(a) Interpretation: The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written. Concept introduction: According Bronsted-Lowry acid and base theory, acids are substance which loses protons H + to form conjugate base and bases are substances which accepts protons to from conjugate acid. For example: HA → H + + A − Here, HA is an acid as it donates a proton to form A − a conjugate base. Similarly, A − + H + → HA Here, A − is a base as it accepts a proton to from HA which is a conjugate acid.
(a) Interpretation: The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written. Concept introduction: According Bronsted-Lowry acid and base theory, acids are substance which loses protons H + to form conjugate base and bases are substances which accepts protons to from conjugate acid. For example: HA → H + + A − Here, HA is an acid as it donates a proton to form A − a conjugate base. Similarly, A − + H + → HA Here, A − is a base as it accepts a proton to from HA which is a conjugate acid.
The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.
Concept introduction:
According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.
For example:
HA→H++A−
Here, HA is an acid as it donates a proton to form A− a conjugate base.
Similarly,
A−+H+→HA
Here, A− is a base as it accepts a proton to from HA which is a conjugate acid.
Expert Solution
Answer to Problem 12QAP
(CH3)3N+H2O→(CH3)3NH++OH−
Explanation of Solution
The given species is (CH3)3N.
On reaction with water, it can act as a base by accepting hydrogen ion from the water molecule. The reaction is shown as follows:
(CH3)3N+H2O→(CH3)3NH++OH−
In the above reaction, (CH3)3N act as a base, H2O acts as an acid, (CH3)3NH+ is a conjugate acid and OH− is a conjugate base.
Therefore, (CH3)3N results in the formation of a basic aqueous solution.
Interpretation Introduction
(b)
Interpretation:
The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.
Concept introduction:
According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.
For example:
HA→H++A−
Here, HA is an acid as it donates a proton to form A− a conjugate base.
Similarly,
A−+H+→HA
Here, A− is a base as it accepts a proton to from HA which is a conjugate acid.
Expert Solution
Answer to Problem 12QAP
HC2O4−+H2O→H2C2O4+OH−
Explanation of Solution
The given species is HC2O4−.
On reaction with water, it can act as a base by accepting hydrogen ion from the water molecule. The reaction is shown as follows:
HC2O4−+H2O→H2C2O4+OH−
In the above reaction, HC2O4− act as a base, H2O acts as an acid, H2C2O4 is a conjugate acid and OH− is a conjugate base.
Therefore, HC2O4− results in the formation of a basic aqueous solution.
Interpretation Introduction
(c)
Interpretation:
The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.
Concept introduction:
According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.
For example:
HA→H++A−
Here, HA is an acid as it donates a proton to form A− a conjugate base.
Similarly,
A−+H+→HA
Here, A− is a base as it accepts a proton to from HA which is a conjugate acid.
Expert Solution
Answer to Problem 12QAP
CN−+H2O→HCN+OH−
Explanation of Solution
The given species is CN−.
On reaction with water, it can act as a base by accepting hydrogen ion from the water molecule. The reaction is shown as follows:
CN−+H2O→HCN+OH−
In the above reaction, CN− act as a base, H2O acts as an acid, HCN is a conjugate acid and OH− is a conjugate base.
Therefore, CN− results in the formation of a basic aqueous solution.
Interpretation Introduction
(d)
Interpretation:
The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.
Concept introduction:
According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.
For example:
HA→H++A−
Here, HA is an acid as it donates a proton to form A− a conjugate base.
Similarly,
A−+H+→HA
Here, A− is a base as it accepts a proton to from HA which is a conjugate acid.
Expert Solution
Answer to Problem 12QAP
S2−+H2O→HS−+OH−
Explanation of Solution
The given species is S2−.
On reaction with water, it can act as a base by accepting hydrogen ion from the water molecule. The reaction is shown as follows:
S2−+H2O→HS−+OH−
In the above reaction, S2− act as a base, H2O acts as an acid, HS− is a conjugate acid and OH− is a conjugate base.
Therefore, S2− results in the formation of a basic aqueous solution.
Interpretation Introduction
(e)
Interpretation:
The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.
Concept introduction:
According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.
For example:
HA→H++A−
Here, HA is an acid as it donates a proton to form A− a conjugate base.
Similarly,
A−+H+→HA
Here, A− is a base as it accepts a proton to from HA which is a conjugate acid.
Expert Solution
Answer to Problem 12QAP
BrO3−+H2O→HBrO3+OH−
Explanation of Solution
The given species is BrO3−.
On reaction with water, it can act as a base by accepting hydrogen ion from the water molecule. The reaction is shown as follows:
BrO3−+H2O→HBrO3+OH−
In the above reaction, BrO3− act as a base, H2O acts as an acid, HBrO3 is a conjugate acid and OH− is a conjugate base.
Therefore, BrO3− results in the formation of a basic aqueous solution.
Interpretation Introduction
(f)
Interpretation:
The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.
Concept introduction:
According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.
For example:
HA→H++A−
Here, HA is an acid as it donates a proton to form A− a conjugate base.
Similarly,
A−+H+→HA
Here, A− is a base as it accepts a proton to from HA which is a conjugate acid.
Expert Solution
Answer to Problem 12QAP
H2C6O5H7−+H2O→H3C6O5H7+OH−
Explanation of Solution
The given species is H2C6O5H7−.
On reaction with water, it can act as a base by accepting hydrogen ion from the water molecule. The reaction is shown as follows:
H2C6O5H7−+H2O→H3C6O5H7+OH−
In the above reaction, H2C6O5H7− act as a base, H2O acts as an acid, H3C6O5H is a conjugate acid and OH− is a conjugate base.
Therefore, H2C6O5H7− results in the formation of a basic aqueous solution.
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Chapter 13 Solutions
Student Solutions Manual For Masterton/hurley's Chemistry: Principles And Reactions, 8th
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