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Manu > Acids and Bases > Flashcards

Acids and Bases Flashcards

1
Q

Acidic Solution

A

Contains more hydrogen ions than hydroxide ions.

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2
Q

Basic Solution

A

Contains more hydroxide ions than hydrogen ions.

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3
Q

Arrhenius model

A

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.

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4
Q

Bronsted-Lowry model

A

A model of acids and bases in which an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor.

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5
Q

Conjugated acid

A

The species produced when a base accepts a hydrogen ion from an acid

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6
Q

Conjugated base

A

The species produced when an acid donates a hydrogen ion to a base

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7
Q

Conjugated acid-base pair

A

Consists of two substances related to each other by the donating and accepting of a single hydrogen ion.

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8
Q

Amphoteric

A

Describes water and other substances that can act as both acids and bases.

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9
Q

Lewis model

A

A Lewis acid is an electron-pair acceptor and a Lewis base is an electron-pair donor.

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10
Q

Electrolyte

A

An ionic compound whose aqueous solution conducts an electric current.

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11
Q

Strong acid

A

an acid that ionizes completely in aqueous solution.

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12
Q

Weak acid

A

An acid that ionizes only partially in dilute aqueous solution

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13
Q

Acid ionization constant

A

The value of the equilibrium constant expression for the ionization of a weak acid.

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14
Q

Strong base

A

A base that dissociates entirely into metal ions and hydroxide ions in aqueous solution

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15
Q

Weak base

A

A base that ionizes only partially in dilute aqueous solution to form the conjugate acid of the base and hydroxide ion

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16
Q

Base ionization constant

A

The value of the equilibrium constant expression for the ionization of a base.

17
Q

Le Chatelier’s principle

A

States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.

18
Q

pH

A

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.

19
Q

pOH

A

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

20
Q

Ion product constant for water

A

The value of the equilibrium constant expression for the self-ionization of water.

21
Q

Neutralization reaction

A

A reaction in which an acid and a base react in aqueous solution to produce a salt and water.

22
Q

Salt

A

An ionic compound made up of a cation from a base and an anion from an acid

23
Q

Titration

A

The process in which an acid-base neutralization reaction is used to determine the concentration of a solution of unknown concentration

24
Q

Titrant

A

A solution of known concentration used to titrate a solution of unknown concentration; also called the standard solution.

25
Q

Equivalance point

A

The point at which the moles of H+ ions from the acid equals moles of OH- ions from the base.

26
Q

Acid-base indicator

A

A chemical dye whose color is affected by acidic and basic solutions.

27
Q

End point

A

The point at which the indicator that is used in a titration changes color.

28
Q

Salt hydrolysis

A

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.

29
Q

Buffer

A

A solution that resists changes in pH when limited amounts of acid or base are added

30
Q

Buffer capacity

A

The amount of acid or base a buffer solution can absorb without a significant change in pH.

31
Q

Who introduced the Arrhenius model

A

The one to introduce this model was Svante Arrhenius, in 1883 he proposed this model of acids and bases.

32
Q

Who made The Bronsted-Lowry model

A

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+)

33
Q

What is the pH scale?

A

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.

34
Q

What is the formula for pH

A

pH = -log[H+]

35
Q

What is the formula for pOH

A

pOH = -log[OH-]

36
Q

How are pH and pOH related

A

pH + pOH = 14.00

37
Q

If they give you pH, how do you calculate the concentration?

A

[H+] = 10^-pH

38
Q

What is the formula for Ion product constant of water

A

Kw = [H+] [OH-]

Manu (18 decks)

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