The ionization constant of the strongest acid isHA Ka = 7.2 x 1o-4HB Ka = 8.5 x 10-8HC Ka = 7.5 x 10-5HD Ka = 6.5 x 10-10%3D

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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section14.9: Lewis Acids And Bases

Problem 14.26E

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33. The ionization constant of the strongest acid is a HA Ka = 7.2 x 10-4 b HB Ka = 8.5 x 10-8 c HC Ka = 7.5 x 10-5 d HD Ka = 6.5 x 10-10
Given the information about the following acids:i= HW pKa = 2ii= HX pKa = 6iii= HY pKa = 10iv= HZ pKa = 20Which conjugate base of these acids will react almost completely with water to hydroxide ion? none all of them HZ HY and HZ
What is the acid dissociation constant Ka for its conjugate acid? If the base dissociation constant Kb for hypochlorite ion is 3.3x10-7
Calculate the pH values of the following solutions: a. a 1.0 M solution of acetic acid (pKa = 4.76) b. a 0.1 M solution of protonated methylamine (pKa = 10.7) c. a solution containing 0.3 M HCOOH and 0.1 M HCOO - (pKa of HCOOH = 3.76)
Some H2CO3 and HCO3- are added to water such that the concentration of each is the same value, 12.0 mmol L-1 (pKa = 6.3, 10.3). The water was initially at pH 7.05 and 25.0 °C. Calculate ΔGrxn in kJ mol-1. (R = 8.3145 J mol-1 K-1)
Determine the principal species at the following pH levels for Nitrilotriacetic acid. The most protonated form is C6H10NO6+. pH= 1,2,3,4,10. pK1 = 1.0, pK2 = 1.81, pK3 = 2.52, pK4 = 9.46.
Calculate the pH of a 0.30 M solution of NH 4Cl (Kb for NH 3 = 1.8 x 10 -5). a. 11.67 b. 9.11 c. 4.89 d. 3.33 e. 7.00
please help! Formic acid (Ka = 1.8 x 10-4) is used as a preservative on hay and animal feed. Hypobromous acid (Ka = 2.0 x 10-9) is used as a germicidal agent for pools and spas. An agricultural chemist wishes to test whether a mixture of the two would be more effective in preventing hay decay over the winter months. Calculate the pH of a solution that is 0.050 M in hypobromous acid and 0.025 M in formic acid.
Calculate the pH of a 0.35 M solution of pyridine (C5H5N; Kb = 1.7 x 10^-9) A. 4.61 B. 4.77 C. 9.39 D. 9.23 E. none of these
What is Ka for the conjugate acid of C₅H₅N (Kb = 1.7 × 10⁻⁹)?
The pH of a 0.25 M solution of a weak monobasic base is 8.76 at 25 oC. Calculate Kb for the base. 3.31 x 10-11 1.32 x 10-10 1.21 x 10-17 5.75 x 10-6 1.74 x 10-9
What is the pH of 0.0050 M NH3 (Kb = 1.8 x 10-5) 10.48 3.52 11.70 2.30

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