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
The end point for a titration can be determined graphically. The end point volume for a first derivative plot corresponds to: The volume base added where the first derivative curve has minimum slope The volume base added where the first derivative curve has a maximum negative slope The volume base added where the first derivative curve crosses the y-axis The volume base added where the first derivative curve has maximum slope (OG) The volume base added where the first derivative curve crosses the x-axis
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
The following data was collected when a 25 mL sample of an unknown acid is titrated with a 1.00 M NaOH Solutio. Determine Ka for the unknown acid.
Interpret pH titration plots. Answer the following about the titration plot shown below, involving a monoprotic acid and base. 20 mL of 0.1M titrand titrated with 0.1M titrant. Data points at 1 mL increments. 14.0 12.0 10.0 5 8.0 6.0 4.0 2.0 0.0 seededood 0 0.0 10.0 مهمه 20.0 30.0 Volume of titrant (mL) (a) Is the species being titrated an acid or a base? (b) Is the species being titrated strong or weak? (c) What is the value of Ka (if a weak acid) or K, (if a weak base) for the species being titrated? If the species is strong (100% dissociated), enter 999. rààààààààà 40.0 50.0
For each of the three titrations, determine the expected pH at each of the following 4 points in the titration. Assume that all acids are exactly 0.1 M and that all bases are exactly 0.2 M for purposes of your calculations. Round your final pH values to the nearest 0.1 pH units since that is how we read the experimental values. The 4 points for which the pH values are to be calculated are: a) after 0 ml of base have been added (initial pH) b) after 10.0 mL of base have been added (halfway to the equivalence point) after 20.0 mL of base have been added (equivalence point) c) after 20.0 mL of base have been added (equivalence point) d)after 25.0 mL of base have been added (5 ml past the equivalence point)
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

A student obtains the following data from the Determining the pKa of an Acid-Base Indicator experiment. Using this data, calculate the pKa of the indicator in the fourth solution. Solution Abs. pH 3.4 + HCI 0.054 pH 4.6 + NaOH 0.564 Sample # actual pH Abs. 1 3.48 0.130 2345 3.77 0.217 3.99 0.296 4.37 0.388 4.54 0.468 Your Answer: Answer (2 points) After creating a graph of pH versus log([HIn]/[In-]), the following trendline is obtained. = -1.0291× + 3.721 y=-1 Calculate the pKa of bromophenol blue from this data to three decimal places. Your Answer: Answer MacBook Pro

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