erences to acce Important question. In the laboratory, a general chemistry student measured the pH of a 0.445 M aqueous solution of triethanolamine, C6H1503N to be 10.720. Use the information she obtained to determine the Kb for this base. K₁(experiment) = Submit Answer Try Another Version 2 item attempts remaining

erences to acce Important question. In the laboratory, a general chemistry student measured the pH of a 0.445 M aqueous solution of triethanolamine, C6H1503N to be 10.720. Use the information she obtained to determine the Kb for this base. K₁(experiment) = Submit Answer Try Another Version 2 item attempts remaining

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.54QE: Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+,...

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12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’
How many significant figures are there in the following numbers: 10.78, 6.78, 0.78? If these were pH values, to how many significant figures can you express the [H+]? Explain any discrepancies between your answers to the two questions.
Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
The pH of 1.0 108 M hydrochloric acid is not 8.00. The correct pH can be calculated by considering the relationship between the molarities of the three principal ions in the solution (H+, Cl, and OH). These molarities can be calculated from algebraic equations that can be derived from the considerations given below. a. The solution is electrically neutral. b. The hydrochloric acid can be assumed to be 100% ionized. c. The product of the molarities of the hydronium ions and the hydroxide ions must equal Kw. Calculate the pH of a 1.0 108-M HCl solution.
A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
In the laboratory, a general chemistry student measured the pH of a 0.580 M aqueous solution of codeine, C18 H21 O3N to be 10.871. Use the information she obtained to determine the Kb for this base. Kb(experiment)=
0.185 M in HCHO2 (Ka = 1.8 ×x 10-4) and 0.230 M in HC2H3O2 (Ka = 1.8 × 10-5) Express your answer to two decimal places. ? Find the pH of each mixture of acids. pH = 2.11 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining In a mixture of two acids that have similar K, values, the dissociation of one acid affects the dissociation of the other acid, and vice versa. Prepare two ICE tables (where I means initial, C means change, and E means equilibrium), one for the dissociation of HCHO2 and one for the dissociation of HC2H3O2. Use the given acid-dissociation constants to calculate the amount of H3O+ produced by each acid in the pair. Part D 6.00x10-2 M in acetic acid (Ka = 1.8 × 10-5) and 6.00×102 M in hydrocyanic acid (Ka = 4.9 × 10-10) Express your answer to two decimal places. ? pH =
In the laboratory, a general chemistry student measured the pH of a 0.590 M aqueous solution of hypochlorous acid to be 3.829. Use the Information she obtained to determine the K₂ for this acid. Ka(experiment) = $ 4 Submit Answer 000 900 F4 R F % 5 T Use the References to access Important values if needed for this question. Retry Entire Group 9 more group attempts remaining G Cengage Learning Cengage Technical Support F5 ^ 6 MacBook Air - F6 Y H & 7 44 F7 U J * 00 8 ► 11 F8 9 K F9 O 1 0 L F10 P Previous Next> F11 + 11 = Save and Exit F12