Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Concept explainers
Question
thumb_up100%
How do I find the moles excess HCl titrated and Moles HCl absorbed by Tablet
Transcribed Image Text:Part IV. Determine the percentage of CaCO3 in an antacid tablet.
HCl (aq) + NaOH (aq) → NaCl (aq) + H₂0 (1)
Molarity
D
Mass of Antacid Tablet
Volume 3.00M HCl Used
Total moles HCl added to flask
Final burette reading
Initial burette reading
Volume of NaOH used
Molarity of NaOH (from Part II)
Moles NaOH used
Moles excess HCl titrated
Moles HCl absorbed by Tablet
(Hint: It is NOT moles titrated.)
Moles CaCO3 in Tablet
Mass CaCO3 in Tablet
Malys
- of saute
IL of CaCO3 in Tablet
Average % CaCO3 in Tablet
1000m2
= 0.0100 5 C
4.6293 *10*²=
mol of
Solute
0.01405
0.001352917
Trial 1
1.4604 12341s
5.00m
5,00
41,05m
41,05m
9.6293 x 10
1.353x10-3
>
Trial 2
L
41.05m
Show your calculations for "Mass % CaCO3 in Tablet" for at least 1 trail below.
105m41108
ML
55.35
0.01
55.34
9.629 31 10
5.329x10-³
Tria! 3
Z
1.234/
48.01
38.4mc
१.८ ।
45.75
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 3 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Calculate the mass of KBr required to be dissolved in 1.25 L solution that has 3.21 M concentration.arrow_forwardPart C – Acid–base and solubility equilibria 1. Rinse 4 regular size test tubes and a 10 mL measuring cylinder thoroughly with water. Number the test-tubes from 1 to 4 in a test tube rack. 2. Into each of test tubes 1 – 3 put a small amount of solid benzoic acid (put the same amount – about the size of a pea – in each test tube). 3. Add 2 mL (use the measuring cylinder) of water to tube 1 and shake to mix the contents. 4. Add 2 mL (measuring cylinder) of 2 M HNO3 to tube 2 and shake to mix the contents. 5. Rinse the measuring cylinder with water, then use it to add 2 mL of 2 M NaOH to tube 3 and shake for about 10 seconds to mix the contents. Rinse the measuring cylinder. 6. Pour about half of the solution from tube 3 into tube 4, than add 2 mL of 2 M HNO3 to tube 4. 7. Allow the test tubes to stand for 2 or 3 minutes then record the appearance of the mixtures in each test tube. 8. Answer the questions on the results page relating to this equilibrium system.arrow_forwardCalculate the molarity of the HCl using 25.00 mL of HCl solution and the volume of the 0.3000 M NaOH also 25mlarrow_forward
- QUESTION 4 Standardizing a solution of sodium hydroxide for our acid-base titration experiment means O a. to prepare a series of standard solutions and determine the average concentration. O b.to prepare the standard solution directly from a solid and not from a solution. O c. to compare the results of your titration with those of other laboratories, or other groups performing the same titration. O d. to determine, by titration , the concentration of the basic solution using a known quantity of a primary standard acid. Click Save and Submit to save and submit. Click Save All Answers to save all answers. F7 F8 F9 F10 F11 F12 Insearrow_forwardA 0.658 g sample of a diprotic acid is dissolved in water and titrated with 0.130 M NAOH. What is the molar mass of the acid if 38.4 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. 10 11 12 13 molar mass: g/mol 18 19 20 21 22 23 24arrow_forwardCalculate the number of moles of NaOH used when 15.45 mL of the 0.0985 M solution was delivered to reach the endpoint of the titration. Remember to report the answer with the correct number of significant fıgures and accepted abbreviated units. Keep in mind the example format below: 0.1025 mLarrow_forward
- The titration of a 5.00 mL sample of an HCl solution of unknown concentration requires 4.90 mL of a 0.1000 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution in M?arrow_forwardWhat are the ingredients in carbonated soda responsible for the color change in litmus paper?arrow_forwardthe percentage of KHP in an unknown sample was determined. Which of the following is NOT true. Aqueous NaOH should be standardized so concentration is accurately known. The moles of KHP can be determined at the endpoint, which is close to the equivalence point. Percentage of KHP, is equal to the mass of KHP found, divided by the mass of the unknown, multiplied by 100.arrow_forward
- You are given an unknown diprotic acid to make an identification. You dissolved 2.0 g of the acid into 100 mL of water and titrated it with 0.2 M NAOH solution. The equiva- lence point was found after titrating 222.00 mL NAOH solution. What is this unknown acid?arrow_forwardWhen a 15.4 mL sample of a 0.327 M aqueous hypochlorous acid solution is titrated with a 0.369 M aqueous sodium hydroxide solution, what is the pH at the midpoint in the titration? pH Use the References to access important values if needed for this question. =arrow_forwardWhat volume of 0.432 M NaOH is needed to titrate 50.0mL of 0.254 M HCl?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY