Properties of acids and bases
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Properties of Acids and Bases. Acids taste sour, will change the color of an acid base indicator, and can be strong or weak electrolytes in aqueous solution. Properties of Acids and Bases.

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Properties of Acids and Bases

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Properties of acids and bases

Properties of Acids and Bases

Acids taste sour, will change the color of an acid base indicator, and can be strong or weak electrolytes in aqueous solution.


Properties of acids and bases1

Properties of Acids and Bases

Bases taste bitter, feel slippery, will change the color of an acid-base indicator, and can be strong or weak electrolytes in aqueous solution.


Arrhenius acids and bases

Arrhenius Acids and Bases

Arrhenius acids are compounds that ionize to yield hydrogen ions (H+) in aqueous solution.


Arrhenius acids and bases1

Arrhenius Acids and Bases

An Arrhenius base is a compound that ionizes to yield hydroxide ions (OH-) in aqueous solution.


Bronsted lowry acids and bases

Bronsted-Lowry Acids and Bases

The Bronsted-Lowry theory defines an acid as a hydrogen-ion donor and a base as a hydrogen-ion acceptor.


Bronsted lowry acids and bases1

Bronsted-Lowry Acids and Bases

A conjugate acid is the particle formed when a base gains a hydrogen ion.

A conjugate base is the particle formed when an acid has donated a hydrogen ion.


Bronsted lowry acids and bases2

Bronsted-Lowry Acids and Bases

A conjugate acid-base pair consists of two substances related by the loss or gain of a single hydrogen ion.


Bronsted lowry acids and bases3

Bronsted-Lowry Acids and Bases


Bronsted lowry acids and bases4

Bronsted-Lowry Acids and Bases

A water molecule that gains a hydrogen ion becomes a positively charged hydronium ion (H3O+).

A substance that can act as both an acid and a base is said to be amphoteric.


Lewis acids and bases

Lewis Acids and Bases

A Lewis acid is a substance that can accept a pair of electrons to form a covalent bond.

A Lewis base is a substance that can donate a pair of electrons to form a covalent bond.


Acids and bases

Acids and Bases


Hydrogen ions from water

Hydrogen Ions from Water


Ion product constant for water

Ion Product Constant for Water

The product of the concentrations of the hydrogen ions and hydroxide ions in water is called the ion-product constant for water (Kw).


Ion product constant for water1

Ion Product Constant for Water

If [H+] = [OH-], then the solution is neutral.

If [H+] > [OH-], then the solution is acidic.

If [H+] < [OH-], then the solution is basic.


The ph concept

The pH Concept

In a neutral solution, the [H+] = 1 x 10-7M. The pH of a neutral solution is 7.


The ph concept1

The pH Concept

If [H+] = [OH-], then the pH = 7.

If [H+] > [OH-], then the pH < 7.

If [H+] < [OH-], then the pH > 7.


The ph concept2

The pH Concept


The ph concept3

The pH Concept


The ph concept4

The pH Concept


Measuring ph

Measuring pH

An indicator is a valuable tool for measuring pH because its acid form and base form have different colors in solution.

Phenolphthalein changes from colorless to pink at pH 7-9.


Measuring ph1

Measuring pH


Strong and weak acids and bases

Strong and Weak Acids and Bases

In general, strong acids are completely ionized in aqueous solution.

Weak acids ionize only slightly in aqueous solution.


Strong and weak acids and bases1

Strong and Weak Acids and Bases

Strong bases dissociate completely into metal ions and hydroxide ions in aqueous solution.

Weak bases react with water to form the hydroxide ion and the conjugate acid of the base.


Strong and weak acids and bases2

Strong and Weak Acids and Bases


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