Acid/ Base & Conjugate Acid & Conjugate Base

Conjugate base is....

The particle that remains when an acid has donated a hydrogen ion.

Conjugate acid is....

The particle formed when a base gains a hydrogen ion.

Base

A compound that produces hydroxide ions in solution.

Acid

A compound that loses hydrogen ions (H+) in solution.

Acids whose names end in "ide"

add prefix -hydro

change "ide" to "ic acid."

Acids whose names end in "ate"

change ending to "ic acid."

Acids whose names end in "ite"

change ending to "ous acid."

True or False: An acid is a substance that produces H+ ions in water.

True

Which of the following must be present in a Bronsted-Lowry acid?

A hydrogen atom.

A chlorine atom.

A nonbinding electron pair.

An OH group.

A hydrogen atom

While a carboxylic acid may contain many hydrogen atoms, the acidic hydrogen atom in any carboxylic acid is attached to a(n) _______ atom in the COOH group.

oxygen

The iodate anion has the formula IO3-. The name of the acid with the formula HIO3 is ______.

iodic acid

Which of the following must be present in a Bronsted-Lowry base?

An oxygen atom.

A hydrogen atom.

A negative charge.

A lone pair of electrons.

A lone pairs electrons.

A Bronsted-Lowry base is a _____.

proton acceptor

Which of the following compounds are Arrhenius bases?

CH3COOH

Ca (OH)2

KOH

NaBr

HNO3

Ca(OH)2

KOH

True or False: An acid contains a hydrogen atom and dissolves in water to form a hydrogen ion, H+.

True

True or False: A base contains hydroxide and dissolves in water to from OH-.

True

A Bronsted-Lowry acid must contain at least one ______ atom.

hydrogen

In aqueous solution, a Bronsted-Lowry acid donates an H+ ion to water to form a(n) ______ ion.

hydronium or H3O+

Which functional group is contained in all carboxylic acids?

OH-

COOH

HCl

CH

COOH

The product formed by loss of a proton from an acid is called its ______.

conjugate base

The product formed by gain of a proton by a base is called its ______.

conjugate acid

A Bronsted-Lowry acid-base reaction involves the transfer of a(n) _____ from the ______ to the _____.

proton

acid

base

Chloride changes to

Chlorous acid

Hydrochloric acid

Chloric acid

Hydrochloric acid

Chlorite changes to

Chlorous acid

Hydrochloric acid

Chloric acid

Chlorous acid

Chlorate changes to

Chlorous acid

Hydrochloric acid

Chloric acid

Chloric acid

A Bronsted-Lowry base is a proton ____, and therefore must contain a ______ pair of electerons.

acceptor

lone

Which of the following is the correct Arrhenius definition of an acid?

An acid is a proton donator.

An acid is a substance that produces hydroxide ions in water.

An acid is a substance that produces H+ ions in water.

An acid is a substance that is sour to the taste.

An acid is a substance that produces H+ ions in water.

Which of the following is a characteristic of all Bronsted-Lowry acid-base reactions?

A change in oxidation states.

The presence of a hydroxide ion.

The transfer of a proton.

The transfer of a proton.

When a Bronsted-Lowry base gains a proton, the species formed is called its _______ acid.

conjugate

What makes a compound an Arrhenius Base?

The subtance must dissolve in water to form hydroxide (OH-) ions.

When a Bronsted-Lowry acid loses a proton, its charge _____ by 1. When a Bronsted-Lowry base gains a proton, its charge ______ by 1.

decreases

increases

An amphoteric species is a molecule or ion that reacts as a(n)...

acid or base.

The following are examples of....

An ionic compound is dissolved in water.

An acid reacts with water to form its conjugate base plus a hydronium ion.

Dissociation

Which statement about weak acids is correct?

Weak acids are not able to donate a proton.

Weak acids are strong bases.

Weak acids only partially dissociate in aqueous solution.

Weak acids are not soluble in water.

Weak acids only partially dissociate in aqueous solution.

Which of the following are common strong Bronsted-Lowry acids?

H2SO4

H3PO4

HCN

HCl

HNO3

HCl

H2SO4

HNO3

Select all of the statements that correctly describe an amphoteric molecule or ion.

It can act as either a base or an acid.

It contains at least one hydrogen atom.

It can undergo either an acid-base reaction or an oxidation-reduction reaction.

It contains at least one chlorine atom.

It contains at least one lone pair of electrons.

It can act as either a base or an acid.

It contains at least one hydrogen atom.

It contains at least one lone pair of electrons.

Hydrofluoric acid (HF) is a stronger acid than hydrocyanic acid (HCN). Which statement about their conjugate bases is correct?

Since cyanide (CN-) and fluoride are both weak bases, they have the same strength.

It is not possible to determine the relative strengths of bases from their conjugate acids.

Cyanide (CN-) is a weaker base than fluoride.

Cyanide (CN-) is a stronger base than fluoride.

Cyanide (CN-) is a stronger base than fluoride.

True or False: The stronger the acid, the weaker the conjugate base.

True

True or False: The stronger the base, the weaker the conjugate acid.

True

A strong acid is an acid that completely ____ in aqueous solution.

dissociates or ionizes

Which of the molecules shown below is a strong Bronsted-Lowey acid?

HBr

HBrO

HBrO3

HBrO2

HBr

Strong acid + strong base means that side of the equilibrium is....

not favored.

favored.

not favored.

In a Bronsted-Lowry acid-base equilibrium, the ______ acid and base will react to form the ______ acid and base.

stronger

weaker

In any aqueous solution, the product of the hydronium and hydroxide concentrations will always be equal to ______ at 25 degrees celcius. This value is known as ______.

10^-14, Kw

True or False: Products are always in the numerator of an equilibrium constant expression.

True

In an aqueous solution of a strong acid, [H3O+] is ______ the acid concentration.

hint* a strong acid dissociates completely in water.

greater than

less than

equal to

equal to

Which of the following equations is the correct expression for Kw?

Kw = [H3O+][OH-]/[H2O]2

Kw = [H3O+]-1[OH-]-1

Kw = [H3O+][OH-]

Kw = [H3O+][OH-]/[H2O]

Kw = [H3O+][OH-]

Which of the following is the correct acid dissociation constant expression for HF?

Ka = [HF]/ [H3O+][F-]

Ka = [H3O+][F-]/[HF]]

Ka = [F-][H3O+]/ [HF][H2O]

Ka = [H3O+][F-] /[HF]

The _____ scale is a logarithmic scale of hydronium ion concentration; it is used to characterize the____ or basicity of an aqueous solution

pH

acidity

For a strong acid, what is the relationship between the hydronium ion concentration and the acid concentration in aqueous solution?

The hydronium ion concentration is equal to the acid concentration.

The hydronium ion concentration is equal to Kw divided by the acid concentration.

The hydronium ion concentration is greater than the acid concentration.

The hydronium ion concentration is equal to Ka.

The hydronium ion concentration is equal to the acid concentration.

Which of the following is the correct definition of pH?

log[OH-]

-log[Ka]

-log[H3O+]

log[H3O+]

-log[H3O+]

In a solution that is basic, the pH will be ______ than 7, and the hydronium ion concentration will be _____ than 10-7 M.

greater

less

What is the hydroxide ion concentration in a 0.010 M solution of NaOH?

1.0 x 1012 M

0.010 M

0.10 M

1.0 x 10-7 M

0.010 M

The pH of a substance is a measure of its

hydronium ion concentration, therefore numbers = the same

Important pH levels

Saliva=

Stomach fluid=

Blood=

Urine=

5.8 - 7.1

1.6 - 1.8

7.4

4.6 - 8.0

The reaction of a Bronsted-Lowry acid with a hydroxide base is called a ____ reaction. The products of the reaction are ____ and a(n) ______.

neutralization

salt

water

What is a net ionic equation?

A balanced equation that contains only the species involved in the reaction.

The complete balanced reaction between two compounds in aqueous solution.

An unbalanced equation that indicates the net product of a reaction.

A balanced equation that contains only the species involved in the reaction.

A chemical equation that contains only the species involved in the reaction is called a(n) ______.

acid-base reaction

net ionic equation

neutralization reaction

spectator ion

net ionic equation

What are spectator ions?

Ions that can act both as Bronsted-Lowry acids and bases

Ions that a appear on both sides of a balanced equation but do not undergo any change

Hydronium and hydroxide ions that occur as a result of the dissociation of water

Ions that precipitate out of a Bronsted-Lowry acid-base reaction

Ions that a appear on both sides of a balanced equation but do not undergo any change

Ions that appear on both sides of a balanced equation but do not participate in the reaction are called ____ ions.

spectator

When an acid reacts with either the carbonate (CO32-) or bicarbonate (HCO3-) ion, the immediate product is _____ acid. This product is unstable however, decomposing to ____ and carbon dioxide.

carbonic

water

A neutralization reaction in which the concentration of an acid (or base) is determined by reacting it with a base (or acid) of known concentration is called a(n) _____.

titration

Which of the following are products of the reaction of an acid with sodium bicarbonate (NaHCO3)?

hydrogen

carbon dioxide

hydroxide

water

ionic salt

carbon dioxide

water

ionic salt

A student has a solution of unknown concentration of the strong acid HCl. Which of the following would be necessary in order to perform a titration to determine the concentration of the solution?

A distillation apparatus

An acid solution of known concentration

A base solution of known concentration

An acid-base indicator

A calibrated buret

A base solution of known concentration

An acid-base indicator

A calibrated buret

Order the steps for writing a balanced equation for the neutralization reaction of a Bronsted-Lowry acid with a hydroxide base.

identify the acid and base on the reactants side, and draw H2O as a product

determine the structure of the salt that that is formed as a product

balance the equation

Which of the following statements correctly describe a buffer solution? Select all that apply.

Multiple select question.

Its pH changes only slightly when either strong acid or strong base is added.

It contains similar amounts of a strong acid and a strong base.

Its pH undergoes no change when either strong acid or strong base is added.

It contains similar amounts of a weak acid and its conjugate base.

Its pH changes only slightly when either strong acid or strong base is added.

It contains similar amounts of a weak acid and its conjugate base.

Bodies of water near limestone deposits (CaCO3) contain appreciable quantities of both the bicarbonate and ______ anions. This helps to buffer them term-66against the effects of rain ______.

carbonate

acidic

What reaction occurs when strong acid is added to a buffer solution?

The strong acid reacts with the weak acid in the buffer to produce more weak acid.

The strong acid reacts with the weak conjugate base in the buffer and converts it to the weak acid.

The strong acid is diluted in the solution so that its presence has no significant effect on the pH.

The strong acid reacts with the weak base in the buffer and converts it to strong base.

The strong acid reacts with the weak conjugate base in the buffer and converts it to the weak acid.

A buffer solution undergoes only slight changes in _____ when either strong acid or strong base is added. It contains similar amounts of a _____ acid and its conjugate ____.

P\pH

weak

base

When strong acid is added to a buffer solution, it reacts with the weak ____ that is present, converting it into the weak _____.

base

acid

The primary components of the buffer system for maintaining a pH of ~7.4 in human blood are ____acid and its conjugate base ____.

carbonic

bicarbonate

During a nuclear reaction, what part of the atom participates in the reaction?

only the protons in the nucleus

subatomic particles of the nucleus

inner electrons

valence electrons

subatomic particles of the nucleus

which of following statements correctly describe the atoms of a given element?

all atoms of an element have the same number of protons

all atoms of an element have the same atomic number

all atoms of an element have the same mass

all atoms of an element have the same number of neutrons

all atoms of an element have the same number of protons

all atoms of an element have the same atomic number

Which statement correctly describe isotopes?

While many isotopes are stable, a greater number of isotopes are radioactive.

Radioisotopes are unstable isotopes of an atom.

Radioactive isotopes spontaneously emit energy to form a more stable nucleus.

Radioisotopes are stable isotopes of an atom that emit energy.

While many isotopes are stable. a greater number of isotopes are radioactive.

Radioisotopes are unstable isotopes of an atom.

Radioactive isotopes spontaneously emit energy to form a more stable nucleus.

Which subatomic particles comprise the atom in nuclear reactions?

Proton

Neutron

Electron

True or False: There are artificial isotopes that are radioactive.

True

True or False: Unstable atoms emit radiation, whereas stable nuclei do not.

True

Which of the following statements about radioactive decay and nuclear reactions are correct? Select all that apply.

Radioactive decay is the process by which an unstable radioactive nucleus emits radiation.

A nuclear equation contains the original nucleus, the new nucleus, and the radiation emitted.

In a nuclear equation, the sum of the mass numbers in the reactants must be equal to the sum of the mass numbers in the products.

Alpha Particle

Contains 2 protons and 2 neutrons.

Gamma Radiation

High-energy Radiation

In positron emission, a proton decays into what type of particle(s)?

A positron and a neutron.

How do you balance a nuclear equation?

Balance the mass numbers and atomic numbers on each side of the equation.