Using the table of indicators identify which of the given indicators would be appropriate for the titration represented in the titration curve. 2,4,6-trinitrotoluene ☐quinaldine red metacresol purple malachite green thymol blue alizarin yellow R 13 12 11 10 9 8 pH 7 6 5 NWAC 4 3 2 1 0 2 4 Titration Curve 6 8 10 12 14 Volume of Titrant (mL) 16 18 20

Using the table of indicators identify which of the given indicators would be appropriate for the titration represented in the titration curve. 2,4,6-trinitrotoluene ☐quinaldine red metacresol purple malachite green thymol blue alizarin yellow R 13 12 11 10 9 8 pH 7 6 5 NWAC 4 3 2 1 0 2 4 Titration Curve 6 8 10 12 14 Volume of Titrant (mL) 16 18 20

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 18Q: Acidbase indicators mark the end point of titrations by magically turning a different color. Explain...

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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.)
A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
2. What is the pH at the equivalence point in the titration of 25.0 mL of 0.090 M phenol (Ka = 1.3 × 10−10) with 0.108 M NaOH? 7.00 5.65 8.98 11.29
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.
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
Acidbase indicators mark the end point of titrations by magically turning a different color. Explain the magic behind acidbase indicators.
Instead of the titration of a strong acid by a strong base considered in Question 5, consider the titration of a strong base by a strong acid. Compare and contrast a strong acidstrong base titration with a strong basestrong acid titration.
Titration Curve Using the table of indicators identify which of the given 13 12 indicators would be appropriate for the titration 11 10 represented in the titration curve. 9 thymol blue 8 pH 7 6 alizarin yellow R 5 O quinaldine red 4 3 O clayton yellow 2 1 metacresol purple 4 6 8 10 12 14 16 18 20 Volume of Titrant (mL) O methyl green 2.
What indicators is best suitable for this titration curve of a weak acid & a strong base?
Titration Curve Using the table of indicators identify which of the given 13 12 indicators would be appropriate for the titration 11 10 represented in the titration curve. 9 thymol blue 8 metacresol purple pH 7 phenol red alizarin O metanil yellow 0 2 6 8 10 12 14 16 18 20 thymolphthalein Volume of Titrant (mL) 4. O54 321
14. Consider this titration curve and answer questions a-h. (2 pts each) 14 12 10 pH 9. 10 15 20 25 30 35 40 ml base added a) This is a (strong/weak) acid titrated with a strong base. b) Place a dot () on the curve at the equivalence point. c) The pH at the equivalence point is d) What volume of base was used to titrate the acid solution to the equivalence point? e) Place a box () on the curve at the half-equivalence point. ) What is the pH at this point?
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