Chem. Health Science: Ch. 9 Acids & Bases

A condition in which the blood pH is less than 7.35.

acidosis

A condition in which the blood pH is greater than 7.45.

alkalosis

In an acidic solution, the hydroxide ion concentration will be _____ than the hydronium ion concentration; in a basic solution, the hydroxide ion concentration will be _____ than the hydronium ion concentration.

lower; greater

Hydrofluoric acid (HF) is a weak acid. When hydrofluoric acid is dissolved in water, the _____ side of the equilibrium shown below is favored. HF + H2O = F- + H3O+

left

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 _____, and therefore must contain a _____ pair of electrons.

acceptor; lone

An amphoteric species is a molecule or ion that can act as both a(n) _____ and a(n) _____.

acid; base

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

acid; base

Which of the following is a common shorthand notation for a Bronsted-Lowry acid? a) BH+ b) B: c) HA d) A-

c) HA

Since pH is a logarithmic scale, a difference of one pH unit between solutions corresponds to a _____-fold difference in hydronium ion concentration.

10

What is the pH of a solution with a hydronium ion concentration of 1 x 10^-6 M?

6

Match each description of a base with its proper definition. Base: - Bronsted-Lowry base - Arrhenius base Def.: - a compound that produces OH- ions in aqueous solution - an H+ acceptor

Bronsted-Lowry base: an H+ acceptor Arrhenius base: a compound that produces OH- ions in aqueous solution

Which of the following is a common shorthand for a Bronsted-Lowry base? a) A- b) HA c) B: d) BH+

C) B:

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.

O

Which functional group (grouping of atoms) is contained in all carboxylic acids? a) COOH b) HCl c) CH d) OH-

a) COOH

Which of the following acid/base combinations could be used to prepare a buffer solution? (choose all) a) HCN and KCN b) H2O and Ca(OH)2 c) KH2PO4 and K2HPO4 d) HNO3 and NaNO3 e) HNO2 and NaNO2

a) HCN and KCN c) KH2PO4 and K2HPO4 e) HNO2 and NaNO2

Which of the species listed can act as Bronsted-Lowry bases? Select all that apply. a) HCO3- b) HS- c) OH- d) BH3 e) CH4

a) HCO3- b) HS- c) OH-

Which of the following are common strong Bronsted-Lowry acids? Select all that apply. a) HCl b) HNO3 c) HCN d) H2SO4 e) H3PO4

a) HCl b) HNO3 d) H2SO4

Which of the following are examples of dissociation? (choose all) a) an acid reacts with water to form its conjugate base plus a hydronium ion b) silver chloride precipitates from an aqueous solution c) methane (CH4) reacts with oxygen to form carbon dioxide and water d) an ionic compound is dissolved in water

a) an acid reacts with water to form its conjugate base plus a hydronium ion d) an ionic compound is dissolved in water

In an aqueous solution of a strong acid, [H3O+] is _____ the acid concentration. a) equal to b) greater than c) less than

a) equal to

Which of the following are products of the reaction of an acid with sodium bicarbonate (NaHCO3)? (choose all) a) ionic salt b) hydrogen c) hydroxide d) carbon dioxide e) water

a) ionic salt d) carbon dioxide e) water

Which of the following statements about strong and weak Bronsted-Lowry bases are correct? (choose all) a) only a small portion of a weak base forms hydroxide ions in aqueous solution b) a strong base reacts with water to form hydronium ions c) a strong base dissociates completely into hydroxide ions d) the strength of a base is directly proportional to its solubility in water

a) only a small portion of a weak base forms hydroxide ions in aqueous solution c) a strong base dissociates completely into hydroxide ions

For a strong base such as KOH, what is the relationship between the base concentration and hydroxide ion concentration? a) the hydroxide ion concentration is equal to the base concentration b) the hydroxide ion concentration is greater than the base concentration c) the hydroxide ion concentration is equal to the square root of the base concentration d) the hydroxide ion concentration is equal to K w divided by the base concentration

a) the hydroxide ion concentration is equal to the base concentration

Hydrofluoric acid (HF) is a stronger acid than hydrocyanic acid (HCN). Which statement about their conjugate bases is correct? a) cyanide (CN-) is a weaker base than fluoride b) cyanide (CN-) is a stronger base than fluoride c) it is not possible to determine the relative strengths of bases from their conjugate acids d) since cyanide (CN-) and fluoride are both weak bases, they have the same strength

b) cyanide (CN-) is a stronger base than fluoride

Ammonium (NH4+) is a stronger acid than water. Which side will be favored in the equilibrium shown below? NH4+ + OH- = NH3 + H2O a) left side (reactants) b) right side (products)

b) right side (products)

For a strong acid, what is the relationship between the hydronium ion concentration and the acid concentration in aqueous solution? a) the hydronium ion concentration is greater than the acid concentration b) the hydronium ion concentration is equal to the acid concentration c) the hydronium ion concentration is equal to K a d) the hydronium ion concentration is equal to K w divided by the acid concentration

b) the hydronium ion concentration is equal to the acid concentration

Which statement about weak acids is correct? a) weak acids are not able to donate a proton b) weak acids only partially dissociate in aqueous solution c) weak acids are strong bases d) weak acids are not water soluble

b) weak acids only partially dissociate in aqueous solution

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 process of splitting a substance into individual ions is known as _____. a) equilibrium b) precipitation c) dissociation d) oxidation

c) dissociation

Which of the following statements correctly describe a buffer solution? (choose all) a) its pH undergoes no change when either a strong acid or a strong base is added b) it contains similar amounts of a strong acid and a strong base c) it contains similar amounts of a weak acid and its conjugate base d) its pH changes only slightly when either a strong acid or a strong base is added

c) it contains similar amounts of a weak acid and its conjugate base d) its pH changes only slightly when either a strong acid or a strong base is added

A chemical equation that contains only the species involved in the reaction is called a(n) _____. a) spectator ion b) acid-base reaction c) net ionic equation d) neutralization reaction

c) net ionic equation

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

carbonate; 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

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

carbonic; water

Match each anion with the name of the acid that is derived from it. Anion: - chloride - chlorite - chlorate Acid: - hydrochloric acid - chlorous acid - chloric acid

chloride: hydrochloric acid chlorite: chlorous acid chlorate: chloric acid

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

conjugate

Which of the following is the correct definition of pH? a) log[H3O+] b) log[OH-] c) -log[K a] d) -log[H3O+]

d) -log[H3O+]

What is the hydroxide ion concentration in a 0.010 M solution of NaOH? a) 0.10 M b) 1.0 x 10^12 M c) 1.0 x 10^-7 M d) 0.010 M

d) 0.010 M

Carbonic acid (H2CO3) contains two acidic hydrogen atoms, and would therefore be known as a(n) _____ acid.

diprotic

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

According to the Bronsted-Lowry definition, acids are proton donors. The "proton" being donated is in fact a(n) _____ atom that has lost its electron. Thus, it is an ion that has the symbol _____, and not a proton from the nucleus of an atom.

hydrogen; H+

A Bronsted-Lowry acid must contain at least one _____ atom. In an aqueous solution, a Bronsted-Lowery acid donates an H+ ion to water to form a(n) _____ ion.

hydrogen; hydronium

A strong acid will react with a molecule of water to form a(n) _____ ion. In this reaction, water acts as a Bronsted-Lowry _____.

hydronium; base

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

Match each human body fluid listed below with its typical pH. Body Fluid: - saliva - stomach fluid - blood - urin pH: - 4.6-8.0 - 1.6-1.8 - 5.8-7.1 - 7.4

saliva: 5.8-7.1 stomach fluid: 1.6-1.8 blood: 7.4 urine: 4.6-8.0

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

spectator