Examine the following information below for a electolytic cell and answer the following questions: Procedure: Procedure: Constructing an Electrolytic Cell (convert energy to ions) 1. Obtain a 6-volt battery, electrodes, and plastic sample cup necessary to build an electrolytic cell like that shown in figure 2 below. Obtain a pH meter and set it to begin collecting data. 2. Weigh 2.0 g of solid KI. Record the mass. Transfer the solid to an Erlenmeyer flask. 3. Add 100 mL of deionized water (measure using a graduated cylinder) to the flask and swirl it until a homogeneous solution is formed. Measure and record the initial pH of this solution. 4. Transfer the 100 mL of KI solution from the Erlenmeyer flask to the plastic sample cup. Place the lid containing the electrodes on top of the sample cup. Attach wires from the batter to the electrodes. Note and record your start time. 5. Observe the electrolysis for several minutes. Record your observations at several time intervals. 6. Let the electrolysis run for at least 15 minutes. After this time period, disconnect the wires. Note and record the time to the nearest minute. 7. Remove and examine the electrodes. Record your observations and the probable identity of any substance that may be present. 8. Stir the solution thoroughly. Measure and record the final pH. 9. Calculate the number of moles of OH- produced. Data recorded: Electrolytic Cell Mass of KI, g 2.006 g Initial pH 5.25 Electrolysis start time 10:06 am Electrolysis finish time 10:22 am Total time of electrolysis 16 minutes Final pH 10.9 A. what is the moles of KI used? B. what is the inital OH- concentration, mol/L? C. what is the inital moles of OH-? D. what is the final OH- concentration, mol/L? E. What is the final moles of OH-? F. Moles of OH- produced? (Hint: d-b)
Examine the following information below for a electolytic cell and answer the following questions:
Procedure:
|
Procedure: Constructing an Electrolytic Cell (convert energy to ions) |
|
|
1. |
Obtain a 6-volt battery, electrodes, and plastic sample cup necessary to build an electrolytic cell like that shown in figure 2 below. Obtain a pH meter and set it to begin collecting data. |
|
2. |
Weigh 2.0 g of solid KI. Record the mass. Transfer the solid to an Erlenmeyer flask. |
|
3. |
Add 100 mL of deionized water (measure using a graduated cylinder) to the flask and swirl it until a homogeneous solution is formed. Measure and record the initial pH of this solution. |
|
4. |
Transfer the 100 mL of KI solution from the Erlenmeyer flask to the plastic sample cup. Place the lid containing the electrodes on top of the sample cup. Attach wires from the batter to the electrodes. Note and record your start time. |
|
5. |
Observe the |
|
6. |
Let the electrolysis run for at least 15 minutes. After this time period, disconnect the wires. Note and record the time to the nearest minute. |
|
7. |
Remove and examine the electrodes. Record your observations and the probable identity of any substance that may be present. |
|
8. |
Stir the solution thoroughly. Measure and record the final pH. |
|
9. |
Calculate the number of moles of OH- produced. |
Data recorded:
|
Electrolytic Cell |
|
|
Mass of KI, g |
2.006 g |
|
Initial pH |
5.25 |
|
Electrolysis start time |
10:06 am |
|
Electrolysis finish time |
10:22 am |
|
Total time of electrolysis |
16 minutes |
|
Final pH |
10.9 |
A. what is the moles of KI used?
B. what is the inital OH- concentration, mol/L?
C. what is the inital moles of OH-?
D. what is the final OH- concentration, mol/L?
E. What is the final moles of OH-?
F. Moles of OH- produced? (Hint: d-b)
Trending now
This is a popular solution!
Step by step
Solved in 9 steps with 11 images
