rial NumberTotal Volume ofTitrant Added(mL)Post Lab Questions34.7b)34.7Burette contains 0.70M of KOH and 100mL of Mystery CH3COOH34.7All part of same question.1. Using data collected from the titration, determine the concentration of the assigned unknown solution.a) Using your answer from question 1, determine the pH of the unknown acetic acid solution BEFORE thetitration began (i.e., when no base has been added) if Ka of acetic acid is 1.8x10-5.Determine the pH of the solution AT EQUIVALENCE POINT of the titration.

Concentration of KOH solution=0.70MVolume of KOH solution is used =34.7mL Volume of unknown CH3COOH…

Trial Number Total Volume of Titrant Added (mL) Post - Lab Questions 34.7 b) 34.7 Burette contains 0.70M of KOH and 100mL of Mystery CH3COOH *All part of same question. 1. Using data collected from the titration, determine the concentration of the assigned unknown solution. 34.7 a) Using your answer from question 1, determine the pH of the unknown acetic acid solution BEFORE the titration began (i.e., when no base has been added) if Ka of acetic acid is 1.8x10-5. Determine the pH of the solution AT EQUIVALENCE POINT of the titration.

Trial Number Total Volume of Titrant Added (mL) Post - Lab Questions 34.7 b) 34.7 Burette contains 0.70M of KOH and 100mL of Mystery CH3COOH *All part of same question. 1. Using data collected from the titration, determine the concentration of the assigned unknown solution. 34.7 a) Using your answer from question 1, determine the pH of the unknown acetic acid solution BEFORE the titration began (i.e., when no base has been added) if Ka of acetic acid is 1.8x10-5. Determine the pH of the solution AT EQUIVALENCE POINT of the titration.

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...

See similar textbooks

Similar questions

Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________
y/ h VG y² ki tions/Interface/acellus_engine.html?ClassID=329083093# News Share files over Blu... FL-CA - Student Inf... Aar $ All Copyright © 2003-2022 International Academy of Science. All Rights Reserved. % 8 15.0 mL of 4.0 M HCI is added to 85.0 mL of water. What is the final concentration of the acid? A .706 F6 * & F7 [?] mol HCI 8 3) Thomas Jefferso... F8 MHCI DELL prt sc apush chapter 7 ma... F10 Enter home F11 end F12 Just Short Answer q... insert y g 4 delete
Solve question 1 please
(4. What effect would the following errors have on the final value of Ka determined from this experiment? a. The pH meter was calibrated incorrectly and the actual pH was 6.4 when the meter read 7.0. The student recorded and used the meter readings. b. After measuring the 10.00 mL of acid, the student added 80 mL of distilled water instead of 75 mL.
EXPERIMENT 10 PRE-LABORATORY QUESTIONS STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0.50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155
Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…
Q4. In this experiment, we add hydrochloric acid to our unknown sodium hydroxide solution during the titration. Sketch a sample pH curve showing how the pH of the titrated solution changes as we add more titrant. Be sure to label both axes of your graph and indicate the position of the equivalence point. C10 p Con Q5 You initially begin with a 0.1593 M hydrochloric acid solution. If you had a 125.0 mL sample of this hydrochloric acid solution, how many grams of HCl would be present in the sample? Show all work. Yourde tobl Q6 Write out a stepwise procedure (list of numbered steps) that you plan to execute when you come to lab to do the titration. (You instructor will review and offer feedback in person; you must have a written procedure before you can start the in-person portion of the final). You can assume you have access to the following equipment: buret/ring stand and buret clamp 25 mL graduated cylinder pipet pump 150 mL beaker (for waste) distilled water 50 mL buret 125 mL…
6. Open the bags and add 3 drops of bromothymol blue to each bottle. The indicator turns yellow if vinegar is still present and is blue-green when vinegar is not present. Record the color of each solution in the table provided. Data Table 1: Reaction Data Sample 7. Add a 4 teaspoon of baking soda to each bag. Effervescence of CO₂ occurs if excess vinegar is present. Record your observations in the table provided. Moles of vinegar (mol) Moles of baking soda (mol) mistry Relative size of bag Was excess vinegar present? Color with indicator? Reacts with additional baking soda? Moles of gas produced (mol) Watch the limiting reagent! #1 0.042 0.014 чем yes yellow #2 0.042 0.028 #3 yes yellow 0.042 0.042 Experiment 11 yes yellow #4 Stoichiometry 0.042 0.88 more small big bigger bigger No 0.071 #5 NO Geen 0.042 Blue Calculations 1. Use Table 1 to determine which reactant was limiting in each trial. Use the amount of limiting reactant to calculate the moles of carbon dioxide gas that were…
Name: Postlab Questions: 1. A student was performing the test for chloride in his unknown. When he added the five drops of HNO3, he observed bubbles forming (effervescence) in his unknown. Was chloride present in his unknown? How do you know? 2. A student added barium chloride to her unknown and immediately witnessed the formation of a precipitate. She concluded that this white precipitate indicated the presence of chloride ion in her unknown. Is she correct? How do you know? 3. A student has two unlabeled bottles of solution. One contains PO4³¯ and the other SO,?". How can this student identify which is which? Page 6 of 6
DATA AND CALCULATIONS Show all calculations neatly on an attached sheet. Trial 1 Trial 2 Trial 3 70.6849. 68.0749 2.61g 23.25ML O.65ML 22.6mL Mass of flask + vinegar Mass of empty flask Mass of vinegar used Final buret reading Initial buret reading Volume of NaOH used Moles of NaOH used 0.00226 mol Moles of açetic acid titrated Mass of acetic acid titrated Mass % acetic acid in vinegar 5.0%
The KI used in this lab has a concentration of 0.500M. In trials 1-4, 1.0 ml of this solution is combined with 4.0 ml of the H2O2. What is the concentration of the KI in this solution after mixing but before the reaction occurs. ( Enter the result in table 1 on the report sheet) (2 sig figs)
Thank you! Data included in pictures! No hand drawn graphs!! Determine the equivalence point and the endpoint of the sudsy ammonia/citric acid reaction by graphing the titration data (pH vs volume citric acid) from Table 3: Titration of Sudsy Ammonia with 0.25 M Citric Acid Data with the Chosen Indicator. Draw a green arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your equivalence point. Draw a blue arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your endpoint. Use a graphing software to create the x-y scatter plot showing the pH of the experimental solution as a function of the volume of citric acid (the titrant) added for the titration data in Question 9. On your graph, the x-axis should be the volume of citric acid added (mL), and the y-axis should be the pH of the experimental…