B) How many moles of KHP were used? C) What volume of NaOH was needed? D) What it the molarity of the standardized NaOH solution?

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Story
base
Students were asked to perform a lab to identify an unknown acid.
The experiment has several parts.
First the students had to make a sodium hydroxide solution with a molarity of approximately 0.2M.
Then the students had to perform a titration with potassium hydrogen phthalate to standardize their
solution.
Finally they had to perform a titration with the unknown acid to find the pKa and the molar mass, then
using their data they had to determine which of the weak acids they had used.
Part 1) Make a sodium hydroxide solution
A student measured 4.03 grams of NaOH in a tared weigh boat. They then dissolved it into approximately 200 mL
of deionized water in a beaker. Once it was completely dissolved the student poured the solution into a 500.0 mL
volumetric flask. The student rinsed the beaker with deionized water and added the rinse water to the volumetric
flask. They repeated with process, adding the rinse water to the volumetric flask again, they mixed this thoroughly.
Finally, they filled the volumetric flask with distilled water, mixing and then waited for the solution to reach room
temperature before topping off the solution.
A) Calculate the theoretical molarity of the NaOH solution.
M = mol
Nuot
4.03g
X
1 ml NaOll
Nabit
39.9985
Part 2) Standardize the NaOH solution.
NaOH is a hygroscopic solid, which means that it can absorb water from its surroundings, therefore it is important
to determine the actual concentration of the sodium hydroxide solution. To do this the sodium hydroxide solution
is titrated with potassium hydrogen phthalate, (KHC8H404, Molar mass = 204.23g/mol). KHP is a stable
monoprotic solid acid. 1.04 grams of potassium hydrogen phthalate was dissolved into 100.0 mL of water, 2 drops
of indicator was added. This was then titrated with the sodium hydroxide solution that was made in part 1. The
initial reading of the buret was 1.23 mL and at the equivalence point in the titration 28.74 mL was the reading on
the base buret.
0.100755 rol Nooit
NaOH(aq) + KHC8H404 (aq) NaKC8H404(aq) + H₂O
OH(aq) + HC8H404°(aq) ⇒ C8H404² (aq) + H₂O)
B) How many moles of KHP were used?
C) What volume of NaOH was needed?
D) What it the molarity of the standardized NaOH solution?
L
netges od
08 (8
Part 3) Determine the identity of a unknown solid
The standardized solution of NaOH was then used to determine the identity of an unknown acid. 0.785 grams of
the unknown monoprotic acid was titrated using 23.55 mL of the sodium hydroxide solution. The graph below was
created.
HA(aq) + OH(aq) = H₂O + A (aq)
Transcribed Image Text:Story base Students were asked to perform a lab to identify an unknown acid. The experiment has several parts. First the students had to make a sodium hydroxide solution with a molarity of approximately 0.2M. Then the students had to perform a titration with potassium hydrogen phthalate to standardize their solution. Finally they had to perform a titration with the unknown acid to find the pKa and the molar mass, then using their data they had to determine which of the weak acids they had used. Part 1) Make a sodium hydroxide solution A student measured 4.03 grams of NaOH in a tared weigh boat. They then dissolved it into approximately 200 mL of deionized water in a beaker. Once it was completely dissolved the student poured the solution into a 500.0 mL volumetric flask. The student rinsed the beaker with deionized water and added the rinse water to the volumetric flask. They repeated with process, adding the rinse water to the volumetric flask again, they mixed this thoroughly. Finally, they filled the volumetric flask with distilled water, mixing and then waited for the solution to reach room temperature before topping off the solution. A) Calculate the theoretical molarity of the NaOH solution. M = mol Nuot 4.03g X 1 ml NaOll Nabit 39.9985 Part 2) Standardize the NaOH solution. NaOH is a hygroscopic solid, which means that it can absorb water from its surroundings, therefore it is important to determine the actual concentration of the sodium hydroxide solution. To do this the sodium hydroxide solution is titrated with potassium hydrogen phthalate, (KHC8H404, Molar mass = 204.23g/mol). KHP is a stable monoprotic solid acid. 1.04 grams of potassium hydrogen phthalate was dissolved into 100.0 mL of water, 2 drops of indicator was added. This was then titrated with the sodium hydroxide solution that was made in part 1. The initial reading of the buret was 1.23 mL and at the equivalence point in the titration 28.74 mL was the reading on the base buret. 0.100755 rol Nooit NaOH(aq) + KHC8H404 (aq) NaKC8H404(aq) + H₂O OH(aq) + HC8H404°(aq) ⇒ C8H404² (aq) + H₂O) B) How many moles of KHP were used? C) What volume of NaOH was needed? D) What it the molarity of the standardized NaOH solution? L netges od 08 (8 Part 3) Determine the identity of a unknown solid The standardized solution of NaOH was then used to determine the identity of an unknown acid. 0.785 grams of the unknown monoprotic acid was titrated using 23.55 mL of the sodium hydroxide solution. The graph below was created. HA(aq) + OH(aq) = H₂O + A (aq)
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