(a) Interpretation: To explain whether CH 3 COO − acts as an acid, base or amphiprotic in pure acetic acid. Concept introduction: As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
(a) Interpretation: To explain whether CH 3 COO − acts as an acid, base or amphiprotic in pure acetic acid. Concept introduction: As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
Solution Summary: The author explains that acetic acid is acid because it can donate its hydrogen.
To explain whether CH3COO− acts as an acid, base or amphiprotic in pure acetic acid.
Concept introduction:
As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
Interpretation Introduction
(b)
Interpretation:
To explain whether H2O act as an acid, base or amphiprotic in pure acetic acid.
Concept introduction:
As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
Interpretation Introduction
(c)
Interpretation:
To explain whether CH3COOH act as an acid, base or amphiprotic in pure acetic acid.
Concept introduction:
As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
Interpretation Introduction
(d)
Interpretation:
To explain whether HClO4 act as an acid, base or amphiprotic in pure acetic acid.
Concept introduction:
As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
Chemists working with fluorine and its compounds some-
times find it helpful to think in terms of acid-base reac-
tions in which the fluoride ion (F¯) is donated and
ассеpted.
(a) Would the acid in this system be the fluoride donor or
fluoride acceptor?
(b) Identify the acid and base in each of these reactions:
CIF;O2 + BF;
CIF,O, · BF,
--
TiF, + 2 KF – K2[TiF,]
A chemist is performing a titration in order to determine the amount of sodium hydroxide, NaOH(aq), in 125 mL of an aqueous
solution.
(a) If 28 mL of a 0.13 M HCl solution was used as a titrant to reach the equivalence point, what was the concentration of
sodium hydroxide in the initial solution?
M
(b) What was the initial pH of the sodium hydroxide solution?
The following two reactions involve proton transfer. In each reaction, identify the
acid and the base. Identify the conjugate base of the acid, and the conjugate acid of
the base. Draw Lewis electron dot diagrams for each molecule, and describe the rear-
rangement of bonding in the reaction as nonbonding electron pairs become cova-
lently shared pairs and vice versa.
(a) H¿O(€) + NH (aq) → H;0* (aq) + NH3(aq)
(b) CH;CH;OH(aq) + NH7 (aq) → CH;CH;O¯(aq) + NH3(aq)
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