Equal volumes of two different weak acids are titrated with 14 0.30 M NAOH, resulting in the following titration curves. 12 10 Which curve corresponds to the titration of the more concentrated weak acid solution? 8- the concentrations are equal 6. the lower, blue curve 4 cannot be determined the upper, red curve 2 10 20 30 40 50 mL NaOH Which curve corresponds to the titration of the weak acid with a larger Ką? the Ka values are equal the lower, blue curve the upper, red curve cannot be determined Hd

Equal volumes of two different weak acids are titrated with 14 0.30 M NAOH, resulting in the following titration curves. 12 10 Which curve corresponds to the titration of the more concentrated weak acid solution? 8- the concentrations are equal 6. the lower, blue curve 4 cannot be determined the upper, red curve 2 10 20 30 40 50 mL NaOH Which curve corresponds to the titration of the weak acid with a larger Ką? the Ka values are equal the lower, blue curve the upper, red curve cannot be determined Hd

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 34QRT

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When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
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.)
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.
Consider die titration of 50.0 mL of 0.10 M H3A (Ka1 = 5.0 104, Ka2 = 1.0 108, Ka3 = 1.0 1012) titrated by 0.10 M KOH. a. Calculate the pH of the resulting solution at 125 mL of KOH added. b. At what volume of KOH added does pH = 3.30? c. At 75.0 mL of KOH added, is the solution acidic or basic?