Conjugate Acids and Bases
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A series of free High School Chemistry Video Lessons and solutions.
Bronsted-Lowry
Bronsted-Lowry definitions of acids and bases are useful in non-aqueous solutions. An acid is defined as a substance that can donate an hydrogen ion while a base can accept a hydrogen ion. Water is an example of an amphiprotic substance which can act either as an acid or a base.
Bronsted Lowry Theory of Acids and Bases
Understanding the bronsted-lowery model of acids and bases.
Conjugate Acids and Bases
Conjugate acids and bases are acids and bases that differ only in the presence or absence of a hydrogen ion. In acid base equilibrium both the forward and backward reaction involve proton transfer. After donating a hydrogen ion, the acid in the forward reaction becomes the base in the reverse reaction. A strong acid or base has a weak conjugate and visa versa.
Introduction to conjugate acids and bases
Understanding acid-base conjugate pairs.
Equilibrium Systems
Conjugate acid and base equilibrium systems are a type of chemical equilibrium in which the rate of the forward and reverse acid-base reaction are equal. In acid/base reactions, the position of equilibrium favors the transfer of the hydrogen ion to the stronger base. The equilibrium constant for this type of equilibrium system is denoted Kc.
Kc = [products] /[reactants]
If Kc > 1 then the products are favored.
If Kc < 1 then the reactants are favored.
Understanding equilibrium systems.
Naming Acids
When naming acids, there are several guidelines that must be followed. The rule for naming acids depends on whether the anion contains oxygen. If the anion does not contain oxygen, acid is named with prefix hydro- and suffix -ic to the root of element. If the anion does contain oxygen, the name is formed from root name of central element of anion or anion name, with a suffix of -ic or -ous. When anion name ends in -ate, the suffix -ic is used.
How to assign names to acids.
Naming acids, oxyacids, ternary, acids, binay
More Lessons for Grade 6
Math Worksheets
A series of free High School Chemistry Video Lessons and solutions.
In this lesson, we will learn
- Bronsted Lowry Theory of Acids and Bases
- Conjugate Acids and Bases
- Equilibrium Systems
- Naming Acids
Bronsted-Lowry
Bronsted-Lowry definitions of acids and bases are useful in non-aqueous solutions. An acid is defined as a substance that can donate an hydrogen ion while a base can accept a hydrogen ion. Water is an example of an amphiprotic substance which can act either as an acid or a base.
Bronsted Lowry Theory of Acids and Bases
Conjugate acids and bases are acids and bases that differ only in the presence or absence of a hydrogen ion. In acid base equilibrium both the forward and backward reaction involve proton transfer. After donating a hydrogen ion, the acid in the forward reaction becomes the base in the reverse reaction. A strong acid or base has a weak conjugate and visa versa.
Introduction to conjugate acids and bases
Equilibrium Systems
Conjugate acid and base equilibrium systems are a type of chemical equilibrium in which the rate of the forward and reverse acid-base reaction are equal. In acid/base reactions, the position of equilibrium favors the transfer of the hydrogen ion to the stronger base. The equilibrium constant for this type of equilibrium system is denoted Kc.
Kc = [products] /[reactants]
If Kc > 1 then the products are favored.
If Kc < 1 then the reactants are favored.
Understanding equilibrium systems.
When naming acids, there are several guidelines that must be followed. The rule for naming acids depends on whether the anion contains oxygen. If the anion does not contain oxygen, acid is named with prefix hydro- and suffix -ic to the root of element. If the anion does contain oxygen, the name is formed from root name of central element of anion or anion name, with a suffix of -ic or -ous. When anion name ends in -ate, the suffix -ic is used.
How to assign names to acids.
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