Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula hydrocyanic acid HCN 4.9 × 10¬10 ethylamine C,H,NH2| 6.4 × 10¯4 hypochlorous acid HCIO 3.0 x 10-8 C,H5NH, 4.3 × 10~10 dlo aniline Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M NaNO3 choose one v 0.1 М КСIO choose one v 0.1 M C6H5NH3BR choose one v 0.1 M NaCN v choose one 1 (lowest) 3

Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula hydrocyanic acid HCN 4.9 × 10¬10 ethylamine C,H,NH2| 6.4 × 10¯4 hypochlorous acid HCIO 3.0 x 10-8 C,H5NH, 4.3 × 10~10 dlo aniline Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M NaNO3 choose one v 0.1 М КСIO choose one v 0.1 M C6H5NH3BR choose one v 0.1 M NaCN v choose one 1 (lowest) 3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 175CWP: Consider 0.10 M solutions of the following compound: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these...

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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.
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
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.
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Each of the following statements concerns a 0.10 M solution of a weak organic base, B. Briefly describe why each statement is either true or false. a [B] is approximately equal to 0.10 M. b [B] is much greater than [HB+]. c [H3O+] is greater than [HB+]. d The pH is 13. e [HB+] is approximately equal to [OH]. f [OH] equals 0.10 M.
Consider 0.10 M solutions of the following compound: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these solutions in order of increasing pH.
A student is asked to bubble enough ammonia gas through water to make 4.00 L of an aqueous ammonia solution with a pH of 11.55. What volume of ammonia gas at 25C and 1.00 atm pressure is necessary?
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