12.0 1 10.0 pH of solution in flask 8.0 Equivalence Point 6.0 4.0 2.0 5 10 15 20 25 30 35 40 45 mL of 0.115 M NAOH added to flask A 50.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. a). What would be the molar mass of the unknown acid if the density of the solution is 1.00g/mL and mass concentration of the acid is 3.00 g/L. Molar Mass = g/mole Please use 3 sig figs for the ans, just provide the value no need for units). (Note: use the plot to estimate the volume needed to reach the equivalence point) ɔ). What would be the pKa of the unknown acid? pka = (please use two sig igs for the ans) (use the plot above to estimate) c). What would be the concentration of the HA and conjugate A- when 9.00 mL of 0.115 M NaOH is used for the titration. (please use 3 sig figs for the ans and just imput the units) (Hint: use the mmoles of HA estimated from part a) O OO O

12.0 1 10.0 pH of solution in flask 8.0 Equivalence Point 6.0 4.0 2.0 5 10 15 20 25 30 35 40 45 mL of 0.115 M NAOH added to flask A 50.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. a). What would be the molar mass of the unknown acid if the density of the solution is 1.00g/mL and mass concentration of the acid is 3.00 g/L. Molar Mass = g/mole Please use 3 sig figs for the ans, just provide the value no need for units). (Note: use the plot to estimate the volume needed to reach the equivalence point) ɔ). What would be the pKa of the unknown acid? pka = (please use two sig igs for the ans) (use the plot above to estimate) c). What would be the concentration of the HA and conjugate A- when 9.00 mL of 0.115 M NaOH is used for the titration. (please use 3 sig figs for the ans and just imput the units) (Hint: use the mmoles of HA estimated from part a) O OO O

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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Question Completion Status: For Solution A, approximately how many mL of HCI were needed to exceed the buffering capacity of this solution? Enter the number only. Don't enter units as part of your answer and don't use commas or scientific notation. Titration curve of Solution A 14 13 12 11- 10 9 8 pH 7 6 5 4 3 2 1 5 4 3 2 1 HCI added (mL) 0 1 2 3 4 5 NaOH added (mL) 14 13 12- 11 10 9 8 pH 7 6.8 2 65 4 3 2 1 Titration curve of Solution B Click Save and Submit to save and submit. Click Save All Answers to save all answers. 54 32 1 HCI added (mL) 0123 NaOH added (mL)
The titration curve attached was obtained from the titration of a 0.225 g sample of a solid acid with 0.100 M KOH. How many moles of acid are present? 14 12 10 8 6. 4. 2 10 15 20 25 30 Volume of KOH added (mL) A. 0.000800 moles Acid B. 0,00160 moles Acid O C. 0,00110 moles Acid D. 0.00255 moles Acid
Please type this, do not write it on a paper.
1. Label your graph "Strong Acid-Strong Base Titration." Create a line graph using the data below, which shows titration of 40.00 mL of 0.100M HCl with 0.100M NaOH. Once you have created the graph and connected the points with a smooth curve, use a colored pencil to label the equivalence point on your graph. Volume NaOH added (mL) 0.00 10.00 20.00 30.00 35.00 39.50 39.99 40.00 40.01 40.25 41.00 45.00 50.00 60.00 70,00 80.00 PH 1 1.22 1.48 1.85 1.85 3.20 4.90 7.00 9.40 10.50 11.09 11.76 12.05 12.30 12.43 12.52
In an acid-base titration experiment, the equivalence point on the titration curve was at a pH of 6.0. Based on this information, which of the following is represents the titration experiment that was conducted? It was a titration conducted between a strong base and strong acid It was a titration conducted between a weak acid and a strong base. It was a titration conducted between a strong acid and a weak base
Match each term with its definition or description. 0000000 The point in a titration when the added amount of standard reagent is equal to the amount of analyte being titrated. A volumetric analysis technique used to determine the unknown concentration of a solution by using the known concentration of another. A solution of unknown concentration. The standard reagent of known concentration that is added from a buret to the analyte solution. A common concentration unit - moles per liter. The point in a titration when a change in the analyte solution is observed, indicating equivalency. It is added to the analyte solution and aids in the observation of the completion of the reaction. molarity equivalence point Answer Bank end point titration titrant analyte indicator
1
A 50.0-ml sample of 0.20 M hydrochloric acid (HCI) is titrated with 0.5 M LIOH. Determine the pH of the solution after the following volumes of LIOH titrant are added. Express your answers to two decimal places. a) pH after 10 mL of LIOH added: b) pH after 20 mL of LIOH added: c) pH after 30 mL of LIOH added: Check
1.A 25.8 mL aliquot of 0.03 M aqueous hydrochloric acid is titrated with 0.02 M NaOH (ac). What volume (mL) of the base is used when the equivalence point is reached? Place the procedure.
When pH titrations occur, more data points become necessary at the vertical deflection near the equivalence point which is accomplished by adding smaller volumes of base from the pipers before taking the pH of the solution. Why are more points needed at this point in the titration curve? Why can larger volumes be used in the area outside of this region?
The pOH is of 0.1 M acetic acid by titration of adding 150 ml of 0.1 M sodium hydroxide to 100 ml ---- O 1.7 8.7 O 12.3
Phosphoric Acid is considered polyprotic. What does this mean? What does this imply about a titration of this molecule? If there is still enough time, draw a titration curve for formic acid. Use a separate sheet of paper If there is still enough time, draw a titration curve for phosphoric acid. Use a separate sheet of paper Compare and contrast the two titration curves.