Using the Brønsted-Lowry model, write equations to show why the following species behave as weak acids in water. (a) Ni(H 2 O) 5 OH + (b) Al(H 2 O) 6 3+ (c) H 2 S (d) HPO 4 2-(e) HClO 2 (e) Cr(H 2 O) 5 (OH) +
Using the Brønsted-Lowry model, write equations to show why the following species behave as weak acids in water.
(a) Ni(H2O)5OH+(b) Al(H2O)63+(c) H2S
(d) HPO42-(e) HClO2 (e) Cr(H2O)5(OH)+
Expert Solution
Interpretation Introduction
(a)
Interpretation:
The equation to show the acidic 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.
Answer to Problem 9QAP
Ni(H2O)5OH++H2O→Ni(H2O)5O+H3O+
Explanation of Solution
The given species is Ni(H2O)5OH+.
On reaction with water, it can act as an acid by donating hydrogen ion to the water. The reaction is shown as follows:
Ni(H2O)5OH++H2O→Ni(H2O)5O+H3O+
In the above reaction, Ni(H2O)5OH+ acts as an acid, H2O acts as a base, Ni(H2O)5O is a conjugate base and H3O+ is a conjugate acid.
Expert Solution
Interpretation Introduction
(b)
Interpretation:
The equation to show the acidic 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.
Answer to Problem 9QAP
Al(H2O)63++H2O→Al(H2O)52+(OH)+H3O+
Explanation of Solution
The given species is Al(H2O)63+.
On reaction with water, it can act as an acid by donating hydrogen ion to the water. The reaction is shown as follows:
Al(H2O)63++H2O→Al(H2O)52+(OH)+H3O+
In the above reaction, Al(H2O)63+ acts as an acid, H2O acts as a base, Al(H2O)52+(OH) is a conjugate base and H3O+ is a conjugate acid.
Expert Solution
Interpretation Introduction
(c)
Interpretation:
The equation to show the acidic 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.
Answer to Problem 9QAP
H2S+H2O→HS−+H3O+
Explanation of Solution
The given species is H2S.
On reaction with water, it can act as an acid by donating hydrogen ion to the water. The reaction is shown as follows:
H2S+H2O→HS−+H3O+
In the above reaction, H2S acts as an acid, H2O acts as a base, HS− is a conjugate base and H3O+ is a conjugate acid.
Expert Solution
Interpretation Introduction
(d)
Interpretation:
The equation to show the acidic 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.
Answer to Problem 9QAP
HPO42−+H2O→PO43−+H3O+
Explanation of Solution
The given species is as follows:
HPO42−
On reaction with water, it can act as an acid by donating hydrogen ion to the water. The reaction is shown as follows:
HPO42−+H2O→PO43−+H3O+
In the above reaction, HPO42− acts as an acid, H2O acts as a base, PO43− is a conjugate base and H3O+ is a conjugate acid.
Expert Solution
Interpretation Introduction
(e)
Interpretation:
The equation to show the acidic 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.
Answer to Problem 9QAP
HClO2+H2O→ClO2−+H3O+
Explanation of Solution
The given species is as follows:
HClO2
On reaction with water, it can act as an acid by donating hydrogen ion to the water. The reaction is shown as follows:
HClO2+H2O→ClO2−+H3O+
In the above reaction, HClO2 acts as an acid, H2O acts as a base, ClO2− is a conjugate base and H3O+ is a conjugate acid.
Expert Solution
Interpretation Introduction
(f)
Interpretation:
The equation to show the acidic 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.
Answer to Problem 9QAP
Cr(H2O)5(OH)++H2O→Cr(H2O)5O+H3O+
Explanation of Solution
The given species is as follows:
Cr(H2O)5(OH)+
On reaction with water, it can act as an acid by donating hydrogen ion to the water. The reaction is shown as follows:
Cr(H2O)5(OH)++H2O→Cr(H2O)5O+H3O+
In the above reaction, Cr(H2O)5(OH)+ acts as an acid, H2O acts as a base, Cr(H2O)5O is a conjugate base and H3O+ is a conjugate acid.
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