A 25.0 mL sample of 0.35 M lactic acid, HC3H5O3, is titrated
with 0.070 M KOH....
A 25.0 mL sample of 0.35 M lactic acid, HC3H5O3, is titrated
with 0.070 M KOH. Determine the pH of the solution at the
equivalence point and at half-way to equivalence point. The Ka of
lactic acid is 1.38x10^-4.
Applications of Aqueous Equilibria: A 25.0 mL sample of 0.100 M
lactic acid (HC3H5O3, Ka = 1.38 X 10^-4) is titrated with a 0.100 M
barium hydroxide. Calculate the pH after the addition of 0.0 mL,
2.0 mL, 4.0 mL, 6.25 mL, 10.0 mL, 12.0 mL, 12.25 mL, 12.5 mL, 13.0
mL, 14.0 mL, and 15.0 mL of the Ba(OH)2
A 25.0 mL sample of 0.30 M HCOOH is titrated with 0.20 M KOH.
What is the pH of the solution after 25.0 mL of KOH has been added
to the acid? Ka = 1.8x10^-4
A 25.0-mL solution of 0.100 M acetic acid is titrated with a
0.200 M KOH solution. Calculate the pH after the following
additions of the KOH solution:
a) 0.0 mL b) 5.0 mL c) 10.0 mL d) 12.5 mL e) 15.0 mL
Calculate the pH of 25.0 mL of 0.110 M aqueous lactic acid being
titrated with 0.150 M NaOH(aq) [See text for Ka value.]
(a) initially
(b) after the addition of 5.0 mL of base
(c) after the addition of a 5.0 mL more of base, Vt=10.0mL
(d) at the equivalence point
(e) after the addition of 5.0 mL of base beyond the equivalence
point
(f) after the addition of 10.0 mL of base beyond the equivalence
point
(g) Pick a...
2)
A 25.0 mL sample of 0.160 M KOH is titrated with 0.250 M
HCl.
Determine the following quantities:
a)
The initial pH of the KOH solution before any acid is added.
b)
The pH of the solution after 3.00 mL of HCl is added.
c)
The quantity of HCl solution required to reach the
equivalence
point.
d)
The pH of the solution at the equivalence point.
e)
The pH of the solution after20.0 mL of HCl is added.
A 25.0 mL sample of a 0.110 M solution of acetic acid is
titrated with a 0.138 M solution of NaOH. Calculate the pH of the
titration mixture after 10.0, 20.0, and 30.0 mL of base have been
added. The Ka for acetic acid is 1.76x10^-5.
A 25.0 mL sample of 0.150 M hydrazoic acid (HN3) is titrated
with a 0.150 M NaOH solution. Calculate the pH at equivalence and
the pH after 26.0 mL of base is added. The Ka of hydrazoic acid is
1.9x10^-5.
A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a
0.150 M NaOH solution. What is the pH at the equivalence point? The
Ka of hydrofluoric acid is 6.8 × 10-4.
A 25.0 mL sample of 0.100 M acetic acid is titrated with a 0.125
M NaOH solution. Calculate the pH of the mixture after 10, 20, and
30 ml of NaOH have been added (Ka=1.76*10^-5)
9.
A buffer is made by mixing 85 mL of 0.13 M lactic acid (HC3H5O3)
with 95 mL of 0.15 M sodium lactate.
a. Calculate the pH of the buffer.
b. Calculate the pH after 3.0 mL of a 0.20 M HCl solution is
added to the buffer.
c. Calculate the pH after 3.0 mL of a 0.20 M NaOH solution is
added to the buffer INSTEAD of the HCl solution.
d. Calculate the pH of the buffer solution if...