Please correct answer and don't used hand raiting Dilute solutions of the same weak acid (pKa =4.5) ranging in concentration from 2 x 10-6 M to 2 x 10-2 Mare titrated with a strong base that is five times more concentrated than the acid.At low concentrations of a weak acid, how does the concentration of the acid affect the shape of the titratThe lower the concentration of the acid, the sharper the inflection at the equivalence point.The shape of the titration curve depends only on the pKa of the acid, not its concentration.The higher the concentration of the acid, the sharper the inflection at the equivalence point.The shape of the titration curve is the same, regardless of the acid's concentration.

Let's evaluate each option:- 1) The lower the concentration of Acid, the sharper the inflection at…

Answered: Dilute solutions of the same weak acid…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.7QAP

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A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.
Consider the following pH curves for 100.0 mL of two different acids with the same initial concentration each titrated by 0.10 M NaOH. a. Which plot represents a pH curve of a weak acid, and which plot is for a strong acid? How can you tell? Cite three differences between the plots that help you decide. b. In both cases the pH is relatively constant before the pH changes greatly. Does this mean that at some point in each titration each solution was a buffered solution? c. True or false? The equivalence point volume for each titration is the same. Explain your answer. d. True or false? The pH at the equivalence point for each titration is the same. Explain your answer.
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
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.
Dilute solutions of the same weak acid (pKą = 4.5) ranging in concentration from 2 × 10-6 M to 2 × 10-2 M (0.002 to 20 mM) are titrated with a strong base that is five times more concentrated than the acid. At low concentrations of a weak acid, how does the concentration of the acid affect the shape of the titration curve? The higher the concentration of the acid, the sharper the inflection at the equivalence point. The lower the concentration of the acid, the sharper the inflection at the equivalence point. The shape of the titration curve is the same, regardless of the acid's concentration. The shape of the titration curve depends only on the pKa of the acid, not its concentration.
o A 55.0 mL solution of 0.150 M potassium alaninate ( H₂NC₂H₂CO₂K) is titrated with 0.150 M HCl. The pKa values for the amino acid alanine are 2.344 (pKal) and 9.868 (pK₂2), which correspond to the carboxylic acid and amino groups, respectively. Calculate the pH at the first equivalence point. pH = Calculate the pH at the second equivalence point. pH = H₂N- CH3 -CH- K Potassium Alaninate
Dilute solutions of the same weak acid (pK, = 4.5) ranging in concentration from 2 x 10 M to 2 x 10 M (0.002 to 20 mM) are titrated with a strong base that is five times more econcentrated than the acid. %3D At low concentrations of a weak acid, how does the concentration of the acid affect the shape of the titration curve? The shape of the titration curve depends only on the pK, of the acid, not its concentration. The lower the concentration of the acid, the sharper the inflection at the equivalence point. The shape of the titration curve is the same, regardless of the acid's concentration. The higher the concentration of the acid, the sharper the inflection at the equivalence point.
A 20.0-mL sample of a 0.125 M diprotic acid (H2A) solution is titrated with 0.1019 M KOH. The acid ionization constants for the acid are Ka1 = 5.2 * 10 - 5 and Ka2 = 3.4 * 10 - 10. At what added volume of base does each equivalence point occur?
5. A weak acid with pKa = 9.37 is titrated with 0.10 M NaOH. Which of the following is true about the pH of the solution at the equivalence point in this titration? A The pH at the equivalence point is below 7. B The pH at the equivalence point is equal to 7. C The pH at the equivalence point is above 7.
A 0.10 M weak acid is titrated with a 0.10 M strong base. Plot the titration curves on the same graph when the pK values of the acid are 4.0, 5.0 and 8.0.
A sample of 0,444 M methylamine (CH3NH2, K 4.29 x 10-) is titrated with 0.444M HCL What is the pH at the equivalence point? %3D

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