The degree of dissociation of acids is often expressed in terms of pKa. pka then isDirectly measured by titration of the acid with sodium hydroxideCalculated by determining the acid's buffer capacityDirectly determined by conductivity measurementThe natural log of the acid's dissociation constantThe reciprocal log of the dissociation constant

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Answered: The degree of dissociation of acids is…

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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Calculating the pH of a weak base titrated with a strong acid An analytical chemist is titrating 104.1 mL of a 0.1200M solution of propylamine (C,H,NH,) with a 0.2600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 53.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume eguals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility APR 23 MacBook Air O00 000 F4
Consider the titration of 100.0 mL of 0.100 M acetic acid (Ka = 1.8 x 105). When 50.00 mL of 0.100 M NaOH is added to the acetic acid solution, calculate the pH of the resulting mixture. Use the simultaneous equations method, showing the derivation of the final equation you used to calculate pH and justify any assumptions made in your derivation.
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A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with standardized 0.113 M HCÌi and the pH of the solution was plotted as a function of titrant added (shown below). Titration of a Weak Base With 0.113 M HCI 12 10 10 20 30 40 50 60 70 80 90 Volume of HCl added (ml) Possible identities for the three liquid bases are shown in the table below. Base pyrole pyrimidine pyridine triethylamine 2.51 x 10-14 1.25 x 10-13 1.70 x 10-9 5.30 x 104 Density (g/mL) 0.967 1.02 0.982 0.762 Based on the data above, identify the weak base and explain your selection. The best explanations will account for all relevant experimental data. Additionally, suggest an indicator to use for this titration if it were to be done without a pH meter. Hd
Describe the pH changes that occur during the titration of a weak base by a strong acid. What is meant by the term equivalence point?
An analytical chemist is titrating 208.8mL of a 0.7500M solution of methylamine CH3NH2 with a 0.5600M solution of HNO3 . The pKb of methylamine is 3.36 . Calculate the pH of the base solution after the chemist has added 236.8mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.
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Cesium buffer helps in determining easily ionizable elements in ICP-MS and ICP-OES. But how? Cesium is easily ionizable element it produces more electrons in the plasma. In principle it should also suppress the ionization of metal of our interest. In that case Cesium buffers interferes our analysis. I don’t understand why Cesium helps to reduce the ionization of sodium and potassium, not the ionization of metal of our interest. Can you please explain how cesium helps to reduce the ionization of only a specific metal not the metal of interest?
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