Use excel to plot the following titration data. Once you have done your plot, make sure to label the axescorrectly. Use your graph to determine the pK, for the weak acid. Attach your plot to the back of thisworksheet.A 1.0M solution of weak acid was titrated with a base and the following data was collected.Equivalents of BasepH observed0.053.40.153.90.254.20.404.50.604.90.755.20.855.40.956.0

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Answered: Use excel to plot the following…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

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Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA. and 100.0 mL of 0.10 M HCl. In calculating the pH for the final solution, you would make some assumptions about the order in which various reactions occur to simplify the calculations. State these assumptions. Does it matter whether the reactions actually occur in the assumed order? Explain.
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
You have 0.10-mol samples of three acids identified simply as HX, HY, and HZ. For each acid, you make up 0.10 M solutions by adding sufficient water to each of the acid samples. When you measure the pH of these samples, you find that the pH of HX is greater than the pH of HY, which in turn is greater than the pH of HZ. a Which of the acids is the least ionized in its solution? b Which acid has the largest Kd?
A 10.0 mL solution of 0.330 M NH, is titrated with a 0.110 M HCI solution. Calculate the pH after the following additions of the HC1 solution: 0.00 mL,10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places. Note: Reference the Ka of acids at 25 °C and Kb of bases at 25 °C tables for additional information.
A 10.0 ml. solution of 0.300 M NH, is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the HCI solution: 0.00 ml., 10.0 ml., 30.0 ml., and 40.0 ml.. Round your answer to 3 decimal places. Note: Reference the K, of acids at 25 °C and K, of bases at 25 °C tables for additional information. Part 1 of 4 0.00 ml. Added, pH= Part 2 of 4 10.0 mL Added, pH = 0.. 0.8
2. In titration experiment at 25°C, a total of 30 mL of 0.1 M NaOH was added dropwise to conical flask containing 25 mL of 0.1 M HCI and few drops of an indicator. Calculate the pH of the solution before the addition of NaOH, at half equivalence point and at the final volume of titration. Sketch a graph of pH against the volume of NaOH added. What is an acid-base indicator? By referring to Table 1 below, suggest the most suitable indicator to be used in the titration above and justify your answer. Table 1 pH range Indicator Phenolphthalein Cresol red 8.3-10,0 7.0-8.8 Bromothymol blue 6.0-7.6 Litmus 4.7-8.3
E University Librarie. E UNIVERSITY POR. Student Detail Sc. Part A The table shows respective color change when a universal indicator is added to the clear solutions. Rank the samples based on increasing order of acid strength. Solutions Color change 0.001 M lactic Light red 0.01 M phenol Light yellow 0.01 M nitrous acid Light orange 0.001 M hydrogen peroxide Light green Rank the solutions by Increasing order of their acid strength. To rank items as equivalent, overlap them. > View Available Hint(s) Reset Help 0.01 Mnitrous acid 0.001 Mlactic acid 0.001 M hydrogen peroxide 0.01 Mphenol Least acidic Most acidic P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions | Contact Us | MacBook Air 80 888 DII DD F3 F4 F5 F6 F7 F8 F9 F10 F11 $ & 3 4 7 8. 9. { R Y U 一 F J K く C V B N M + I| .. .- エト

Methyl red has apk, of 5.0 and is red in its acid form and yellow in its basic form. Part A If several drops of this indicator are placed in a 28.0-mL sample of 0.110M HCI, what color will the solution appear? O yellow O red Submit Request Answer Part B If 0.110 M NAOH is slowly added to the a sample, in what pH range will the indicator change color? Express your answers using one decimal place. Enter your answers in ascending order separated by a comma. ν ΑΣΦ pH. pH3 Submit Request Answer
13) Bromthymol blue (BTB) is a chemical indicator that is blue all alone. When combined with a basic solution, it turns green as a solution becomes more acidic it turns yellow in an acidic solution. Fill in what color you think bromthymol blue would be in each of the situations in the chart. If solution color is given, simply provide a logical, possible pH value based on the outcomes. Fill in the missing ions as well! Situation pH BTB color Ion present Water directly out of tap 7.2 pH after exhaled air is blown through a straw into water for 5 5.1 H+ min. 14 pH after a snail has lived in water for three days Very Yellow pH with 2mL of bleach added to the water Very Blue 5.0 pH with instant coffee added to the water pH after an aquatic plant is grown in water for three days in bright sunlight Light Blue OH- 14)Is BTB a chemical indicator? 15) What then does it "indicate"? 16) Based on the data above, why does drinking coffee cause stomach pain for some indivudals? 17) What effect does…
Based on that experimental titration curve of the IU unknown sample, can you sketch out the titration curve if both the starting weak acid solution and the NaOH solution are diluted 10 times? What about diluting another 10 times on top of that? Particularly, you should pay attention to the size of the pH jumps around each equivalence point, as well as the relative positions of the flat regions before or after the pH jumps. For the sake of simplicity, no need to consider activity in this exercise.
Give the name of another weak base that will have a similar titration curve. Briefly explain the reason for the similarity. (Weak acid given is TRIS base) - [ ] Before strong acid is added to weak base: pH is between 10 and 11 - [ ] After 10 mL of strong acid to weak base: pH is between 8 and 9 - [ ] After 25 mL of strong acid is added to weak base: pH is between 8 and 9 - [ ] After 40 mL of strong acid is added to weak base: pH is between 7 and 8 - [ ] After 50 mL of strong acid is added to weak base: pH is between 4 and 5 - [ ] After 60 mL of strong acid is added to weak base: pH is between 2 and 3
Answer the following questions about the titration curve shown below. a) Choose the correct words from each pair, then explain your reasoning.The sample is a [ strong / weak ] [ acid / base ].The titrant is a [ strong / weak ] [ acid / base ]. b) What is the equivalence point volume and pH for this titration? How do you know? c) A 50.0 mL sample was titrated with 0.20 M titrant to create the titration curve. Calculate the original concentration of the sample.

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