SmartBook Ch. 4 Pt. III

Which of the following options gives the correct net ionic equation for the reaction between an aqueous solution of the weak acid HNO2 and aqueous lithium hydroxide, LiOH? a) HNO2 (aq) + LiOH (aq) → H2O (l) + LiNO2 (aq) b) H+ (aq) + NO2- (aq) + Li+ (aq) + OH- (aq) →H2O (l) + Li+ (aq) + NO2- (aq) c) HNO2 (aq) + OH- (aq) → H2O (l) + NO2- (aq) d) H3O+ (aq) + OH- (aq) → 2H2O (l)

c) HNO2 (aq) + OH- (aq) → H2O (l) + NO2- (aq)

Strong acids and bases dissociate completely in water and are therefore classified as _____. a) weak electrolytes b) concentrated solutions c) strong electrolytes d) nonelectrolytes

c) strong electrolytes

A(n) _____ is a procedure in which the known concentration of one solution is used to determine the unknown concentration of another. a) acid-base titration b) dilution c) titration d) redox

c) titration

A procedure in which the known concentration of one solution is used to determine the unknown concentration of another is called a(n) _____.

titration

How many milliliters of 0.120 M H3PO4 are needed to neutralize a solution containing 0.750 g of KOH (56.11 g/mol)? a) 37.1 mL b) 0.0371 mL c) 111 mL d) 55.5 mL e) 0.0555 mL

a) 37.1 mL

Which of the following are considered bases? Select all that apply. a) NH3 b) CH3COOH c) Na2O d) Ca(OH)2 e) K2SO4

a) NH3 c) Na2O d) Ca(OH)2

Which of the following features are often present in the formula of a compound that is a strong base? Select all that apply. a) O2- b) OH- c) N d) K+

a) O2- b) OH-

One definition for acids and bases describes each type of substance in terms of the ions it produces in aqueous solution. Match each type of substance with the ion produced in water. 1) Acid 2) Base a) OH- b) H+

b, a

Which of the following options correctly describe the products of the reaction between a strong acid and a strong base in aqueous solutions? Select all that apply. a) The net ionic equation is typically given by H+ (aq) + OH- (aq) → H2O (l). b) There is no net ionic equation as all species are soluble in water. c) The reaction produces H3O+ and OH- ions. d) The reaction usually produces an insoluble precipitate. e) The reaction forms a salt and water.

a) The net ionic equation is typically given by H+ (aq) + OH- (aq) → H2O (l). e) The reaction forms a salt and water.

Why is an acid able to produce ions in aqueous solution? Assume that the general formula of an acid is given by HA, where A is usually a halogen or oxygen atom. a) The polar H-A bond breaks due to the attraction between H and the O of water. b) An acid is an ionic compound that dissociates when it dissolves in water. c) An acid contains electrons that are released in solution to form ions.

a) The polar H-A bond breaks due to the attraction between H and the O of water.

A titration is carried out using a 0.250 M solution of sulfuric acid and 35.2 mL of 0.450 M NaOH. Select all the options that correctly reflect the quantities of the two substances at the equivalence point. The balanced molecular equation is H2SO4 (aq) + 2NaOH (aq) → 2H2O (l) + Na2SO4 (aq). a) The volume of H2SO4 used is equal to 31.7 mL. b) The volume of H2SO4 used is equal to 63.4 mL. c) 3.16 × 10-2 mol of H2SO4 are required to neutralize the NaOH. d) There are 1.58 × 10-2 moles of NaOH present in the original solution.

a) The volume of H2SO4 used is equal to 31.7 mL. d) There are 1.58 × 10-2 moles of NaOH present in the original solution.

The ionic compound that results from the reaction between an acid and a base is called _____. a) a salt b) a neutralization c) sodium chloride d) a soap e) water

a) a salt

A(n) _____ releases H+ in water, therefore it must have one or more _____ atoms as part of its structure.

acid, hydrogen

Which of the following solutions are acidic? Select all that apply. a) CaCO3 (aq) b) CH3CH2COOH (aq) c) H3PO4 (aq) d) NaOH (aq) e) HBr (aq)

b) CH3CH2COOH (aq) c) H3PO4 (aq) e) HBr (aq)

Which of the following options gives the correct total ionic equation for the reaction between an aqueous solution of the weak acid HF and strong base aqueous potassium hydroxide, KOH? a) H+ (aq) + F-(aq) + K+ (aq) + OH-(aq) → H2O (l) + K+ (aq) + F- (aq) b) HF (aq) + K+ (aq) + OH- (aq) → H2O (l) + F- (aq) + K+ (aq) c) H3O+ (aq) + OH- (aq) → 2H2O (l) d) HF (aq) + KOH (aq) → H2O (l) + KF (aq)

b) HF (aq) + K+ (aq) + OH- (aq) → H2O (l) + F- (aq) + K+ (aq)

A compound is described as a strong acid. What does this term mean? Select all that apply. a) The molecules of the compound hold tightly to their H atoms. b) The compound ionizes completely in water. c) There are no intact molecules of the compound remaining in solution. d) The molarity of the solution is high. e) The molecules of the compound are strongly bonded and do not ionize.

b) The compound ionizes completely in water. c) There are no intact molecules of the compound remaining in solution.

How do the equations differ for the neutralization reaction between a strong acid/strong base and a weak acid/strong base? a) The weak acid must appear as an undissociated, intact molecule both on the reactant and product sides of the equation. b) The weak acid reactant must appear as an undissociated, intact molecule in the equation. c) The strong acid reactant must appear as an undissociated, intact molecule in the equation. d) The equations do not differ. e) The anion of the weak acid is a product, not a spectator ion.

b) The weak acid reactant must appear as an undissociated, intact molecule in the equation. e) The anion of the weak acid is a product, not a spectator ion.

The term salt refers to the ionic compound formed from a neutralization reaction in which the _____ comes from the base and the _____ comes from the acid. a) anion; cation b) cation; anion

b) cation; anion

The _____ occurs in an acid-base titration when the amount (in moles) of H+ ions is brought together with the same amount (in moles) of OH- ions in the starting solution. a) half-equivalence point b) equivalence point c) equilibrium point d) end point

b) equivalence point

How many milliliters of 0.120 M H2SO4 are needed to neutralize a solution containing 0.250 g of NaOH (40.00 g/mol)? a) 0.0104 mL b) 10.4 mL c) 52.1 mL d) 26.0 mL e) 0.0260 mL

d) 26.0 mL

Which of the following solutions is not considered to be acidic? a) H2SO3 (aq) b) HNO3 (aq) c) CH3COOH (aq) d) LiOH (aq) e) HF (aq)

d) LiOH (aq)

During the titration of an acid with a base, the _____ point is the point at which the amount of _____ ions in the original acid solution will have reacted with the _____ amount of OH- ions from the basic solution.

equivalence, hydrogen, same

An acid can be defined as a substance that produces _____ ions when dissolved in water, while a base produces _____ ions in aqueous solutions.

hydrogen, hydroxide

An acid is a covalently bonded substance that nonetheless produces _____ ions when dissolved in water. This occurs because the acid molecule contains a(n) _____ covalent bond between H and another atom X (such as the bond in H-Cl). The H of the acid is strongly attracted to the partially negative O atom of water. The H-X bond in the acid breaks and the acid _____.

hydrogen, polar, dissociates

When a strong acid reacts with a strong base, the products are typically a(n) _____ compound, which is called a(n) _____, and the neutral molecule _____.

ionic, salt, water

Strong acids and bases _____ completely into _____ in water. The resulting solution conducts electricity well; hence these compounds are classified as _____ electrolytes.

ionize, ions, strong

An ionic compound that results from the reaction of an acid and a base is called a(n) _____ . The cation in this compound comes from the _____ while the anion comes from the _____.

salt, base, acid

A(n) _____ acid or base will dissociate completely in water, whereas a(n) _____ acid or base dissociates very little in water.

strong, weak