Acid/ Base & Conjugate Acid & Conjugate Base

Which of the following is the correct definition of pH? log[OH-] -log[Ka] -log[H3O+] log[H3O+]

-log[H3O+]

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

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

Important pH levels Saliva= Stomach fluid= Blood= Urine=

5.8 - 7.1 1.6 - 1.8 7.4 4.6 - 8.0

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 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

Acid

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

Base

A compound that produces hydroxide ions in solution.

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

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.

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

A positron and a neutron.

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.

How do you balance a nuclear equation?

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

Which functional group is contained in all carboxylic acids? OH- COOH HCl CH

COOH

Which of the following compounds are Arrhenius bases? CH3COOH Ca (OH)2 KOH NaBr HNO3

Ca(OH)2 KOH

Chlorate changes to Chlorous acid Hydrochloric acid Chloric acid

Chloric acid

Chlorite changes to Chlorous acid Hydrochloric acid Chloric acid

Chlorous acid

Alpha Particle

Contains 2 protons and 2 neutrons.

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.

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 of the molecules shown below is a strong Bronsted-Lowey acid? HBr HBrO HBrO3 HBrO2

HBr

Which of the following are common strong Bronsted-Lowry acids? H2SO4 H3PO4 HCN HCl HNO3

HCl H2SO4 HNO3

Gamma Radiation

High-energy Radiation

Chloride changes to Chlorous acid Hydrochloric acid Chloric acid

Hydrochloric acid

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

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.

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.

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]

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-]

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

Which subatomic particles comprise the atom in nuclear reactions?

Proton Neutron Electron

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.

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.

Conjugate acid is....

The particle formed when a base gains a hydrogen ion.

Conjugate base is....

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

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.

What makes a compound an Arrhenius Base?

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

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.

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

True

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

True

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

True

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

True

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

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 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 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.

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

acceptor lone

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

acid or base.

Acids whose names end in "ide"

add prefix -hydro change "ide" to "ic acid."

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

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

base acid

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

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

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

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

Acids whose names end in "ate"

change ending to "ic acid."

Acids whose names end in "ite"

change ending to "ous acid."

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

conjugate

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

conjugate acid

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

conjugate base

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

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

dissociates or ionizes

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

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

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

hydrogen

The pH of a substance is a measure of its

hydronium ion concentration, therefore numbers = the same

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

hydronium or H3O+

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

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

iodic acid

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

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

Strong acid + strong base means that side of the equilibrium is.... not favored. favored.

not favored.

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

pH acidity

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

proton acid base

A Bronsted-Lowry base is a _____.

proton acceptor

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

spectator

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

stronger weaker

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

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