Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula -8 HONH, 1.1 × 10 hypochlorous acid HCIO 3.0 × 10 hydroxylamine -8 C,H,NH, 6.4 × 10* dlo hydrofluoric acid HF 6.8 x 10 ethylamine Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to thể s 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 М КСI choose one 0.1 M KCIO choose one 0.1 M HONH3Br choose one v 0.1 M NaF choose one

Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula -8 HONH, 1.1 × 10 hypochlorous acid HCIO 3.0 × 10 hydroxylamine -8 C,H,NH, 6.4 × 10* dlo hydrofluoric acid HF 6.8 x 10 ethylamine Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to thể s 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 М КСI choose one 0.1 M KCIO choose one 0.1 M HONH3Br choose one v 0.1 M NaF choose one

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 191MP

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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.
. 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.
. Strong buses are bases that completely ionize in water to produce hydroxide ion, OH-. The strong bases include the hydroxides of the Group I elements. For example, if 1.0 mole of NaOH is dissolved per liter, the concentration of OH ion is 1.0 M. Calculate the [OH-], pOH, and pH for each of the following strong base solutions. a. 1.10 M NaOH b. 2.0104M KOH c. 6.2103M CsOH d. 0.0001 M NaOH
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.
Note whether hydrolysis occurs for each of the following ions. If hydrolysis docs occur, write the chemical equation for it. Then write the equilibrium expression for the acid or base ionization (whichever occurs). a NO3 b OCl c NH2NH3+ d Br
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?