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Answer:
B. False
A. True
B. False in
Explanation:
1.
From Bronsted-Lowrys definition of Acids and bases, a strong acid is a substance that gives up a proton (to form a weak conjugate base), while a strong base is one that willingly accepts a proton.
Therefore in the reaction,
HA(aq) + H2O (l) ⇌ H3O+ (aq) + A-
The stronger HA is, the weaker the A- and vice versa; the weaker HA is, the stronger A-. Example, HCl is a strong acid and its conjugate base, Cl- is a weak base.
B. False
2.
Electron drawing groups are molecules and/or atoms that enable the release of a proton from a specie. They cause inductive as well as mesomeric effects. Examples, -NO2, -COOH, -OH etc.
Fluoride ion is the most stable in this series because it's the most electronegative while carbon is the least stable because it's the least electronegative. Because of this, we were able to say that H-F was the most acidic, because it had the most stable conjugate base.
A. True.
3.
pKa1 = -log[Ka1]
= -log[1.2 x 10-4]
= 3.92
pKa2 = -log[Ka2]
= -log[1.5 x 10-8]
= 7.82
Using Bronsted-Lowry definition, the smaller the pKa value the more ease the acid loses its proton, that is, the smaller the pKa value, the stronger the acid.
Therefore, pKa2 > pKa1, so Ka value of 1.2 x 10-4 is a stronger acid than Ka value of 1.5 x 10-8
B. False.
1. B. False
2. A. True
3. B. False
1.
Bronsted Lowry Concept:
According to Bronsted Lowry, an acid is a proton (H⁺) donor, and a base is a proton acceptor.
The given reaction,
[tex]HA(aq) + H_2O (l)[/tex] ⇌ [tex]H_3O^+ (aq) + A^-[/tex]
The stronger HA is, the weaker the A- and vice versa; the weaker HA is, the stronger A-.
Example, HCl is a strong acid and its conjugate base, Cl- is a weak base.
- Thus the given statement is False.
2.
Electron drawing groups are molecules and/or atoms that enable the release of a proton from a species. Examples, -NO₂, -COOH, -OH etc.
Fluoride ion is the most stable in this series because it's the most electronegative while carbon is the least stable because it's the least electronegative. Because of this, we were able to say that H-F was the most acidic, because it had the most stable conjugate base.
- Thus the given statement is True.
3.
[tex]p_{Ka_1} = -log[Ka_1]\\\\p_{Ka_1}= -log[1.2 * 10^{-4}]\\\\p_{Ka_1}= 3.92[/tex]
[tex]p_{Ka_2} = -log[Ka_2]\\\\p_{Ka_2}= -log[1.5 * 10^{-8}]\\\\p_{Ka_2}= 7.82[/tex]
Using Bronsted-Lowry definition, the smaller the pKa value the more ease the acid loses its proton, that is, the smaller the pKa value, the stronger the acid.
Therefore, [tex]p_{Ka_2} > p_{Ka_1}[/tex], so Ka value of[tex]1.2 * 10^{-4}[/tex] is a stronger acid than Ka value of [tex]1.5 * 10^{-8}[/tex]
- Thus the given statement is False.
Find more information about "Acid and Base" here:
brainly.com/question/12916250
