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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.)

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.)

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3. de33520 m Experiment 12 | Titration 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? Name: a 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.
Transcribed Image Text:3. de33520 m Experiment 12 | Titration 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? Name: a 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.
0.00/254 0.0100L 12.54x0 10omanson TMOTHCL OOL HAI 7 Name: Macy hufford Data Table and Results Nao C₂30₂ H₂O+NaC₂H₂O₂ Molarity of NaOH:.3455 M 0.25% F Par olaccuc acid 0.01000L Volume of acid added to flask Initial buret reading Final buret reading Volume of base titrated into flask* Trial 1 Experiment 12 | Titration 10.00ML AV=VP-Vi Trial 2 10.0m 10.0m 10.0 Calculated molarity of acetic acid in your unknown *Final buret reading - Initial buret reading. Unknown #: True molarity: Trial 3 0.01 21:19426.09 21.07m 42.38m4 47.18ml 21.01mL 21.19mL 21.09 Trial 4 (if needed) Trial 5 (if needed) 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.) trial 1: Choose the three trials that have molarities that agree within 1% of one another and use these three molarities to calculate your average molarity. 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.
Transcribed Image Text:0.00/254 0.0100L 12.54x0 10omanson TMOTHCL OOL HAI 7 Name: Macy hufford Data Table and Results Nao C₂30₂ H₂O+NaC₂H₂O₂ Molarity of NaOH:.3455 M 0.25% F Par olaccuc acid 0.01000L Volume of acid added to flask Initial buret reading Final buret reading Volume of base titrated into flask* Trial 1 Experiment 12 | Titration 10.00ML AV=VP-Vi Trial 2 10.0m 10.0m 10.0 Calculated molarity of acetic acid in your unknown *Final buret reading - Initial buret reading. Unknown #: True molarity: Trial 3 0.01 21:19426.09 21.07m 42.38m4 47.18ml 21.01mL 21.19mL 21.09 Trial 4 (if needed) Trial 5 (if needed) 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.) trial 1: Choose the three trials that have molarities that agree within 1% of one another and use these three molarities to calculate your average molarity. 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.
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