ex1 Name:Mr. B8.3-Base lonizationBy the end of this section, I will be able to:the solve problems related to equilibrium by performing calculations involving concentrations ofreactants and productsbase-dissociation constant, or base-ionization constant, K,The Base-Ionization Constant, K₁:SCH4U8.3✓identify common equilibrium constants, including K., Kap, Kw, Ka, K, and Kp, and write theexpressions for each✓explain the Arrhenius and Brønsted-Lowry theories of acids and basesKey Terms:100-meSame deal as acids and Ka, except for bases. The base-dissociation constant (or base-ionizationconstant), Kb, is an equilibrium constant for the dissociation/ionization of a base.B(aq) + H₂O(1)BH(aq) + OH(aq)K₁ =[BH][OH][B(aq)]To solve problems involving bases is the same protocol as it is for acids, except:the reaction and ICE table involves OH, instead of H₂O*the final concentration will be for OH, instead of H₂O*, so will result in pOH which needs tochange to pHCDate:ex1. One of the uses for aniline is the manufacturing of dyes. Aniline is soluble in water and acts as aweak base. When a solution containing 5.0 g/L of aniline was prepared, the pH was determined to be8.68. Calculate the base-ionization constant, Kb, for aniline.(ans Kb=4.3*10-¹0)CHẠNH,12(aq) + H₂O(1) C₂H₂NH3(g) + OH(aq)Ø7.5810-10-3+xE1.5x10-XPage 1 of 214Leex2. The characteristic bitter taste of tonic water is due to the addition of quinine. Quinine is a natura(ans pH=occurring white crystalline compound. It is used to treat malaria. The K, for quinine is 3.3*10. Wh-the pH of a 3.6*10³ mol L solution of quinine?C20H24N₂O2(aq) + H₂O(C20H24N₂O₂H(aq) + OH(aq)

pH of the solution = 8.68 Concentration of aniline solution = 5.0 g/L

change to pH ex1. One of the uses for aniline is the manufacturing of dyes. Aniline is soluble in water and acts as a weak base. When a solution containing 5.0 g/L of aniline was prepared, the pH was determined to be 8.68. Calculate the base-ionization constant, K, for aniline. (ans K₂=4.3*10-¹0) CH_NH, * H,O < CHẠNH H₂O) I 7.5810-10:5 13(aq) + OH (2₂) Ø +x

change to pH ex1. One of the uses for aniline is the manufacturing of dyes. Aniline is soluble in water and acts as a weak base. When a solution containing 5.0 g/L of aniline was prepared, the pH was determined to be 8.68. Calculate the base-ionization constant, K, for aniline. (ans K₂=4.310-¹0) CH_NH, H,O < CHẠNH H₂O) I 7.5810-10:5 13(aq) + OH (2₂) Ø +x

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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