Arrange the following solution fromlowest pH to highest pH:0.20 М СН,СООН (К, — 1.8 х 10-5)0.06 М СH,COОН (К, — 1.8 х 10-5)0.75 М CH,СООН (К, 3 1.8 х 10-)%3D%3DSectionа.0.20 М СH3СООН < 0.06 MCH-COОH <0.75 М СH,COОНb. 0.75 М СH,CООН < 0.06 МCH;COOHCH;COOH0.20МС.0.06 М СH,СООН < 0.20 МCH-COОH <0.75 М СH,COОНd. p.75 M CН,СООН < 0.20 мCH-COОH <0.06 М СH,COОН

The correct answer about pH is given below

Arrange the following solution from lowest pH to highest pH: 0.20 М СH,СООН (К, — 1.8 х 10-5) 0.06 M СН,CООН (К, %3 1.8 х 10-5) 0.75 М CH,CООН (К, — 1.8 х 10-5) а. Section 0.20 M СH,СООН < 0.06 м CH-COОH <0.75 М СН,СООН b. 0.75 M СH,COОH < 0.06 М CH;COOH 0.20 M CH;COOH с. 0.06 М СH,COОH < 0.20 М CH-COОH <0.75 М СН,СООН d. p.75 M CH,COОН < 0.20 М CH-COОН <0.06 М CH,CООН

Arrange the following solution from lowest pH to highest pH: 0.20 М СH,СООН (К, — 1.8 х 10-5) 0.06 M СН,CООН (К, %3 1.8 х 10-5) 0.75 М CH,CООН (К, — 1.8 х 10-5) а. Section 0.20 M СH,СООН < 0.06 м CH-COОH <0.75 М СН,СООН b. 0.75 M СH,COОH < 0.06 М CH;COOH 0.20 M CH;COOH с. 0.06 М СH,COОH < 0.20 М CH-COОH <0.75 М СН,СООН d. p.75 M CH,COОН < 0.20 М CH-COОН <0.06 М CH,CООН

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 17ALQ

See similar textbooks

Similar questions

Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
Estimate the pH of a solution in which bromcresol green is blue and thymol blue is yellow. (See Fig. 14-8.)
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.
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.
Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 13-2 and 13-3. a. NaNO3 b. NaNO2 c. C5H5NHClO4 d. NH4NO2 e. KOCl f. NH4OCl
Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide