In an acid base titration experiment, 50.0 ml of a 0.0500 m
solution of acetic acid ( ka =7.5 x 10^-5) was titrated with a
0.0500 M solution of NaOH at 25 C. The system will acquire this pH
after addition of 20.00 mL of the titrant:
Answer is 4.581
Please show all work
For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M
sodium hydroxide, determine the pH when:
(a) 50.0 mL of base has been added.
(b) 75.0 mL of base has been added.
(c) 100.0 mL of base has been added.
50.0 ml of an acetic acid (CH3COOH) of unknown
concentration is titrated with 0.100 M NaOH. After 10.0 mL of the
base solution has been added, the pH in the titration flask is
5.30. What was the concentration of the original acetic acid
solution? (Ka(CH3COOH) = 1.8 x
10-5)
How many mL of 0.200 M HBr acid would be needed to neutralize
50.0 grams of calcium hydroxide solid that is completely dissolved
in enough water to make 500. mL of solution?
You would like to make 100.00 mL of a 4.76 pH acetic
acid/acetate buffer, in which the acid concentration is 0.070M.
Write the reaction of the buffer with HCl solution. How many mL of
0.100 M HCl can react with the buffer before it is exhausted? And
Write the reaction of the buffer with NaOH solution. How many mL of
0.100 M NaOH can react with the buffer before it is exhausted?
You mix 50.0 mL of a weak monoprotic acid with 50.0 mL of NaOH
solution in a coffee cup calorimeter. Both solutions (and the
calorimeter) were initially at 22.0C. The final
temperature of the neutralization reaction was determined to be
22.5C.
a) What is the total amount of heat evolved in this reaction?
Show all work.
b) If 0.135 moles of the monoprotic acid were neutralized in
this reaction, what is the molar heat of neutralization (enthalpy)
for this reaction?
If you started with an acetic acid solution of 2.0 mL of 0.84M
Acetic acid and shifted it with 0.2mL of 0.01M HCl (4 drops), what
is the new pH?.
Initial pH
Final pH
Ka of acetic acid = 1.8 x
10-50.3
Start by finding the equilibrium concentrations of the acetic
acid solution. Calculate the Ph based on this initial concentration
(initial Ph).
Calculate the moles of everything (compounds in the equilibrium
AND the acid). Shift the equilibrium with the...
You titrate 50.0 mL of 0.100 M benzoic acid (C6H5COOH) with
0.250 M KOH. What is the pH of the final solution at the
equivalence point? Ka of C6H5COOH = 6.3 x 10-5.
If all work could be shown I would appreciate it! I'm super
confused.
6. You mix 50.0 mL of a weak monoprotic acid with 50.0 mL of
NaOH solution in a coffee cup calorimeter. Both solutions (and the
calorimeter) were initially at 22.0OC. The final temperature of the
neutralization reaction was determined to be 22.5OC. a) What is the
total amount of heat evolved in this reaction? Show all work. b) If
0.135 moles of the monoprotic acid were neutralized in this
reaction, what is the molar heat of neutralization (enthalpy) for
this...
In a buffer solution prepared from 10 mL of 3.0 M benzoic acid
(HC6H5CO2) added to 20 mL of a 2.0
M sodium benzoate (NaC6H5CO2) and
diluted to a total volume of 200mL- Calculate each of the
following:
a. The original pH of the buffer solution
b. The pH upon addition of 8.0 mL of 2.0 M NaOH to part a
c. The pH upon addition of 30.0 mL of 2.0 M HCl to part a