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?
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
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Chapter16: Acids And Bases
Section: Chapter Questions
Problem 65AP: . The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in...
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4-)
![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?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F57c52580-fa5a-4aad-906a-3a46491efd67%2Fc6f3bfc0-db99-4b32-baf3-bd06e86d342a%2Fv9mzzqq.jpeg&w=3840&q=75)
Transcribed Image Text: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?
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