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Acid-Base Titration Lab Report Gum

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Gunner Gum

on 14 May 2014

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Transcript of Acid-Base Titration Lab Report Gum

Step 1
Step 2
Step 3
Reference 1
Reference 2
Reference 3
Reference 4
Grade and Comments
Great Job!
magnetic stirrer
LabQuest App
stirring bar
Vernier pH Sensor
wash bottle
HCl solution
distilled water
~0.1 M NaOH solution
The purpose of the lab was to titrate HCL. with NaOH to find the concentration of HCL.

If I add a certain amount of NaOH, then I'll be able to find the concentration of HCL
Lab Group
Gwen Cockrum
Karina Moreno
2nd Hour Chemistry
Mrs. Seger
Evaluation of Data
Titration Lab Report
Place then. beaker on a
magnetic stirrer and add a stirring bar

Connect the pH Sensor to LabQuest
Set up the data-collection mode

Use a utility clamp to suspend a pH Sensor on a ring stand as shown in Figure 2. Position the pH Sensor in the HCl solution and adjust its position so that it is not struck by the stirring bar.
Step 4
Obtain and wear goggles.

ring stand
pipet bulb or pump
1 utility clamp
250 mL beaker
50 mL buret
2nd utility clamp
10 mL pipet
2nd 250 mL beaker
Print a copy of the graph of pH vs. volume.

Dispose of the beaker contents as directed by your teacher. Rinse the pH Sensor and return it to the pH storage solution.

And that's it, you're done!
Start data collection.
Before you have added any drops of NaOH solution, tap Keep and enter 0 as the buret volume in mL. Select OK to store the first data pair for this experiment.
Add the next increment of NaOH titrant (enough to raise the pH about 0.15 units). When the pH stabilizes, tap Keep, enter the current buret reading (to the nearest 0.01 mL), and then select OK. You have now saved the second data pair for the experiment.
Continue adding NaOH solution in increments that raise the pH by about 0.15 units and enter the buret reading after each increment. When a pH value of approximately 3.5 is reached, change to a one-drop increment. Enter a new buret reading after each increment. Note: It is important that all increment volumes in this part of the titration be equal; that is, one-drop increments. After a pH value of approximately 10 is reached, again add larger increments that raise the pH by about 0.15 pH units, and enter the buret level after each increment. Continue adding NaOH solution until the pH value remains constant. Stop data collection.
Examine the data on the displayed graph of pH vs. volume to find the equivalence point—that is the largest increase in pH upon the addition of 1 drop of NaOH solution. To examine the data pairs on the displayed graph, tap any data point. As you tap each data point (or use the ► or ◄ keys on LabQuest), the pH and volume values are displayed. Move to the region of the graph with the largest increase in pH. Find the NaOH volume just before this jump. Record this value in the data table. Then record the NaOH volume after the drop producing the largest pH increase was added. Note: Another method for determining the equivalence-point volume is described in the Alternate Equivalence Point Method of this experiment.
Use a pipet bulb to pipet 10 mL of
the HCl solution into a 250 mL
beaker. Add 50 mL of distilled water.
Obtain a 50 mL buret and rinse the buret with a few mL of the ~0.1 M NaOH solution. Dispose of the rinse solution as directed by your teacher. Use a utility clamp to attach the buret to the ring stand. Fill the buret a little above the 0.00 mL level of the buret with ~0.1 M NaOH solution. Drain a small amount of NaOH solution so it fills the buret tip and leaves the NaOH at the 0.00 mL level of the buret. Record the precise concentration of the NaOH solution in your data table.

You are now ready to perform the titration.
Volume of buret before: 2.9 mL
Volume of buret after: 5.4mL
Total volume: 2.5mL
Molarity of NaOH: 0.1

Origonal color: clear
Ending color: dark pink
0.1(0.025) = 0.010X
0.0025 = 0.010X
X= 0.25M

The beaker at first was just clear. As we kept adding drop of NaOh the color kinda turned into a pink hue for a moment. Then all of a sudden our graph jumped and shortly after our color change to a bright florescent pink. The reason why this happens is because up until the equivalence point, there was more HCl, but the second both solution evened out, the graph jumped.
We learned that titration is how you can figure out what the concentration of a unknown solution is and how to calculate it from the information we get from the lab.

My conclusion was right because we added 2.4 mL of NaOH to HCl and we were addle to find HCl's concentration.

Sources of error included: labquest not working, not getting the measurements right, spilled sodium hydroxide, stopping the magnetic stir thing,
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