Ka= Il0.265 0-2165 x2=7.685 x10-7 0.205-X [HC I0] C -x X+ X-8.166x10-5 E 0-2165-× H30+]=D6.76lex1D-6 2.Determine pH and percent ionization for a 0.015M acetic acid solution at 25°C. The Ka for acetic acid solution is Ka 1.8 X10-5 3. At 2000 °C the equilibrium constant for the reaction below is Kc= 2.4x103. If the initial concentration of NO is 0.500 M, what are the equilibrium concentrations of each substance? 2 NO (g) N2 (g) + 02 (g) 4. At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICI(g) = 12(g) + Cl2(g). What is the equilibrium concentration of ICI if 0. 45 mol of I2 and 0. 45 mol of Cl2 are initially mixed in a 2.0-L flask?

Ka= Il0.265 0-2165 x2=7.685 x10-7 0.205-X [HC I0] C -x X+ X-8.166x10-5 E 0-2165-× H30+]=D6.76lex1D-6 2.Determine pH and percent ionization for a 0.015M acetic acid solution at 25°C. The Ka for acetic acid solution is Ka 1.8 X10-5 3. At 2000 °C the equilibrium constant for the reaction below is Kc= 2.4x103. If the initial concentration of NO is 0.500 M, what are the equilibrium concentrations of each substance? 2 NO (g) N2 (g) + 02 (g) 4. At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICI(g) = 12(g) + Cl2(g). What is the equilibrium concentration of ICI if 0. 45 mol of I2 and 0. 45 mol of Cl2 are initially mixed in a 2.0-L flask?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.30QE

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