11. Mass % HCl in sample * See Example 2 for calculations for lines 4-9 Show your setup for the calculation of the molarity of the HCl for Trial 1 here. Refer to Example 2. Show your setup for the calculation of the percent HCl in the solution here. Refer to Example 3. Use your average molarity.
11. Mass % HCl in sample * See Example 2 for calculations for lines 4-9 Show your setup for the calculation of the molarity of the HCl for Trial 1 here. Refer to Example 2. Show your setup for the calculation of the percent HCl in the solution here. Refer to Example 3. Use your average molarity.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Answer question 11, Mass % HCI in sample. Then, show your setup for the calculation of the molarity of the HCI for Trial. For the last section, show your setup for the calculation of the percent HCI in the solution. (Use the chart for reference)
Transcribed Image Text:II. Titration of an Acidic Solution
0.289 M NaOH
Molarity of standard NaOH solution
Trial 1
Trial 2
Trial 3
1.7
9.8
11.5
1. Initial buret reading, mL
20.9
29.1
31.0
2. Final buret reading, mL
19.2
19.3
19.5
3. Volume of NaOH, mL
(see Example 1)
0.0192
0.0193
0.0195
*4. Volume of NaOH, L
0.0055488
0.0055777
0.0056355
5. Moles of NAOH, mol
0.0055488
0.0055777
0.0056355
6. Moles of HCI, mol
2.00
2.00
2.00
7. Volume of HCI (The Works), mL
(from pipet)
0.002
0.002
0.002
8. Volume of HCI, L
2.77
2.79
2.82
9. Molarity of HCI, mol/L
2.79 mol/L
10. Average molarity HCI
11. Mass % HCI in sample
Transcribed Image Text:11. Mass % HCl in sample
* See Example 2 for calculations for lines 4-9
Show your setup for the calculation of the molarity of the HCl for Trial 1 here. Refer to Example 2.
Show your setup for the calculation of the percent HCl in the solution here. Refer to Example 3. Use
your average molarity.
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