Question
In: Chemistry
We dissolve 4.44 g of an unknown acid, HA, in enough water to produce 25.0 mL...
We dissolve 4.44 g of an unknown acid, HA, in enough water to
produce 25.0 mL of solution. The pH of this solution of HA(aq) is
1.44. We titrate this solution with a 0.250 M solution of NaOH. It
takes 38.8 mL of the NaOH solution to reach the equivalence point.
The temperature is 25oC.
(a) What is the molar mass of HA?
(b) What is the pKa value of HA(aq)?
(c) What is the pH at the equivalence point?
(d) What is the pH at the midpoint in the titration when you have
as much HA(aq) as A-(aq)?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
A 0.1276 g sample of an unknown monoprotic acid was dissolved in 25.0 mL of water...
A 0.1276 g sample of an unknown monoprotic acid was dissolved in
25.0 mL of water and titrated with 0.0633 M NaOH solution. The
volume of base required to bring the solution to the equivalence
point was 18.4 mL. (a) Calculate the molar mass of the acid. (b)
After 10.0 mL of base had been added during the titration, the pH
was determined to be 5.87. What is the Ka of the unknown acid? (10
points)
You have a 1.153 g sample of an unknown solid acid, HA, dissolved in enough water...
You have a 1.153 g sample of an unknown solid acid, HA,
dissolved in enough water to make 20.00 mL of solution. HA reacts
with KOH(aq) according to the following balanced chemical
equation: HA(aq)+KOH(aq)--->KA(aq)+H2O(l)
if 13.40 mL of 0.715 M KOH is required to titrate the unknown
acid to the equivalence point, what is the concentration of the
unknown acid? ALSO What is the molar mass of HA?
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to...
Assume you dissolve 0.235 g of the weak acid benzoic acid,
C6H5CO2H, in enough water to make 8.00 ✕ 102 mL of solution and
then titrate the solution with 0.158 M
NaOH. C6H5CO2H(aq) + OH-(aq)-->
C6H5CO2-(aq) + H2O(ℓ)
What are the concentrations of the following ions at the
equivalence point? M-Na+=___
M-H3O+=____
M-OH-=____
M-C6H5CO2-=_____
What is the pH of the solution? _____
Assume you dissolve 0.281 g of the weak acid benzoic acid in enough water to make...
Assume you dissolve 0.281 g of the weak acid benzoic
acid in enough water to make 1.00x10^2 mL of solution and then
titrate the solution with 0.171 M NaOH. Ka=6.3x10^-5.
what are the concentrations of Na+ H3O+ OH- and
C6H5CO2-
Assume you dissolve 0.216 g of the weak acid benzoic acid in enough water to make...
Assume you dissolve 0.216 g of the weak acid benzoic acid in
enough water to make 100 mL of solution and then titrate the
solution with 0.144 M . ( Ka for benzoic acid = 6.3 times 10^-5.)
a) What was the pH of the original benzoic acid solution? b) What
are the concentrations of all of the following ions at the
equivalence point: Na, H3O, OH, and C6H5CO2? c) What is the pH of
the solution at the equivalence...
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to...
Assume you dissolve 0.235 g of the weak acid benzoic acid,
C6H5CO2H, in enough water to make 1.00 ✕ 102 mL of solution and
then titrate the solution with 0.168 M NaOH. C6H5CO2H(aq) + OH-(aq)
C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following
ions at the equivalence point?
Na+, H3O+, OH- C6H5CO2-
M Na+ ?
M H3O+ ?
M OH- ?
M C6H5CO2- ?
What is the pH of the solution?
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to...
Assume you dissolve 0.235 g of the weak acid benzoic acid,
C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and
then titrate the solution with 0.133 M NaOH. C6H5CO2H(aq) + OH-(aq)
C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following
ions at the equivalence point? Na+, H3O+, OH- C6H5CO2- Incorrect:
Your answer is incorrect. M Na+ Incorrect: Your answer is
incorrect. M H3O+ Incorrect: Your answer is incorrect. M OH-
Incorrect: Your answer is incorrect....
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to...
Assume you dissolve 0.235 g of the weak acid benzoic acid,
C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and
then titrate the solution with 0.138 M NaOH.
C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ)
What are the concentrations of the following ions at the
equivalence point?
Na+, H3O+ ,OH-
C6H5CO2-
M Na+
M H3O+
M OH-
M C6H5CO2-
What is the pH of the solution?
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to...
Assume you dissolve 0.235 g of the weak acid benzoic acid,
C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and
then titrate the solution with 0.128 M NaOH.
C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ)
What are the concentrations of the following ions at the
equivalence point?
Na+, H3O+, OH-
C6H5CO2-
___M Na+
___M H3O+
___M OH-
___M C6H5CO2-
What is the pH of the solution?
ssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to...
ssume you dissolve 0.235 g of the weak acid benzoic acid,
C6H5CO2H, in enough water to make 4.00 ✕ 102 mL of solution and
then titrate the solution with 0.163 M NaOH. C6H5CO2H(aq) + OH-(aq)
C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following
ions at the equivalence point? Na+, H3O+, OH- C6H5CO2- M Na+ M H3O+
M OH- M C6H5CO2- What is the pH of the solution?
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