Water as an Acid and Base
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Transcript of Water as an Acid and Base
Water as an Acid and Water as an Acid and BaseBaseChapter 15.1C
How can it be?How can it be?How can a substance be both an
acid and a base?Substances that can behave
either as an acid or as a base are called amphoteric substances.
Water is the most common amphoteric substance.
Ionization of WaterIonization of WaterLet’s look at the following equation
to understand why water is amphoteric:
H2O + H2O H3O+ + OH-
In this reaction, one water molecule acts as an acid by donating a proton, the other water molecule acts as a base by accepting the proton.
However, this reaction only happens to a small extent
Concentration of IonsConcentration of IonsIn any solution you will have a
certain concentration of H3O+ and OH- ions.
To demonstrate concentration, we place ions in brackets
Example: [H+] and [OH-]Note: to simplify we often write H3O+
as H+
The proportion of H3O+ and OH- ions determines whether your solution is acidic or basic
Ion-Product ConstantIon-Product ConstantIn a solution, [H+][OH-] = 1.0 x 10-14
This number is known as Kw, the ion-product constant for water
If your solution has more [H+] than [OH-], the solution is acidic
If your solution has more [OH-] than [H+], the solution is basic.
If [H+] and [OH-] are equal, your solution is neutral
You can use Kw and [H+] or [OH-] to solve for the other
Example 1Example 1Calculate the [H+] if [OH-]= 1.0 x 10-5
M, and identify whether this solution is acidic, basic, or neutral
[H+][OH-] = 1.0 x 10-14
[H+][1.0 x 10-5 M] = 1.0 x 10-14
Solve for [H+]:[H+] = (1.0 x 10-14)/ (1.0 x 10-5 )= 1.0
x 10-9 MSince we have more [OH-] than [H+],
the solution is basic.
Example 2Example 2Calculate [OH-] if [H+]= 10.0 M, and
identify whether this solution is acidic, basic, or neutral
[H+][OH-] = 1.0 x 10-14
[10.0 M][OH-] = 1.0 x 10-14
Solve for [OH-][OH-]= (1.0 x 10-14)/ (10.0 M) = 1.0 x
10-15 MSince we have more [H+] than [OH-]
the solution is acidic.
Book Work!Book Work!Complete the following
assignment:P 590 #22, 23