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Investigating Indicators
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An indicator solution does what its name suggests – it indicates. In chemistry, a common use of
an indicator is to signal the equivalence point of a reaction between an acid and a base.
Generally, an indicator is itself a weak organic acid or a blend of weak organic acids. The
indicator establishes equilibrium in aqueous solution, which is shifted according to LeChatelier’s
principle as the solution changes in pH. The indicator is one color in the presence of a range of
concentrations of H+ or OH– ions, and another color when the acidity changes. Knowing when an
indicator will change color helps you determine the precise equivalence point of an acid-base
reaction. This knowledge is also important as you select the proper indicator for a given reaction.
OBJECTIVES
In this experiment, you will
• Conduct strong acid-strong base titrations using solutions of hydrochloric acid and sodium
hydroxide, and three different indicator solutions.
• Select the proper indicator to use with a titration involving a weak acid or a weak base,
based on your observations and measurements.
Figure 1
CHOOSING A METHOD
If you choose Method 1, you will conduct the titration in a conventional manner. You will
deliver volumes of NaOH titrant from a buret. You will enter the buret readings manually to
store and graph each pH-volume data pair.
If you choose Method 2, you will use a Vernier Drop Counter to conduct the titration. NaOH
titrant is delivered drop by drop from the reagent reservoir through the Drop Counter slot. After
the drop reacts with the reagent in the beaker, the volume of the drop is calculated and a
pH-volume data pair is stored.
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MATERIALS
Materials for both Method 1 (buret) and Method 2 (Drop Counter)
Vernier computer interface
computer
Vernier pH Sensor
0.10 M NaOH solution
0.10 M HCl solution
0.10 M HC2H3O2 solution
0.10 M NH3 solution
250 mL beaker
50 mL graduated cylinder
magnetic stirrer (if available)
stirring bar or Microstirrer
wash bottle
ring stand
utility clamp
phenolphthalein indicator solution
bromthymol blue indicator solution
methyl orange indicator solutions
distilled water
Materials required only for Method 1 (buret)
50 mL buret
10 mL pipet
buret clamp
Materials required only for Method 2 (Drop Counter)
Vernier Drop Counter
reagent reservoir
5 mL pipet
100 mL beaker
10 mL graduated cylinder
a second 250 mL beaker
METHOD 1: Measuring Volume Using a Buret
1. Obtain and wear goggles.
Part I Strong Acid – Strong Base Titrations
2. Use a graduated cylinder to measure out 20 mL of 0.10 M HCl solution into a 250 mL
beaker. Add exactly two drops of methyl orange indicator solution to the beaker of HCl
solution. CAUTION: Handle the hydrochloric acid with care. It can cause painful burns if it
comes in contact with the skin.
3. Place the beaker on a magnetic stirrer and add a stirring bar. If no magnetic stirrer is
available, stir the reaction mixture with a stirring rod during the titration.
4. Connect a pH Sensor to Channel 1 of the Vernier computer interface.
5. Use a utility clamp to suspend the pH Sensor on a ring stand as shown in Figure 1. Position
the pH Sensor in the HCl solution and adjust its position so that it is not struck by the stirring
bar.
6. Rinse and fill the buret with 0.10 M NaOH solution. CAUTION: Sodium hydroxide solution
is caustic. Avoid spilling it on your skin or clothing.
7. Start the Logger Pro program on your computer. Open the file “11a Indicators” from the
Advanced Chemistry with Vernier folder.
8. You are now ready to begin the titration. Conduct the titration carefully, as described below.
Watch carefully to see if the indicator changes color before, at the same time, or after the
rapid change in pH at the equivalence point. If this is a suitable indicator for the reaction, it
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should change color at about the same time as the jump in pH occurs. In your data table,
record the volume when the indicator changes color.
a. Before you have added any NaOH solution, click
. Once the displayed pH reading
has stabilized, click
. In the edit box, type “0” (for 0 mL added). Press the ENTER
key to store the first data pair for this experiment.
b. Add 1 mL of the NaOH titrant. When the pH stabilizes, click
. In the edit box, type
the current buret reading. Press ENTER. You have now saved the second data pair for the
experiment.
c. Continue adding NaOH solution 1 mL at a time, and enter the buret reading after each
increment, until the pH of the mixture is about 5.
d. Add NaOH in 0.5 mL increments until the pH is about 10.
e. Continue adding NaOH solution in 1 mL increments until the pH value remains constant.
9. When you have finished collecting data, click
.
10. Dispose of the reaction mixture as directed. Rinse the pH Sensor with distilled water in
preparation for the next titration.
11. Label the point on your graph where the indicator solution changes color and describe the
color change. To do this, choose Text Annotation from the Insert menu. Print a copy of the
titration curve.
12. Repeat the necessary steps to conduct a second and third trial, using the bromthymol blue and
phenolphthalein indicator solutions. Repeat Step 11 to analyze the titration curve for your
second and third trials.
Part II Select an Appropriate Indicator for the Titration of a Weak Acid or a Weak Base
13. Obtain a weak acid or weak base solution from your instructor. If you are testing a weak
acid, use the 0.10 M NaOH solution as the titrant. If you are testing a weak base, rinse and
fill your buret with the weak base solution, and titrate 20 mL of 0.10 M HCl solution. Use the
results of your previous tests to select the appropriate indicator solution for this trial. Conduct
the trial using the same procedure as before. Label the point on your graph where the
indicator solution changes color and describe the color change. Print a copy of the titration
curve.
METHOD 2: Measuring Volume Using a Drop Counter
1. Obtain and wear goggles.
Part I Strong Acid – Strong Base Titrations
2. Add 40 mL of distilled water to a 100 mL beaker. (You can add less, about 20 mL, if you
will be using a stirring bar instead of the Microstirrer.) Use a pipet bulb (or pipet pump) to
pipet 5.00 mL of the HCl solution into the 100 mL beaker with distilled water. Add exactly
one drop of methyl orange indicator solution to the beaker of HCl solution. CAUTION:
Handle the hydrochloric acid with care. It can cause painful burns if it comes in contact with
the skin.
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Figure 2
3. Lower the Drop Counter plate onto a ring stand and clamp it into position (see Figure 2).
4. Connect the Drop Counter to DIG/SONIC 1 of the Vernier computer interface. Connect the
pH Sensor to CH 1 of the interface.
5. Start the Logger Pro program on your computer. Open the file “11b Indicators (Drop
Count)” from the Advanced Chemistry with Vernier folder.
6. Obtain the plastic 60 mL reagent reservoir. Close both valves by turning the handles to a
horizontal position. Follow the steps below to set up the reagent reservoir for the titration.
a. Rinse the reagent reservoir with a few mL of the 0.10 M NaOH solution and pour the
NaOH into an empty 250 mL beaker.
b. Use a utility clamp to attach the reservoir to the ring stand.
c. Fill the reagent reservoir with slightly more than 60 mL of the 0.100 M NaOH solution.
d. Place the 250 mL beaker, which contains the rinse NaOH, beneath the tip of the reservoir.
e. Drain a small amount of the NaOH solution into the 250 mL beaker so that it fills the
reservoir’s tip. To do this, turn both valve handles to the vertical position for a moment,
then turn them both back to horizontal.
f. Discard the drained NaOH solution in the 250 mL beaker as directed.
7. Calibrate the drops that will be delivered from the reagent reservoir. Note: If you are using
the stored calibration (20 drops per mL), then skip this step.
a. Choose Calibrate ` DIG 1: Drop Counter (mL) from the Experiment menu.
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b. Proceed by one of these two methods:
• If you have previously calibrated the drop size of your reagent reservoir and want to
continue with the same drop size, select the Manual button, enter the number of
. Then proceed directly to Step 8.
Drops/mL, and click
• If you want to perform a new calibration, select the Automatic button, and continue
with Step c below.
c. Place a 10 mL graduated cylinder directly below the slot on the Drop Counter, lining it up
with the tip of the reagent reservoir.
d. Open the bottom valve on the reagent reservoir (vertical). Keep the top valve closed
(horizontal).
e. Click the Start button.
f. Slowly open the top valve of the reagent reservoir so that drops are released at a slow rate
(~1 drop every two seconds). You should see the drops being counted on the computer
screen.
g. When the volume of the NaOH solution in the graduated cylinder is between 9 and 10 mL,
close the bottom valve of the reagent reservoir.
h. Enter the precise volume of NaOH (read to the nearest 0.01 mL) in the edit box. Record
the number of Drops / mL displayed on the screen for possible future use.
i. Click
. Discard the NaOH solution in the graduated cylinder as directed, and set the
graduated cylinder aside.
8. Assemble the apparatus as shown in Figure 2.
a. Place the magnetic stirrer on the base of the ring stand.
b. Insert the pH Sensor through the large hole in the Drop Counter.
c. Attach the Microstirrer to the bottom of the pH Sensor. Rotate the paddle wheel of the
Microstirrer, and make sure that it does not touch the bulb of the pH Sensor.
d. Adjust the positions of the Drop Counter and reagent reservoir so they are both lined up
with the center of the magnetic stirrer.
e. Lift up the pH Sensor, and slide the 100 mL beaker containing the HCl solution (from
Step 2) onto the magnetic stirrer. Lower the pH Sensor into the beaker.
f. Adjust the position of the Drop Counter so that the Microstirrer on the pH Sensor is just
touching the bottom of the beaker.
g. Adjust the reagent reservoir so its tip is just above the Drop Counter slot.
9. Turn on the magnetic stirrer so that the Microstirrer is stirring at a fast rate.
. No data will be collected until the
10. You are now ready to begin collecting data. Click
first drop goes through the Drop Counter slot. Fully open the bottom valve. The top valve
should still be adjusted so drops are released at a rate of about 1 drop every 2 seconds. When
the first drop passes through the Drop Counter slot, check the data table to see that the first
data pair was recorded.
11. Watch carefully to see if the indicator changes color before, at the same time, or after the
rapid change in pH at the equivalence point. Note: Volume is displayed in the live table. If
this is a suitable indicator for the reaction, it should change color at about the same time as
the jump in pH occurs. Note the volume when the indicator changes color.
12. After the jump in pH occurs, continue to deliver about 3 more milliliters of NaOH solution,
then click
. Turn the bottom valve of the reagent reservoir to a closed (horizontal)
position. Dispose of the beaker contents as directed.
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13. Label the point on your graph where the indicator solution changes color and describe the
color change. To do this, choose Text Annotation from, the Insert menu. Print a copy of the
titration curve.
14. Repeat the necessary steps to conduct a second and third trial, using the bromthymol blue and
phenolphthalein indicator solutions. Repeat Step 13 to analyze the titration curve for your
second and third trials.
Part II Select an Appropriate Indicator for the Titration of a Weak Acid or a Weak Base
15. Obtain a weak acid or weak base solution from your instructor. If you are testing a weak
acid, use the 0.10 M NaOH solution as the titrant. If you are testing a weak base, rinse and
fill your reagent reservoir with the weak base solution, and titrate 5 mL of 0.10 M HCl
solution. Use the results of your previous tests to select the appropriate indicator solution for
this trial. Conduct the trial using the same procedure as before. Label the point on your graph
where the indicator solution changes color and describe the color change. Print a copy of the
titration curve.
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REPORT SHEET
Name__________________________Date______
Attach your graphs to this sheet
1. Describe how the three indicator solutions worked in the titrations.
2. Which indicator solution is the best for a strong acid-strong base titration? Specify the
color changes and the pH readings where the color changes occurred.
3. For which type of acid-base titrations would the other two indicator solutions be best
suited? Explain.
4. Use the graphs to compare how accurately the indicator solutions “indicated” the
equivalence point of the titrations that you conducted. In your judgment, can an indicator
alone accurately determine the equivalence point of an acid-base reaction? Explain.
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