(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.
If weak acids ionize only a few percent in aqueous solution, why is it possible to fully neutralize a weak acid by reacting it with the stoichiometric equivalent of sodium hydroxide solution, NaOH(aq)?
Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be made to determine the molar concentrations of the base?
The pH of an aqueous solution of 0.137 M sodium hypochlorite, NaClO (aq), is ________________
This solution is: ________ (ACIDIC, BASIC, OR NEUTRAL?)
Chapter 16 Solutions
General Chemistry: Principles and Modern Applications - With Solutions Manual and Modified MasteringChemistry Code
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