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=4.3*10-¹0) CH_NH, * H,O < CHẠNH H₂O) I 7.5810-10:5 13(aq) + OH (2₂) Ø +x
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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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Question
ex1
![Name:
Mr. B
8.3-Base lonization
By the end of this section, I will be able to:
the solve problems related to equilibrium by performing calculations involving concentrations of
reactants and products
base-dissociation constant, or base-ionization constant, K,
The Base-Ionization Constant, K₁:
SCH4U
8.3
✓identify common equilibrium constants, including K., Kap, Kw, Ka, K, and Kp, and write the
expressions for each
✓explain the Arrhenius and Brønsted-Lowry theories of acids and bases
Key Terms:
100-me
Same deal as acids and Ka, except for bases. The base-dissociation constant (or base-ionization
constant), 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 to
change to pH
C
Date:
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, Kb, for aniline.
(ans Kb=4.3*10-¹0)
CHẠNH,
12(aq) + H₂O(1) C₂H₂NH3(g) + OH(aq)
Ø
7.5810-10-3
+x
E
1.5x10-X
Page 1 of 2
14
Le
ex2. 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)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0b708563-5b0b-48a0-87b8-404b78fa66c6%2F4290719a-8eb1-4dfa-8313-eca289b03137%2Fh2l8by_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Name:
Mr. B
8.3-Base lonization
By the end of this section, I will be able to:
the solve problems related to equilibrium by performing calculations involving concentrations of
reactants and products
base-dissociation constant, or base-ionization constant, K,
The Base-Ionization Constant, K₁:
SCH4U
8.3
✓identify common equilibrium constants, including K., Kap, Kw, Ka, K, and Kp, and write the
expressions for each
✓explain the Arrhenius and Brønsted-Lowry theories of acids and bases
Key Terms:
100-me
Same deal as acids and Ka, except for bases. The base-dissociation constant (or base-ionization
constant), 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 to
change to pH
C
Date:
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, Kb, for aniline.
(ans Kb=4.3*10-¹0)
CHẠNH,
12(aq) + H₂O(1) C₂H₂NH3(g) + OH(aq)
Ø
7.5810-10-3
+x
E
1.5x10-X
Page 1 of 2
14
Le
ex2. 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)
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