Introduction:
In 1909 S.P.L. Sorensen published a paper in Biochem Z in which he discussed the effect of H1+ ions on the activity of enzymes. In the paper he invented the term pH to describe this effect and defined it as the -log[H1+ ]. In 1924 Sorensen realized that the pH of a solution is a function of the "activity" of the H1+ ion not the concentration and published a second paper on the subject. A better definition would be pH=-log[aH1+ ], where aH1+ denotes the activity of the H1+ ion. The activity of an ion is a function of many variables of which concentration is one. It is unfortunate that chemistry texts use a definition for pH that has been obsolete for over 50 years.
Because of the difficulty in accurately measuring
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Keyterms:
Buffer: a substance or combination of substanes capable of neutralizing limited quantities of either acid(H3O+) or base (OH-) added to it.
Dynamic Equilibrium: Two offsetting processes occur at equal rates, producing a state of balance where no net changes is observed.
Molar Consentration or Molarity: Concentration of a solution measured as the number of moles of solute per liter of solution. For example, a 6 M HCl solution contains 6 moles of HCl per liter of solution.
Hypothesis:
I predict that out of the 20 solutions that we are going to be testing, about 6 of them will be an acid, 3 will be neutral and 11 will be a base.
Data Table:
UNKNOWN Acid or
Base pH
1 Neutral 6
2 Neutral 7
3 Base 8
4 Acid 3
5 Acid 4
6 Acid 3
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