A student performed three CH₂Cl2 layer titrations in Part 2 using a standard sodium thiosulfate solution with a concentration of 0.01154 M. They reported the following measurements: Final CH₂Cl₂ Layer Burette Reading Initial CH₂Cl2 Layer Burette Reading Final Thiosulfate Burette Reading Initial Thiosulfate Burette Reading Determination #1 19.86 mL 12.44 mL 28.88 mL 1.23 mL Determination #2 27.53 mL 19.86 mL 29.22 mL 1.44 mL Determination #3 35.01 mL 27.53 mL 29.02 mL 1.18 ML How many moles of iodine did they use in their first titration (ie. their first determination)? Report your answer to the correct number of significant figures and only report the numerical value (no units).

A student performed three CH₂Cl2 layer titrations in Part 2 using a standard sodium thiosulfate solution with a concentration of 0.01154 M. They reported the following measurements: Final CH₂Cl₂ Layer Burette Reading Initial CH₂Cl2 Layer Burette Reading Final Thiosulfate Burette Reading Initial Thiosulfate Burette Reading Determination #1 19.86 mL 12.44 mL 28.88 mL 1.23 mL Determination #2 27.53 mL 19.86 mL 29.22 mL 1.44 mL Determination #3 35.01 mL 27.53 mL 29.02 mL 1.18 ML How many moles of iodine did they use in their first titration (ie. their first determination)? Report your answer to the correct number of significant figures and only report the numerical value (no units).

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 90AE: The following plot shows the pH curves for the titrations of various acids by 0.10 M NaOH (all of...

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Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
The following plot shows the pH curves for the titrations of various acids by 0.10 M NaOH (all of the acids were 50.0-mL samples of 0.10 M concentration). a. Which pH curve corresponds to the weakest acid? b. Which pH curve corresponds to the strongest acid? Which point on the pH curve would you examine to see if this acid is a strong acid or a weak acid (assuming you did not know the initial concentration of the acid)? c. Which pH curve corresponds to an acid with Ka 1 106?
Consider the following two acids: pKa1 = 2.98; pKa2 = 13.40 HO2CCH2CH2CH2CH2CO2H Adipic acid pKa1 = 4.41; pKa2 = 5.28 In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results.
Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.
Using Figure 17.11, suggest an indicator to use in each of the following titrations: (a) The weak base pyridine is titrated with HCl. (b) Formic acid is titrated with NaOH. (c) Ethylenediamine, a weak diprotic base, is titrated with HCl. Figure 17.11 Common acid-base indicators. The color changes occur over a range of pH values. Notice that o few indicators hove color changes over two different pH ranges.