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Introductory Chemistry: A Foundati...
. Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?
Interpretation:
The approximate pH values of five “everyday solutions” should be determined. It also requires one to relate the sour taste of the acidic compounds relate to the indicated pH values.
Concept Introduction:
It is important to have a scale to compare the strength of a property. Acidity of a certain solution is a critical parameter that one must consider in comparing reaction conditions, yields and activity of the enzymes. Therefore, it is important to have an easy and understandable scale that one gets a clear idea about the acidity of a given solution. pH value is defined in order to satisfy this requirement for aqueous solutions. Essentially it is a measure of the amount of H+ ions in a solution.
In order to represent small H+ concentrations in a more convenient manner a representation called a pN scale is used. This pN scale is based on common logarithm (base 10 logarithm). In this system if N represents a number then,
pN=-log1 0 N = (-1) log1 0 N
This pN means to take the log of the number of the number that follows and multiply the result by (-1).
Let N = [H+ (aq)] then in aqueous media [H+ (aq)] = [H3 O+ (aq)]
Therefore;
Chapter 16 Solutions
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