1. Consider the titration of 25.00 mL of 0.150 M acetic acid (HC,H3O2, Ka = 1.8 × 10) (aq) with 0.175 M NaOH(aq). What is the pH of the titration solution ... a. before any NaOH is added? b. ... after 10.00 mL of NaOH is added? c. ... at the equivalence point? Also, what volume of NaOH is required to reach this? d. For this titration, which is the best indicator to use: phenolphthalein, bromothymol blue, or methyl orange? Justify your answer.

1. Consider the titration of 25.00 mL of 0.150 M acetic acid (HC,H3O2, Ka = 1.8 × 10) (aq) with 0.175 M NaOH(aq). What is the pH of the titration solution ... a. before any NaOH is added? b. ... after 10.00 mL of NaOH is added? c. ... at the equivalence point? Also, what volume of NaOH is required to reach this? d. For this titration, which is the best indicator to use: phenolphthalein, bromothymol blue, or methyl orange? Justify your answer.

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 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...

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You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
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.
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1. Consider the titration of 25.00 mL of 0.150 M acetic acid (HC2H3O2, Ka = 1.8 × 10−5 ) (aq) with 0.175 M NaOH(aq). What is the pH of the titration solution . . . a. . . . before any NaOH is added? b. . . . after 10.00 mL of NaOH is added? c. . . . at the equivalence point? Also, what volume of NaOH is required to reach this? d. For this titration, which is the best indicator to use: phenolphthalein, bromothymol blue, or methyl orange? Justify your answer
A stainless steel alloy is to be analyzed for its chromium content. A 3.30 g sample of the steel is used to produce 250.0 mL of a solution containing Cr2O72−. A 10.0-mL portion of this solution is added to BaCl2(aq). When the pH of the solution is properly adjusted, 0.145 g BaCrO4(s) precipitates. A.) What is the percent Cr, by mass, in the steel sample? Express your answer numerically as a percentage.
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same) and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.