how would you make a 50 ml of a 10% acetic acid solution from
a 30% acetic acid solution? (i.e., what volume of 30% stock
solution and what volume of water would you use?)
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?
a 25.0mL solution containing 0.60 M HC2H3O2(acetic acid) was
titrated with 0.50 M NaOH. Ka of acetic acid is 1.8*10^-5
Calculate pH at initial volume(0mL added)
Calculate pH at 1/2 equivalence point.
Calculate pH at equivalence point.
Calculate pH at 20.00 mL
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...