Acids and Bases Flashcards
Acidic Solution
Contains more hydrogen ions than hydroxide ions.
Basic Solution
Contains more hydroxide ions than hydrogen ions.
Arrhenius model
A model of acids and bases; states that an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution and a base is a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution.
Bronsted-Lowry model
A model of acids and bases in which an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor.
Conjugated acid
The species produced when a base accepts a hydrogen ion from an acid
Conjugated base
The species produced when an acid donates a hydrogen ion to a base
Conjugated acid-base pair
Consists of two substances related to each other by the donating and accepting of a single hydrogen ion.
Amphoteric
Describes water and other substances that can act as both acids and bases.
Lewis model
A Lewis acid is an electron-pair acceptor and a Lewis base is an electron-pair donor.
Electrolyte
An ionic compound whose aqueous solution conducts an electric current.
Strong acid
an acid that ionizes completely in aqueous solution.
Weak acid
An acid that ionizes only partially in dilute aqueous solution
Acid ionization constant
The value of the equilibrium constant expression for the ionization of a weak acid.
Strong base
A base that dissociates entirely into metal ions and hydroxide ions in aqueous solution
Weak base
A base that ionizes only partially in dilute aqueous solution to form the conjugate acid of the base and hydroxide ion
Base ionization constant
The value of the equilibrium constant expression for the ionization of a base.
Le Chatelier’s principle
States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.
pH
The negative logarithm of the hydrogen ion concentration of a solution ; acidic solutions have a pH values between 0-7, basic solutions have values between 7-14, and a solution with a pH of 7.0 is neutral.
pOH
The negative logarithm of the hydroxide ion concentration of a solution; a solution with a pOH below 7.0 is basic and a solution with a pOH of 7.0 is neutral
Ion product constant for water
The value of the equilibrium constant expression for the self-ionization of water.
Neutralization reaction
A reaction in which an acid and a base react in aqueous solution to produce a salt and water.
Salt
An ionic compound made up of a cation from a base and an anion from an acid
Titration
The process in which an acid-base neutralization reaction is used to determine the concentration of a solution of unknown concentration
Titrant
A solution of known concentration used to titrate a solution of unknown concentration; also called the standard solution.
Equivalance point
The point at which the moles of H+ ions from the acid equals moles of OH- ions from the base.
Acid-base indicator
A chemical dye whose color is affected by acidic and basic solutions.
End point
The point at which the indicator that is used in a titration changes color.
Salt hydrolysis
The process in which anions of the dissociated salt accept hydrogen ions from water, or the cations of the dissociated salt donate hydrogen ions to water.
Buffer
A solution that resists changes in pH when limited amounts of acid or base are added
Buffer capacity
The amount of acid or base a buffer solution can absorb without a significant change in pH.
Who introduced the Arrhenius model
The one to introduce this model was Svante Arrhenius, in 1883 he proposed this model of acids and bases.
Who made The Bronsted-Lowry model
Danish chemist Johannes Bronsted and English chemist Thomas Lowry proposed a more inclusive model of acids and bases - a model that focuses on the hydrogen ion (H+)
What is the pH scale?
The pH scale is the negative logarithm of the hydrogen ion concentration of a solution ; acidic solutions have a pH values between 0-7, basic solutions have values between 7-14, and a solution with a pH of 7.0 is neutral.
What is the formula for pH
pH = -log[H+]
What is the formula for pOH
pOH = -log[OH-]
How are pH and pOH related
pH + pOH = 14.00
If they give you pH, how do you calculate the concentration?
[H+] = 10^-pH
What is the formula for Ion product constant of water
Kw = [H+] [OH-]
