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Example Questions
Example Question #2 : Strong And Weak Acids/Bases
reacts with in aqueous solution according to the chemical equation provided. If it took of a solution to titrate of an solution, what was the concentration of original solution?
Using the concentration of as a conversion factor, we can convert the volume of to moles by dimensional analysis:
At the equivalence point of the titration:
Example Question #31 : Acid Base Reactions
Determine the acid dissociation constant expression for the given reaction.
Acid dissociation constant which is denoted as is the equilibrium constant for the ionization of an acid. Therefore, the numerator contains the product of the concentrations of the substances on the product side of the chemical equation. The denominator contains the product of the concentrations of the substances on the reactant side of the chemical equation. is omitted in the acid dissociation constant expression because as the solvent it is in excess and therefore the change in its concentration is negligible in comparison to the other substances in solution.
Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions
Identify the Bronsted-Lowry acid in the following equation:
Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that becomes , which it lost an , or a proton. Thus, water must be the Bronsted-Lowry acid.
Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions
Identify the Lewis Base in the following reaction:
Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that becomes . Since accepted a proton, it must be the Lewis base.
Example Question #3 : Lewis, Brønsted Lowry, And Arrhenius Definitions
Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?
Bronsted-Lowry acid
None of these
Lewis acid
Arrhenius acid
Arrhenius acid
There are three main definitions for acids and bases: the Lewis acids and bases, Bronsted-Lowry acids and bases, and Arrhenius acids and bases.
A Lewis acid is a species which can accept an electron pair from a donor. An example of a Lewis acid is ; as a cation, it can accept an electron pair. A Lewis base is a species which can donate an electron pair. An example of a Lewis base is ; as an anion, it can donate an electron pair.
A Bronsted-Lowry acid is a species which can donate a proton. An example of a Bronsted-Lowry acid is , which can donate its hydrogen ion. A Bronsted-Lowry base is a species which can accept a proton from a donor. An example of a Bronsted-Lowry base is , which can accept a hydrogen ion in order to become water.
An Arrhenius acid is a species which releases hydrogen ions into solution. An example of an Arrhenius acid is . When this compound dissolves in aqueous solution, it produces and . An Arrhenius base is a species which releases hydroxide ions into solution. An example of an Arrhenius base is . When this compound dissolves in aqueous solution, it produces and .
Example Question #34 : Acid Base Reactions
What is the pH of a solution?
PH is defined as , where is hydronium concentration). In order to do this we simply take :
=
Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions
According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?
There are no acids in the reaction
Remember a Brønsted-Lowry acid is defined as a proton donor.
In the forward reaction, is a proton donor. In the backward reaction, is the proton donor.
The acids in this reaction are and .