PH | Wikipedia audio article
Channel: wikipedia tts
Date: 2018-12-25

This is an audio version of the Wikipedia Article:
https://en.wikipedia.org/wiki/PH


00:01:34 1 History
00:04:31 2 Definition and measurement
00:04:40 2.1 pH
00:05:43 2.2 p[H]
00:11:06 2.3 pH indicators
00:13:35 2.4 pOH
00:13:46 2.5 Extremes of pH
00:14:39 2.6 Non-aqueous solutions
00:15:56 2.7 Unified absolute pH scale
00:17:06 3 Applications
00:18:54 3.1 pH in soil
00:19:32 3.1.1 Classification of soil pH ranges
00:20:40 3.2 pH in nature
00:20:54 3.3 Seawater
00:22:03 3.4 Living systems
00:22:12 4 Calculations of pH
00:22:32 4.1 Strong acids and bases
00:23:17 4.2 Weak acids and bases
00:25:23 4.3 General method
00:26:43 5 See also
00:27:01 6 References
00:27:50 7 External links
00:28:48 Calculations of pH
00:30:27 Strong acids and bases
00:31:10 2. Sodium hydroxide, NaOH, is an example of a strong base. The p[OH] value of a 0.01M solution of NaOH is equal to −log10(0.01), that is, p[OH]
00:32:20 Weak acids and bases
00:34:30 CH
00:38:29 General method
00:42:19 See also



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SUMMARY
=======
In chemistry, pH () is a logarithmic scale used to specify the acidity or basicity of an aqueous solution.  It is approximately the negative of the base 10 logarithm of the molar concentration, measured in units of moles per liter, of hydrogen ions. More precisely it is the negative of the base 10 logarithm of the activity of the hydrogen ion. At 25 °C, solutions with a pH less than 7 are acidic and solutions with a pH greater than 7 are basic. The neutral value of the pH depends on the temperature, being lower than 7 if the temperature increases. Pure water is neutral, pH 7 at (25 °C), being neither an acid nor a base. Contrary to popular belief, the pH value can be less than 0 or greater than 14 for very strong acids and bases respectively.Measurements of pH are important in agronomy, medicine, chemistry, water treatment, and many other applications.
The pH scale is traceable to a set of standard solutions whose pH is established by international agreement.
Primary pH standard values are determined using a concentration cell with transference, by measuring the potential difference between a hydrogen electrode and a standard electrode such as the silver chloride electrode.
The pH of aqueous solutions can be measured with a glass electrode and a pH meter, or an indicator.
There are three current theories used to describe acid–base reactions: Arrhenius, Bronsted-Lowry and Lewis when determining pH.