Experiment Details - Experimentium

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Experiment of Two-indicator Titration of NaHCO3 and Na2CO3 Details

VIDEO LINKS:

<h4><span style="text-decoration: underline">Consider before watching the videos:</span></h4>
How do you know that all your baking soda turned into sodium carbonate?
<h2>Lab Experiments (Write protocols and perform experiments based on these):</h2>
<ol>
 	<li><a href="https://youtu.be/c2uccfz3cUU?si=YQtgjfPOase7OdUO">Preparing the sodium bicarbonate solution</a></li>
 	<li><a href="https://youtu.be/ClG9fQtB9IE?si=0kd1G1RoWLRxZx7c">Preparing the sodium carbonate solution</a></li>
 	<li><a href="https://youtu.be/flrYfzrggzM?si=rhBhaFaA6WCytdaK">Preparing the baking soda/sodium carbonate solution (synthesized product)</a></li>
 	<li><a href="https://youtu.be/wDnLePbyVZY?si=qNPqZZaZxRo3jMCQ">Titration the baking soda solution with HCl</a></li>
 	<li><a href="https://youtu.be/nEcK1RRoSRk?si=TMP1kHcaVnZqXfPD">Titrating the sodium carbonate solution with HCl</a></li>
 	<li><a href="https://youtu.be/1V6RrE2dU94?si=ZG6DD1HYsm3brSiW">Titrating the baking soda/sodium carbonate solution with HCl</a></li>
</ol>
&nbsp;
<h2>Lab Techniques (Write protocols and perform experiments based on these):</h2>
<ol>
 	<li><a href="https://youtu.be/n6SdVEK4BpM">Preparing the Burette</a> Note: The HCl solution will be in the burette</li>
</ol>
&nbsp;
<h2>Data analysis and calculations (Use these if you need help with your data and calculations)</h2>
<ol>
 	<li><a href="https://youtu.be/cvsO_nbBOeU?si=0zp0bCWwyhb-EdmR">Titrating NaHCO<sub>3</sub> with HCl</a></li>
 	<li><a href="https://youtu.be/YDVFcgA4HKs?si=qQOs633eSN70ibYx">Titrating Na<sub>2</sub>CO<sub>3</sub> with HCl</a></li>
 	<li><a href="https://youtu.be/xH0tObKae4E?si=_NsxdxUumHbD3pTl">Titrating NaHCO<sub>3</sub>/ Na<sub>2</sub>CO<sub>3 </sub>with HCl</a></li>
</ol>
&nbsp;
<h2>The prelab is due before your lab class meets and must include Experimental Protocol, Chemical Table and Equipment Table.</h2>

Experimental Protocol

Chemical Table

<blockquote>(Representation) Prepare your chemical table including the materials you will use in the experiment.  Here is a general template that you may use.</blockquote>
<table>
<tbody>
<tr>
<td width="78">Chemical Name</td>
<td width="78">Chemical Formula</td>
<td width="68">Molar Mass (g/mol)</td>
<td width="77">Hazards</td>
<td width="314">Reference</td>
<td width="56">PPE</td>
</tr>
<tr>
<td width="78"><strong><u>Sodium Chloride</u></strong></td>
<td width="78"><strong><u>NaCl</u></strong></td>
<td width="68"><strong><u>58.5</u></strong></td>
<td width="77"><strong><u>Skin irritation</u></strong></td>
<td width="314"><a href="https://fscimage.fishersci.com/msds/21105.htm"><strong>https://fscimage.fishersci.com/msds/21105.htm</strong></a></td>
<td width="56"><strong> </strong></td>
</tr>
<tr>
<td width="78"><strong> </strong></td>
<td width="78"><strong> </strong></td>
<td width="68"><strong> </strong></td>
<td width="77"><strong> </strong></td>
<td width="314"><strong> </strong></td>
<td width="56"><strong> </strong></td>
</tr>
<tr>
<td width="78"><strong> </strong></td>
<td width="78"><strong> </strong></td>
<td width="68"><strong> </strong></td>
<td width="77"><strong> </strong></td>
<td width="314"><strong> </strong></td>
<td width="56"><strong> </strong></td>
</tr>
<tr>
<td width="78"><strong> </strong></td>
<td width="78"><strong> </strong></td>
<td width="68"><strong> </strong></td>
<td width="77"><strong> </strong></td>
<td width="314"><strong> </strong></td>
<td width="56"><strong> </strong></td>
</tr>
</tbody>
</table>

Equipment Table

Data Collection

<ol>
 	<li>(Acquiring competencies) Following your detailed protocol based on the videos, perform all the experiments. Record your observations and take pictures of your key steps in the process. Your observations and images need to be incorporated in your data section and this section should be as detailed as possible as you will use this information to complete your discussion.</li>
 	<li>(Acquiring competencies) Following your detailed protocol based on the videos, fill in the tables below:</li>
</ol>
&nbsp;

<strong>Titration of sodium bicarbonate with phenolphthalein and methyl red</strong>
<table width="732">
<tbody>
<tr>
<td width="78">Volume NaHCO<sub>3</sub>

(mL)</td>
<td width="84">Initial

volume HCl (mL)</td>
<td width="84">Drops of indicator 1 added

(drops)</td>
<td width="66">Color at start</td>
<td width="78">Color at endpoint 1</td>
<td width="90">Ending volume 1 of HCl

(mL)</td>
<td width="90">Drops of indicator 2 added</td>
<td width="78">Color at endpoint 2</td>
<td width="84">Ending volume 2 of HCl

(mL)</td>
</tr>
<tr>
<td width="78"></td>
<td width="84"></td>
<td width="84"></td>
<td width="66"></td>
<td width="78"></td>
<td width="90"></td>
<td width="90"></td>
<td width="78"></td>
<td width="84"></td>
</tr>
<tr>
<td width="78"></td>
<td width="84"></td>
<td width="84"></td>
<td width="66"></td>
<td width="78"></td>
<td width="90"></td>
<td width="90"></td>
<td width="78"></td>
<td width="84"></td>
</tr>
</tbody>
</table>
<strong> </strong>

<strong>Titration of known concentration of sodium carbonate</strong>
<table width="726">
<tbody>
<tr>
<td width="72">Volume Na<sub>2</sub>CO<sub>3</sub>

(mL)</td>
<td width="66">Initial

volume HCl (mL)</td>
<td width="102">Drops of indicator 1 added

(drops)</td>
<td width="66">Color at start</td>
<td width="78">Color at endpoint 1</td>
<td width="90">Ending volume 1 of HCl

(mL)</td>
<td width="90">Drops of indicator 2 added</td>
<td width="78">Color at endpoint 2</td>
<td width="84">Ending volume 2 of HCl

(mL)</td>
</tr>
<tr>
<td width="72"></td>
<td width="66"></td>
<td width="102"></td>
<td width="66"></td>
<td width="78"></td>
<td width="90"></td>
<td width="90"></td>
<td width="78"></td>
<td width="84"></td>
</tr>
<tr>
<td width="72"></td>
<td width="66"></td>
<td width="102"></td>
<td width="66"></td>
<td width="78"></td>
<td width="90"></td>
<td width="90"></td>
<td width="78"></td>
<td width="84"></td>
</tr>
</tbody>
</table>
&nbsp;

<strong>Titration of unknown concentration of sodium carbonate and sodium bicarbonate</strong>
<table width="732">
<tbody>
<tr>
<td width="78">Volume NaHCO<sub>3</sub>/Na<sub>2</sub>CO<sub>3</sub>

(mL)</td>
<td width="66">Initial

volume HCl (mL)</td>
<td width="102">Drops of indicator 1 added

(drops)</td>
<td width="66">Color at start</td>
<td width="78">Color at endpoint 1</td>
<td width="90">Ending volume 1 of HCl

(mL)</td>
<td width="90">Drops of indicator 2 added</td>
<td width="78">Color at endpoint 2</td>
<td width="84">Ending volume 2 of HCl

(mL)</td>
</tr>
<tr>
<td width="78"></td>
<td width="66"></td>
<td width="102"></td>
<td width="66"></td>
<td width="78"></td>
<td width="90"></td>
<td width="90"></td>
<td width="78"></td>
<td width="84"></td>
</tr>
<tr>
<td width="78"></td>
<td width="66"></td>
<td width="102"></td>
<td width="66"></td>
<td width="78"></td>
<td width="90"></td>
<td width="90"></td>
<td width="78"></td>
<td width="84"></td>
</tr>
</tbody>
</table>

Data Processing

<ol>
 	<li>(Representation) Write the balanced molecular equation for the reaction of sodium bicarbonate with HCl.</li>
 	<li>(Representation) Write the complete ionic equation for the reaction of sodium bicarbonate with HCl.</li>
 	<li>(Representation) Write the net ionic equation for the reaction of sodium bicarbonate with HCl.</li>
 	<li>(Analysis) Classify the reaction.</li>
 	<li>(Manipulation) Calculate the moles of sodium bicarbonate you used to make your solution.</li>
 	<li>(Manipulation) Calculate the number of liters of the sodium bicarbonate solution you prepared.</li>
 	<li>(Manipulation) Calculate the theoretical concentration (molarity) of the known solution of sodium bicarbonate.</li>
 	<li>(Manipulation) In your titration of sodium bicarbonate with HCl, calculate the volume of HCl used in liters.</li>
 	<li>(Manipulation) Based on the concentration of the HCl and the volume used, determine the number of moles of HCl neutralized in the titration.</li>
 	<li>(Analysis) Identify the number of moles of sodium bicarbonate consumed in this titration.</li>
 	<li>(Manipulation) Calculate the experimental concentration of your sodium bicarbonate solution from your titration using the volume of the sodium bicarbonate solution in liters, and the moles of sodium bicarbonate calculated from the titration.</li>
 	<li>(Representation) Fill out the following table with your data from the titration of NaHCO<sub>3 </sub>with 0.1M HCl with methyl red.</li>
</ol>
<u> </u>
<table width="708">
<tbody>
<tr>
<td width="78">Volume NaHCO<sub>3</sub>

Solution

(mL)</td>
<td width="78">Volume NaHCO<sub>3</sub>

Solution

(L)</td>
<td width="72">Initial volume HCl (mL)</td>
<td width="66">Ending volume 1 of HCl

(mL)</td>
<td width="90">Volume HCl added part 1

(mL)</td>
<td width="72">Volume HCl added (L)</td>
<td width="66">Moles HCl</td>
<td width="78">Moles

NaHCO<sub>3</sub></td>
<td width="108">Experimental Molarity of

NaHCO<sub>3</sub>

(M)</td>
</tr>
<tr>
<td width="78"></td>
<td width="78"></td>
<td width="72"></td>
<td width="66"></td>
<td width="90"></td>
<td width="72"></td>
<td width="66"></td>
<td width="78"></td>
<td width="108"></td>
</tr>
<tr>
<td width="78"></td>
<td width="78"></td>
<td width="72"></td>
<td width="66"></td>
<td width="90"></td>
<td width="72"></td>
<td width="66"></td>
<td width="78"></td>
<td width="108"></td>
</tr>
</tbody>
</table>
&nbsp;
<ol start="13">
 	<li>(Analysis) Compare the concentrations of the sodium bicarbonate solution determined by two different methods and use your data to support your conclusions.</li>
 	<li>Representation) Write the balanced molecular equation for the reaction of sodium carbonate with HCl.</li>
 	<li>(Representation) Write the complete ionic equation for the reaction of sodium carbonate with HCl.</li>
 	<li>(Representation) Write the net ionic equation for the reaction of sodium carbonate with HCl.</li>
 	<li>(Analysis) Classify the reaction.</li>
 	<li>(Manipulation) Calculate the moles of sodium carbonate based on the grams used to prepare your solution.</li>
 	<li>(Manipulation) Calculate the number of liters in the sodium carbonate solution you prepared.</li>
 	<li>(Manipulation) Calculate the concentration (molarity) of the sodium carbonate solution you prepared.</li>
 	<li>(Manipulation) Calculate the volume of HCl (in liters) required to reach the endpoint in the titration of sodium carbonate with phenolphthalein.</li>
 	<li>(Manipulation) Based on the concentration of the HCl and the volume used (Initial volume – ending HCl volume for phenolphthalein part of the titration), calculate the number of moles of HCl neutralized in this part of the titration.</li>
 	<li>(Analysis) Identify the number of moles of sodium carbonate consumed in this part of the titration.</li>
 	<li>(Analysis) Identify the species in solution at endpoint of the phenolphthalein titration.</li>
 	<li>(Manipulation) Based on the moles consumed and the volume of sodium carbonate you started with, determine the experimental concentration of your sodium carbonate solution.</li>
 	<li>(Manipulation) Using the initial volume as the volume at the end of the phenolphthalein titration, and the final volume as the color change for methyl red indicator, calculate the volume of HCl consumed in the titration with methyl red.</li>
 	<li>(Manipulation) Based on the concentration of the HCl solution and the volume used in the methyl red portion of the titration, calculate the moles of HCl consumed.</li>
 	<li>(Manipulation) Calculate the number of moles of sodium bicarbonate consumed.</li>
 	<li>(Representation) Fill out the following table with your data from the titration of known Na<sub>2</sub>CO<sub>3 </sub>with 0.1M HCl with phenolphthalein and methyl red.</li>
</ol>
Part 1: Titration with phenolphthalein
<table width="714">
<tbody>
<tr>
<td width="78">Volume Na<sub>2</sub>CO<sub>3</sub>

solution

(mL)</td>
<td width="78">Volume Na<sub>2</sub>CO<sub>3</sub>

solution

(L)</td>
<td width="72">Initial volume HCl (mL)</td>
<td width="72">Ending volume 1 of HCl

(mL)</td>
<td width="72">Volume HCl added part 1

(mL)</td>
<td width="72">Volume HCl added (L)</td>
<td width="60">Moles HCl</td>
<td width="90">Moles

Na<sub>2</sub>CO<sub>3</sub>

consumed</td>
<td width="120">Concentration

Na<sub>2</sub>CO<sub>3</sub>

&nbsp;

(moles/L)</td>
</tr>
<tr>
<td width="78"></td>
<td width="78"></td>
<td width="72"></td>
<td width="72"></td>
<td width="72"></td>
<td width="72"></td>
<td width="60"></td>
<td width="90"></td>
<td width="120"></td>
</tr>
</tbody>
</table>
&nbsp;

Part 2: Titration with methyl red
<table width="552">
<tbody>
<tr>
<td width="84">Ending volume 1 of HCl

(mL)</td>
<td width="96">Ending Volume 2 of HCl

(mL)</td>
<td width="96">Volume HCl added part 2

(L)</td>
<td width="78">Moles HCl</td>
<td width="102">Moles of NaHCO<sub>3 </sub>consumed part 2

(mL)</td>
<td width="78">Volume mixture solution

(L)</td>
<td width="72">Initial volume HCl (mL)</td>
<td width="72">Ending volume 1 of HCl

(mL)</td>
<td width="72">Volume HCl added part 1

(mL)</td>
<td width="78">Volume HCl added (L)</td>
<td width="60">Moles HCl</td>
<td width="90">Moles

Na<sub>2</sub>CO<sub>3</sub>

consumed</td>
<td width="120">Concentration

Na<sub>2</sub>CO<sub>3</sub>

(mole/L)</td>
</tr>
<tr>
<td width="78"></td>
<td width="78"></td>
<td width="72"></td>
<td width="72"></td>
<td width="72"></td>
<td width="78"></td>
<td width="60"></td>
<td width="90"></td>
<td width="120"></td>
</tr>
</tbody>
</table>
&nbsp;

Part 2: Titration with methyl red
<table width="552">
<tbody>
<tr>
<td width="84">Ending volume 1 of HCl

(mL)</td>
<td width="96">Ending Volume 2 of HCl

(mL)</td>
<td width="96">Volume HCl added part 2

(L)</td>
<td width="78">Moles HCl</td>
<td width="102">Moles of NaHCO<sub>3 </sub>consumed part 2

&nbsp;</td>
</tr>
<tr>
<td width="84"></td>
<td width="96"></td>
<td width="96"></td>
<td width="96"></td>
<td width="78"></td>
<td width="102"></td>
</tr>
</tbody>
</table>
&nbsp;
<ol start="32">
 	<li>(Manipulation) Calculate the difference in moles between Part 1 and Part 2 of the moles of sodium carbonate and sodium bicarbonate, then comment of the success of your decomposition of the sodium bicarbonate.to sodium carbonate reaction.</li>
 	<li>(Analysis) Comment on the need for 2 indicators for this titration.</li>
 	<li>(Analysis) Comment on how the experiment would be different if only phenolphthalein was used.</li>
 	<li>(Analysis) Comment on how the experiment would be different if only methyl red was used.</li>
 	<li>(Analysis) Identify at least one of the 12 principles of green chemistry applied in this experiment. Justify your selection. <a href="https://www.acs.org/green-chemistry-sustainability/principles/12-principles-of-green-chemistry.html">12 Principles of Green Chemistry</a></li>
 	<li>(Assumptions) Fill in the following table using the observations and data from your experiments</li>
</ol>
<table>
<tbody>
<tr>
<td width="212">Assumptions made</td>
<td width="192">Testing the assumption</td>
<td width="219">If assumptions are wrong ...</td>
</tr>
<tr>
<td width="212">Sodium carbonate is not a stable solid.</td>
<td width="192">Leave uncovered for an hour and check.</td>
<td width="219">Weigh it before and after.</td>
</tr>
<tr>
<td width="212"></td>
<td width="192"></td>
<td width="219"></td>
</tr>
</tbody>
</table>
&nbsp;
<h1>Summary</h1>
The summary has two parts: an abstract and an experimental protocol reflecting the experiment that you actually performed. The abstract and experimental protocol should both be between 100-250 words, size 12 Arial font each. There may be multiple experimental protocols for one experiment.
<h2>Part 1.</h2>
<strong>Title of Experiment:</strong> Performed tasks and applied techniques to accomplish the goal of the experiment and a description of the system under study (the title you are given for the lab is insufficient).

Ex. Calibration of burette techniques to determine endpoints in an acid – base neutralization reaction using phenolphthalein, sodium hydroxide and hydrochloric acid.

Discussion

Abstract

(This is a highlight of what you learned from performing the experiment and processing your collected data. Below is a template and an example of what you are expected to write.)

In this lab experiment we investigated [purpose of your experiment] using [list the materials you worked with] and we found that [present the highlights of your results (include numbers)]. The results [present significant results]. The collected data compares to [draw conclusion about your results compared to other sources (this could be another group or the literature value)]. The [add type of measurement individually] measurement was collected using [describe instrument by sensitivity].

&nbsp;

Think through this before writing:
<ol>
 	<li>Purpose: What were you trying to do?</li>
 	<li>Materials used: What chemicals and materials did you work with?</li>
 	<li>Method: What instruments were used to collect measurements and how were the measurements collected?</li>
 	<li>Results: What did you find out about the objects under study?</li>
 	<li>Significance: What did you learn about the precision and accuracy of your techniques? How do your determined values compare to reported values?</li>
</ol>
&nbsp;

&nbsp;
<h2>Part 2.</h2>
<strong>Title of Protocol </strong>(Brief description of the experiment in bold)

Ex. Making baking soda solution

Ex. Making sodium carbonate solution

Ex. Making solution of decomposition product

Ex. Titrating NaHCO<sub>3 </sub>with HCl using methyl red indicator

Ex. Titrating Na<sub>2</sub>CO<sub>3 </sub>with HCl using methyl red indicator and phenolphthalein

Ex. Titrating NaHCO<sub>3</sub>/ Na<sub>2</sub>CO<sub>3 </sub>with HCl using methyl red indicator and phenolphthalein

<strong>Experimental Protocol</strong>

(This is a condensed and organized description of the protocol you actually completed during class. Use the exact amounts of materials and list the exact equipment that you used in performing the experiment. The length of this section depends on the complexity of your experiment, usually 3-4 sentences maximum in one paragraph.)

&nbsp;

(For each material and procedure)