FINALS Flashcards by AZIZA DOROTHY DORADO

ACID PROPERTIES:
When dissolved in water, acids

Conduct electricity
Change blue litmus to red
Have a sour taste
React with bases to neutralize their properties
React with active metals to liberate hydrogen

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BASE PROPERTIES:
When dissolved in water, bases

Conduct electricitv
Change red litmus to blue
Have a slippery feeling
React with acids to neutralize their properties

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classification of substances in terms of their behavior in water.

acid-base

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is a substance with H in its formula that
dissociates to yield H3O

acid

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is a substance with OH in its formula that dissociates to yield OH-

base

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When an acid reacts with a base, they undergo

neutralization

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is a substance that dissociates in aqueous medium to form yield hydronium ions, H3O+

arrhenius acid

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dissociates completely into ions in water

strong acid

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A _____ solution of a strong acid contains no HA molecules

dilute

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A ______ acid dissociates slightly to form ions in water

weak

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In a dilute solution of a weak acid, most HA molecules are _________.

undissociated

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T or F | THE EXTENT OF DISSOCIATION FOR STRONG ACIDS
• There are no HA molecules in solution

The HA will turn into hydronium ion and an anion

True

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Gaseous form of HCI -> called as

hydrogen chloride gas

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When hydrogen chloride is aqueous or added to water, it becomes

Hydrochloric acid

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THE EXTENT OF DISSOCIATION FOR WEAK ACIDS: Most HA molecules are _________.

undissociated

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Weak acid: Majority will not be converted into individual ions, rather, around __ to ___% will not be converted

98-99%

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Weak acid: Small part will be converted into ________ ion and anion when weak acid dissociates in water

hydronium ion

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Stronger acids have more

H3O

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Liberates hydrogen from hydrochloric acid ( strong or weak acid?). There’s a violent formation of bubbles

strong acid

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If _______, then the acid is strong

Ka > 1

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If ______, then the acid is weak

Ka < 1

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If ______, then the base is strong

Kb > 1

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If ______, then the base is strong

Kb > 1

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If _____,thenthebaseisweak.

Kb<1

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HCl

Strong acid

HBr

Strong acid

HNO3

Strong acid

H2SO4

Strong acid

HClO4

Strong acid

Weak acid

HCN

Weak acid

HClO

Weak acid

HNO2

Weak acid

RCOOH

Weak acid

Carboxylic acids

Weak acid

CH3OOH

Weak acid

C6H5OOH

Weak acid

oxoacids in which the number of O atoms exceeds the number of ionizable protons by two or more

Strong acids

acids in which H is not bonded to O or to a halogen

Weak acids

oxoacids in which the number of O atoms equals or exceeds the number of ionizable protons by one

Weak acids

water-soluble compounds containing O2- or OH- ions

Strong bases

M2O or MOH (M = Group 1A(1) metal (Li, Na, K, Rb, Cs)

strong base

MO or M(OH)2 (M = group 2A(2) metal (Ca, Sr, Ba)

strong base

ammonia (NH3)

Weak base

amines

Weak base

RNH2

Weak base

R2NH

Weak base

R3N

Weak base

AUTOIONIZATION OF WATER Also called "___________"

self ionization of water or auto-dissociation of water

an ionization reaction in pure water or in an aqueous solution, in which a water molecule, H2O, deprotonates loses the nucleus of one of its hydrogen atoms) to become a hydroxide ion, OH-

AUTOIONIZATION OF WATER

The water molecule can act as a ____ or ____ Forming the conjugate acids and base

base or an acid

WATER IS

AMPHOTERIC

"__________" means the ability of a substance to react either as an acid or as a base.

Amphoteric

Water dissociates very slightlyaqinto ions oinaqan equilibrium process known as autoionization or

self-ionization

Kw= [H3O+][OH-] =

1.0x10^-14 (at 25° C)

[H3O+] = [OH-] =

1.0x10^-7 (at 25°C)

A change in ____ causes an inverse change in [OH-], and vice versa.

[H3O+]

In an acidic solution

[H3O+] > [OH-]

In a neutral solution

[H3O+] = [OH-]

In basic solution

[H3O+]<[OH-]

pH: In an acidic solution

pH < 7.00

pH: In a neutral solution

pH = 7.00

pH: In basic solution

pH > 7.00

The higher the pH, the lower the [H3O+] and the _____ acidic the solution.

less

____ and ____ scales express the acidity and basicity of dilute aqueous solutions

pH and pOH

It is known as the power of hydrogen or the measure of hydrogen ions H+ or hydronium ions [H3O+] concentrations

It is the measure of hydroxide ion [OH-] concentration

pOH

pKw =

-log Kw

pKw =-log Kw

(= 14.0 at 25°C)

T or F| If [H3O] increases, [OH] decreases (and vice versa)

True

T or F| If pH increases, pOH decreases (and vice versa)

True

• These expressions are analogous to the expression for pH.

pKa and pKb

We derived it to express the concentration in a more convenient way using whole numbers

pKa and pKb

pKa =

-log Ka

pKb =

-log Kb

The ______ the value of pKa the stronger the acid

smaller

The ______ the value of pKb, the stronger the base.

smaller

An acid is a proton donor, any species that donates an H+ ion. • An acid must contain H in its formula.

Brønsted-Lowry Acid-Base

A base is a proton acceptor, any species that accepts an H+ ion. • A base must contain a lone pair of electrons to bond to H+.

Brønsted-Lowry Acid-Base

An acid-base reaction is a proton-transfer process.

Brønsted-Lowry Acid-Base

__________acid is a substance that is a proton donor.

Brønsted-Lowry

_______base is a substance that is a proton acceptor.

Brønsted-Lowry

A _________________ reaction occurs when an acid and a base react to form their conjugate base and conjugate acid, respectively.

Brønsted-Lowry acid-base

The ___ direction of an acid-base reaction depends on the relative strength of the acids and bases involved.

net

A reaction will favor the formation of the ______ acid and base.

weaker

The stronger the acid is, the _____ its conjugate base.

weaker

- is called the acid-dissociation constant or the equilibrium constant for the dissociation of weak acid.

– is a measure of acid strength.

Percent Ionization

Percent Ionization formula =

concentration of ionized HA/original concentration of HA x 100%

is any species that donates an electron pair to form a bond.

Lewis base

is any species that accepts an electron pair to form a bond.

Lewis acid

donation and acceptance of an electron pair to form a covalent bond.

Lewis acid-base

Lewis acid is a substance that is an electron pair _______.

acceptor

Lewis base is an electron pair ____.

donor

Molecules that contain a polar multiple bond often function as

Lewis acids

A ______cation acts as a Lewis acid when it dissolves in water to form a hydrated ion

metal

FINALS Flashcards

(97 cards)