
b. 25.0 mL of 0.250 M NaOH added to 35.0 mL of 0.1785 M HF
c. 20.0 mL of 0.250 M NaOH added to 20.0 mL of 0.350 M HF
Please show your work so I can better understand this. thanks!...
Consider a monoprotic weak acid (HA) that is titrated with a strong base. What is the relationship between the strength of the weak acid and the pH of the solution at the equivalence point?
There is no relationship between the strength of the acid and the pH at the equivalence point.
The pH at the equivalence point is always 7 in an acid base titration.
The weaker the acid, the higher the pH at the equivalence point.
The stronger the...
When a weak acid (HA) is titrated with NaOH (a strong base),
(a) what species are present in the weak acid solution before the titration is started?
(b) what species is/are decreasing during the titration?
(c) what species is/are increasing during the titration?
(d) what species is/are not involved in the reaction?
(e) what is meant by the equivalence point?
(f) what important species concentration increases after the equivalence point?
A 25.0 mL of a weak acid is titrated with a strong base (0.1 M).
Calculate the pH of the solution during the titration if the weak
acid concentration is 0.10 M and its Ka = 1.8 x 10-5 and 10.0 mL of
base has been added. (Hint: use Henderson-Hasselbach equation).
a) pH = 4.56
b) pH= 5.28
c) pH= 4.74
An acid with a Ka= 0.000343, is titrated with a
strong base, what would the pH be after half the volume of base
needed to reach the equivalenc point has been added?
Classify each titration curve as representing a strong acid titrated with a strong base, a strong base titrated with a strong acid, a weak acid titrated with a strong base, a weak base titrated with a strong acid, or a polyprotic acid titrated with a strong base. Calculate the pH of the resulting solution if 20.0 mL of 0.200 M HCl(aq) is added to 30.0 mL of 0.200 M NaOH(aq). pH = Calculate the pH of the resulting solution if 20.0 mL...
Weak Acid - Strong Base Titration
Calculate the pH at the given amounts below in the titration.
You are titrating 35.0 mL of .15 M HNO2 with .1 M NaOH
until you reach 100 mL of NaOH added.
For this problem the Ka value is 4.6 x 10-4
a) 0.00 mL NaOH added
b) 30.0 mL NaOH added
c) 60.0 mL NaOH added
d) 100.0 mL NaOH added
What is the approximate pH at the equivalence point of a weak
acid-strong base titration if 25 mL 21) of aqueous formic acid
requires 29.80 mL of 0.0567 M NaOH? Ka =1.8 × 10-4 for
formic acid.
A) 2.46 B) 8.12 C) 11.54 D) 5.88