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pH

Definition

The pH of a solution is the negative logarithm of the hydrogen ion (H+) concentration (in moles per liter = molarity). Chemists write "hydrogen ion concentration" as [H+]. pH tells you whether a solution is acidic, basic or neutral. The corresponding ranges are: Acidic - the pH is between zero and 7.0 Neutral - the pH is 7.0 Basic (also called alkaline) - the pH is between 7.0 and 14. For strong acids or bases, these values may actually be higher than 14 or lower than 0, but the 0-14 range is most commonly encountered.

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Additional Info

The pH scale is logarithmic. That means each change of one in pH value is 10 times more or less acidic. Therefore, a substance with a pH of 2 is 1,000 times more acidic than one with a pH of 5!

The pH values of some common substances are given in the table below.

Substance	Typical pH	[H+], M
Stomach acid (gastric juices)	1.4	0.0398
Lemon juice	2.4	0.00398
Vinegar	3.0	1 x 10-3
Tomatoes	4.2	6.31 x 10-5
Water exposed to air	5.5	3.16 x 10-6
Pure water	7.0	1 x 10-7
Blood or tears	7.4	3.98 x 10-8
Baking soda	8.4	3.98 x 10-9
Household ammonia	11.5	3.16 x 10-12
Household bleach	12.5	6.31 x 10-13

pH can be measured in many different ways. A simple example is litmus paper which can tell you if a solution is basic or acidic. Other fast and inexpensive indicator papers and reagents can also be used. Examples include phenolphthalein, bromophenol blue, methyl red and gentian violet (see Further Reading below for more). Electronic pH meters can provide very accurate pH determinations over a wide range of hydrogen ion concentrations, but cost more than simple indicators.

Finally, note that the concept of pH is technically/generally correct only for dilute solutions (say, 0.001 M and below). As the concentration of a dissolved substance, in this case, H⁺ becomes greater, chemists use a concept called activity instead. This is because ions have charge, and when there are enough ions in the solution, they begin to interact in ways that may affect their availability to interact with other species. But for the purposes that most of need on an MSDS, pH works just fine.

SDS Relevance

MSDS's include pH because it is important to know the pH of substances that may be corrosive or could react with incompatible materials. For example acids and bases should not be stored or used near each other as their accidental combination could generate a huge amount of heat and energy, possibly resulting in an explosion.

pH is also important to know in case you spill the material on your skin or eyes. Whenever a substance enters the eye, flush with water for 15 minutes and get prompt medical attention. If a basic substance enters the eye this is particularly important as basic materials tend to cause worse eye damage and are harder to flush out of the eye tissues than acidic materials.

Further Reading

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University of Akron has slides concerning acid-base chemistry and pH. pH Simplified by Robert J. Joyce. Acids and Bases at ChemTutor.com. Acid-Base Chemistry at Shodor.org. Acids, Bases, Salts at Scribd. Acids, Bases and Salt - Background and Naming at Teachers.Net. How sensors work - pH measurement at sensorland.com. pH Measurement FAQs at Cole-Parmer, a supplier of pH measurement tools. The Molecular Basis of Indicator Color Changes at General Chemistry Online! Also see Acids and bases: Frequently asked questions which includes indicators. Acid-Base Indicators at Chemguide. Chembuddy discusses activity vs. pH. More on pH vs activity at Stetson University. See also: acid, base, eye wash.

Additional definitions from Google and OneLook.

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