1. If you get to the end point of your titration and wait a few hours, you'll find that the color has disappeared. What has happened? Write the chemical equations for the reactions involved in this delayed color change. (Hint: See the note at the end of Step 12 in the Procedure Section of this experiment.) 2. Why do we titrate into a flask and not a beaker? 3. What effect would each of the following errors have on the determined concentration of th unknown acid? Would the calculated result be erroneously high, erroneously low, or unaffected a You forgot to condition the buret and it contained some deionized water before you added the NaOH. Circle one: too low / unaffected / too high b. The Erlenmeyer flask was wet with deionized water before you added the acid to it. Circle one: too low / unaffected / too high C. You forgot to condition the pipet before using it to transfer the acid to the flask. Circle one: too low / unaffected / too high / depends d. The final buret reading was mistakenly recorded too high (e.g., recorded as 35.00 m instead of the actual 30.00 mL). Circle one: too low / unaffected/too high Based on the true molarity of your acetic acid unknown, and assuming that its density solution is 1.01 g/mL, calculate the mass percent of acetic acid in your unknown.
1. If you get to the end point of your titration and wait a few hours, you'll find that the color has disappeared. What has happened? Write the chemical equations for the reactions involved in this delayed color change. (Hint: See the note at the end of Step 12 in the Procedure Section of this experiment.) 2. Why do we titrate into a flask and not a beaker? 3. What effect would each of the following errors have on the determined concentration of th unknown acid? Would the calculated result be erroneously high, erroneously low, or unaffected a You forgot to condition the buret and it contained some deionized water before you added the NaOH. Circle one: too low / unaffected / too high b. The Erlenmeyer flask was wet with deionized water before you added the acid to it. Circle one: too low / unaffected / too high C. You forgot to condition the pipet before using it to transfer the acid to the flask. Circle one: too low / unaffected / too high / depends d. The final buret reading was mistakenly recorded too high (e.g., recorded as 35.00 m instead of the actual 30.00 mL). Circle one: too low / unaffected/too high Based on the true molarity of your acetic acid unknown, and assuming that its density solution is 1.01 g/mL, calculate the mass percent of acetic acid in your unknown.
Chapter8: Polyfunctional Acids And Bases
Section: Chapter Questions
Problem 10P
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Transcribed Image Text:0100L
34хота OT NEOR
OO HRI
Data Table and Results
Molarity of NaOH: 3455M
125FF-In
or
Volume of acid added to
flask
Initial buret reading
Final buret reading
X
molaceuc acid
Volume of base titrated into
flask*
TmName:
Naon+Call30
0.01000L
10.00
Trial 1
Experiment 12 | Titration
Macy huffort
1000ML
AV-VF-Vi
DEPORT
Trial 2
H₂O+NaC₂H30₂
Unknown #:
True molarity: 700M
Trial 3
10.0mi10.0m² 10.0m
0.021.19426.09
21.01.m42.38m4 47.18mL
21.01mL 21.19m 21.09m
Calculated molarity of acetic 0.7259M 0.7321M0.7287M
acid in your unknown
*Final buret reading - Initial buret reading.
Calculate the molarity of acetic acid in your unknown for each trial and show a sample calculation
below. (Your instructor may require that you show the calculations for all trials. If so, attach them
on a separate piece of paper, if necessary.)
triala:
thal 3
trial 1:*
(0.3455 21.09
(0.3455x210122=0.7259M
0.3455x2119
10.00
Trial 4
(if needed)
Trial 5
(if needed)
= 0.7289M
10.00
0.7323M
=0.7287M
Choose the three trials that have molarities that agree within 1% of one another and use these three
molarities to calculate your average molarity.
1(0.7259+0.7321+0.7287)
3
Obtain the true molarity for your acetic acid solution from your instructor and record it at the top of
your data table below the unknown number. Using the average molarity that you calculated above,
calculate the percent error for your unknown.
(0.7289-0.700)
*100=4.13%.
0700
Transcribed Image Text:Name:
Post-Lab Questions
1. If you get to the end point of your titration and wait a few hours, you'll find that the color has
disappeared. What has happened? Write the chemical equations for the reactions involved in
this delayed color change. (Hint: See the note at the end of Step 12 in the Procedure Section of
this experiment.)
2. Why do we titrate into a flask and not a beaker?
a
150 med Experiment 12 | Titration
3. What effect would each of the following errors have on the determined concentration of the
unknown acid? Would the calculated result be erroneously high, erroneously low, or unaffected?
C.
You forgot to condition the buret and it contained some deionized water before you
added the NaOH. Circle one: too low / unaffected / too high
b.
The Erlenmeyer flask was wet with deionized water before you added the acid to it.
Circle one: too low / unaffected / too high
You forgot to condition the pipet before using it to transfer the acid to the flask.
Circle one: too low / unaffected / too high / depends
d. The final buret reading was mistakenly recorded too high (e.g., recorded as 35.00 ml
instead of the actual 30.00 mL). Circle one: too low / unaffected/too high
4. Based on the true molarity of your acetic acid unknown, and assuming that its density of the
solution is 1.01 g/mL, calculate the mass percent of acetic acid in your unknown.
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