Electrolytes
An electrolyte will dissolve in water to form a solution that will conduct an electric current. the ability of the solution to conduct an electric current is due to the presence of ions that are free to move. therefore, all ionic compounds are electrolytes. Also, some polar covalent compounds form ions and conduct electricity when dissolved in water. for example HCI and HBr. However nonelectrolytes, such as organic solvents,do not conduct electricity.
weak electrolytes in aqueous solution attain an equilibrium constant for such systems is called the dissociation constant . The value of dissociation constant changes with a change of temperature.
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Arrhenius Theory of Acids-Bases .
CONCEPTUAL DEFINITIONS OF ACIDS
Arrhenius' theory. An acid is a substance that yields hydrogen ions in aqueous solutions. This conceptual definitions is adequate when considering reactions in aqueous solutions. As knowledge of the mechanism of chemical reactions has increased, more inclusive definitions have been advanced. The characteristic properties of acids in aqueous solution are due to an excess of hydrogen ions.
Identify Conjugate Acid Base Pairs (Bronsted Lowry)
.Bronsted-Lowry Theory- An Acid is any species (molecule or Ion0 that can donate a proton to another species. The Bronsted-Lowry does not replace the Arrhenius Theory, but extends it. The Bronsted-Lowry Theory definition of an acid includes all substances that are acids according to the Arrhenius definition.
In addition some molecules and ions are classified as acids under the Bronsted-Lowry definition that are not acids in the Arrhenius sense for example in the reaction >>>Formula p.120<<<
The water molecule donates a proton to the ammonia and is considered an acid in the Bronsted-Lowry sense. In the reverse reaction, the ammonium ion will donate a proton and act as the acid, while the hydroxide ion accepts the proton and acts as a base.
Bronsted-Lowry - Acid & Base Theory, conjugates explained .
a base is any species [molecule or iron] that can accept a proton. the brostead -lowery definition extends in the Arrhenius defintiion to include many species in addition to the oh that can accept a proton.
pH, Indicators and Acid Base Reactions .
bases may be defined in terms of their characteristics properties
poerational definition of bases:
1. aqueous solutions of bases conduct electricity.some examples of the relative degree of ionization are shown in the re3ferance tables for chemistry.
2.bases cause color changes in acid-base indicators. they cause red litmus to turn blue and phenophthalien[a weak, colorless acid] to turn pink.
3. bases react with acids to form water and a salt.
4. aqueous solutions of bases feel slippery.
5.strong bases have a caustic action on the skin.
Doctor Campbell's Science Demo - pH Indicators
Hydronium Ion Formation Tutorial.
Lewis Dot Structure of H3O+, (Hydronium Ion) .
What is pH?
What is pH .2
Calculating pH for acid-base titrations (1) .
How To: Acid-Base Titration
Strength of Acids and Bases .
Acid and Base Strength .
