At the equivalence point, the following titrations (just a mixture of two solutions) give either acidic or basic solutions. mixture Type of solution Relevant K values а. NaOH + HCN basic K, of HCN = 4.9 x 10-10 b. NaOH + HNO2 basic Ka of HNO2 4.0 x 10-4 %3D c. HCI + NH3 acidic K, of NH3 = 1.8 x 10-5 %3D For each mixture, (1) write the major species present at the equivalence point, and (2) equilibrium reaction that produces the acidic or basic solution.
At the equivalence point, the following titrations (just a mixture of two solutions) give either acidic or basic solutions. mixture Type of solution Relevant K values а. NaOH + HCN basic K, of HCN = 4.9 x 10-10 b. NaOH + HNO2 basic Ka of HNO2 4.0 x 10-4 %3D c. HCI + NH3 acidic K, of NH3 = 1.8 x 10-5 %3D For each mixture, (1) write the major species present at the equivalence point, and (2) equilibrium reaction that produces the acidic or basic solution.
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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 7RQ: Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations...
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Question
![At the equivalence point, the following titrations (just a
mixture of two solutions) give either acidic or basic solutions.
mixture
Type of solution
Relevant K values
а. NaOH + HCN
basic
K, of HCN = 4.9 x 10-10
b. NaOH + HNO2
basic
Ka of HNO2 = 4.0 x 10-4
c. HCI + NH3
acidic
K, of NH3 = 1.8 x 10-5
For each mixture, (1) write the major species present at the equivalence point, and (2)
equilibrium reaction that produces the acidic or basic solution.
mixture
(1) Major species
present at eq. pt. after
the two species react
(don't include water)
(2) Equilibrium reaction with water (exclude
spectator ions that don't participate in the reaction)
NOTE: This reaction predicts the pH of the solution.
а. NaOH + HCN
b. NaOH + HNO2
c. HCI + NH3
Rank the solutions from lowest pH to highest pH, assuming the total volume and molarities
of products is the same.
Lowest pH
Highest pH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F668f7243-fecb-4dca-9846-a35dbaef67d8%2Fa187fe94-c9f9-4473-9546-67507019a18e%2Fca36dip_processed.png&w=3840&q=75)
Transcribed Image Text:At the equivalence point, the following titrations (just a
mixture of two solutions) give either acidic or basic solutions.
mixture
Type of solution
Relevant K values
а. NaOH + HCN
basic
K, of HCN = 4.9 x 10-10
b. NaOH + HNO2
basic
Ka of HNO2 = 4.0 x 10-4
c. HCI + NH3
acidic
K, of NH3 = 1.8 x 10-5
For each mixture, (1) write the major species present at the equivalence point, and (2)
equilibrium reaction that produces the acidic or basic solution.
mixture
(1) Major species
present at eq. pt. after
the two species react
(don't include water)
(2) Equilibrium reaction with water (exclude
spectator ions that don't participate in the reaction)
NOTE: This reaction predicts the pH of the solution.
а. NaOH + HCN
b. NaOH + HNO2
c. HCI + NH3
Rank the solutions from lowest pH to highest pH, assuming the total volume and molarities
of products is the same.
Lowest pH
Highest pH
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