3. If 20.05 mL of 0.105 M HCI are titrated with 17.35 mL of an NaOH solution. a. Write the balanced chemical equation. Show all physical states. b. Using solution stoichiometry, what is the molarity of the NaOH solution? 4. If there is on average 1.000g of CaCO3 in a tablet of Extra Strength TumsTM, how many moles of CaCO3 is this?
3. If 20.05 mL of 0.105 M HCI are titrated with 17.35 mL of an NaOH solution. a. Write the balanced chemical equation. Show all physical states. b. Using solution stoichiometry, what is the molarity of the NaOH solution? 4. If there is on average 1.000g of CaCO3 in a tablet of Extra Strength TumsTM, how many moles of CaCO3 is this?
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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Please help with questions 3 & 4
Transcribed Image Text:Erlenmeyer Flask
Balance
Weigh Boat
Balance
At Home Buret
Graduated Cylinder(s)
Antacid Tablets
Prelab:
1. What is the pH of a 4.8 x 10-5 M HCI solution?
Plastic bag
5% Distilled White Vinegar (0.833M)
2. What is the pH of a 9.8 x 10-6 M NaOH solution?
3. If 20.05 mL of 0.105 M HCl are titrated with 17.35 mL of an NaOH solution.
a. Write the balanced chemical equation. Show all physical states.
b. Using solution stoichiometry, what is the molarity of the NaOH solution?
4.
If there is on average 1.000g of CaCO3 in a tablet of Extra Strength TumsTM, how many moles of
CaCO3 is this?
5. Using chemical equation (3) at the beginning of this lab, determine the moles of CaCO3 and
then the corresponding moles of acetic acid this is equivalent to.
6. Given the moles of acetic acid you calculated in #5, and the accepted value of 0.833M as the
concentration of household vinegar (Acetic Acid) determine the approximate volume each trial
should use. (Please keep this volume in mind as rough estimates on when to slow the titration
down)
7. How will you know that your chemical reaction is complete in this lab?
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