Question

A
22.5 mL sample of an acetic acid solution is titrated with a 0.175M
NaOH solution. The equivalence point is reached when 37.5 mL of the
base is added.

What was the concentration of acetic acid in the original
(22.5mL) sample?

What is the pH of the equivalence point?

Ka acetic acid= 1.75E-5

Answer #1

A 25 mL aliquot of an HCl solution is titrated with 0.100 M
NaOH. The equivalence point is reached after 21.27 mL of the base
were added. Calculate the concentration of the acid in the original
solution, the pH of the original HCl solution and the original NaOH
solution

A 25.0 mL sample of a 0.115 M solution of acetic acid is
titrated with a 0.144 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 1.76 x 10^-5).
10.0 mL of base =
20.0 mL of base =
30.0 mL of base =

A 25.00-mL sample of propionic
acid, HC3H5O2, of unknown concentration
A 25.00-mL sample of propionic
acid, HC3H5O2, of unknown
concentration was titrated
with 0.151 M KOH. The equivalence
point was reached when was titrated
with 0.151 M KOH. The equivalence
point was reached when 41.28 mL of
base had been added. What is the pH at the equivalence point?
41.28 mL of base had been added. What is
the pH at the equivalence point? Ka for propionic acid is
1.3×10–5 at 25°C.Ka for propionic acid is
1.3×10–5 at 25°C.
Select one:
a. 8.93
b. 7.65
c. 9.47
d. 5.98
e. 9.11

A student performs the following experiment: 25.0 mL of 0.1 M
acetic acid is titrated to the equivalence point with 25.0 mL of
0.1 M NaOH. Calculate the pH at the equivalence point. The
equilibrium constant Ka for acetic acid is 1.8*10^-5. Compare this
value with the experimental value.
Experimental value for acetic acid is pH = 8.8 and volume of
base = 24 mL at equivalence point.

A certain weak acid, HA, with a Ka value of 5.61×10−6,
is titrated with NaOH. More strong base is added until the
equivalence point is reached. What is the pH of this solution at
the equivalence point if the total volume is 40.0 mL ?

A 32.44 mL sample of 0.202M acetic acid is titrated with 0.185 M
sodium hydroxide. Calculate the pH of the solution 1. before any
NaOH is added 2. after 24.00 mL of NaOH is added 3. at the
equivalence point

1. When a 19.6 mL sample of a
0.498 M aqueous acetic acid
solution is titrated with a 0.343 M aqueous
potassium hydroxide solution,
what is the pH after 42.7 mL of potassium
hydroxide have been added?
pH=
2.What is the pH at the equivalence point in the titration of a
22.2 mL sample of a 0.413 M
aqueous acetic acid solution with a
0.500 M aqueous potassium
hydroxide solution?
pH=

A 20.00-mL sample of formic acid (HCO2H) is titrated with a
0.100 M solution of NaOH. To reach the endpoint of the titration,
30.00 mL of NaOH solution is required. Ka = 1.8 x
10-4
What is the pH of the solution after the addition of 10.00 mL of
NaOH solution?
What is the pH at the midpoint of the titration?
What is the pH at the equivalence point?

A
sample of acetic acid (weak acid) was neutralized with .05M NaOH
solution by titration. 34 mL of NaOH had been used. Show your work.
CH3COOH + NaOH-----CH3COONa + H2O
a) Calculate how many moles of NaOH were used?
b) How many moles of aspirin were in a sample?
c) Calculate how many grams of acetic acid were in the
sample
d) When acetic acid is titrated with NaOH solution what is the
pH at the equivalence point? Circle the...

A certain weak acid, HA, with a Ka value of 5.61×10−6, is
titrated with NaOH.
1)A solution is made by titrating 9.00 mmol (millimoles) of HA
and 1.00 mmol of the strong base. What is the resulting pH?
2)More strong base is added until the equivalence point is
reached. What is the pH of this solution at the equivalence point
if the total volume is 41.0 mL ?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 5 minutes ago

asked 5 minutes ago

asked 10 minutes ago

asked 14 minutes ago

asked 14 minutes ago

asked 20 minutes ago

asked 25 minutes ago

asked 27 minutes ago

asked 32 minutes ago

asked 33 minutes ago

asked 39 minutes ago

asked 50 minutes ago