Chapter 14

What is the freezing-point depression of an aqueous solution of an electrolyte that produces three ions for every formula unit that dissociates if the electrolyte's concentration is 1.25 m?Kf = -1.86°C/m. a) -1.25°C b) -6.98°C c) -1.86°C d) -5.58°C

-6.98°C

The pH scale in general use ranges from 0 to 14. 0 to 1. -1 to 1. 0 to 7.

0 to 14.

What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L solution? a) 0.0132 M b) 0.0253 M c) 0.459 M d) 1.363 M

0.0253 M

32.4 mL of a 0.58 M solution of H3PO4 is titrated with NaOH. It takes 40 mL of NaOH to reach the equivalence point. What is the concentration (molarity) of the NaOH? Answer to 2 decimals. NO BALANCING YOU SILLY GOOSE

1.41

83.3 mL of a 0.547 M solution of H2SO4 is titrated with NaOH. It takes 48.8 mL of NaOH to reach the equivalence point. What is the concentration (molarity) of the NaOH? Answer to 2 decimals. NO BALANCING YOU SILLY GOOSE

1.87

The antilogarithm of a number, y, is the inverse of y. y raised to the power of 10. 10 raised to the power of y. the square root of y.

10 raised to the power of y.

Which expression represents the concentration of OH- ions in solution? 10-14 ¸ [H3O+] 10-14 ´ [H3O+] [OH-] ¸ 10-14 10-14 - [H3O+]

10-14 ¸ [H3O+]

Which expression represents the concentration of H3O+ ions in solution? (,=division) 10-14 ´ [OH-] 10-14 - [OH-] [OH-] ¸ 10-14 10-14 ¸ [OH-]

10-14 ¸ [OH-]

What is the pH of a 10-4 M HCl solution? 8 6 4 10

4

If [H3O+] = 8.26 ´ 10-5 M, what is the pH of the solution? 2.161 4.083 8.024 3.912

4.083

What is the hydronium ion concentration of a solution whose pH is 7.30? 1.4 ´ 10-11 M 5.0 ´ 10-8 M 7.1 ´ 10-6 M 3.8 ´ 10-8 M

5.0 ´ 10-8 M

A pressure of 745 mm Hg equals... a) 745 pascal b) 745 torr c) 1 pascal d) 1 torr

745 torr

The molar enthalpy of fusion for water is 6.008 kJ/mol. What quantity of energy is released when 253 g of liquid water freezes? (Molar mass of water is 18.02 g/mol.) a) 759 kJ b) 84.4 kJ c) 2.33 kJ d) 0.429 kJ

84.4 kJ

The ideal gas law combines Boyle's law, Charles's law, Gay-Lussac's Law and... a) Dalton's principle. b) Graham's law. c) Avogadro's law. d) Raoult's law.

Avogadro's law.

In the reaction represented by the equation , H2O is a(n)... a) Arrhenius. b) Brønsted-Lowry base. c) Lewis base. d) Brønsted-Lowry acid.

Brønsted-Lowry acid.

Which of the following is not a strong acid? a) HNO3 b) HCl c) H2SO4 d) CH3COOH

CH3COOH

Which of the following is not an oxyacid? a) H2SO4 b) HClO4 c) H2O2 d) HClO2

H2O2

Which of the following is a triprotic acid? H3PO4 HCl H2SO4 CH3COOH

H3PO4

In the equation HCl(g) + H2O(l) ® H3O+(aq) + Cl-(aq), which species is a Brønsted-Lowry acid? a) HCl b) Cl- c) H2O d) None of the above

HCl

In the reaction represented by the equation HF + H2O ⇔ H3O+ + F-, a conjugate acid-base pair is... a) F- and H2O. b) HF and H2O. c) H3O+ and HF. d) HF and F-.

HF and F-.

Which of the following is amphoteric? a) H+ b) SO4 c) HSO4- d) H2SO4

HSO4

Which of the following is a strong base? KOH NH3 HCl H2

KOH

An electron-pair donor is a... a) Arrhenius acid. b) Brønsted-Lowry base. c) Lewis base. d) Brønsted-Lowry acid.

Lewis base.

Which of the following gases does not dissolve in atmospheric water to produce acidic solutions? a) O2 b) NO c) NO2 d) CO2

O2

Why could the pressure of a sample of gas at a constant volume fall 75 mm Hg? a) The temperature decreased. b) The temperature increased. c) The volume increased. d) The container exploded.

The temperature decreased.

Arrhenius theorized that a base is a chemical compound that a) increases the concentration of hydroxide ions when dissolved in water. b) increases the concentration of hydrogen ions when dissolved in water. c) decreases the concentration of hydrogen ions when dissolved in water. d) decreases the concentration of hydroxide ions when dissolved in water.

a) increases the concentration of hydroxide ions when dissolved in water.

A Brønsted-Lowry acid is a(n) a) proton donor. b) electron-pair acceptor. c) electron-pair donor. d) proton acceptor.

a) proton donor.

A metal solution is a(n)... a) emulsion. b) alloy. c) suspension. d) colloid.

alloy.

What is the hydronium ion concentration of a solution whose pH is 4.12? a) 5.1 ´ 10-6 M b) 7.6 ´ 10-5 M c) 4.4 ´ 10-8 M d) 6.4 ´ 10-5 M

b) 7.6 ´ 10-5 M

Which indicator is used to study neutralization of a strong acid with a strong base? a) phenolphthalein b) bromthymol blue c) methyl orange d) None of the above

b) bromthymol blue

A conjugate acid is the species that a) remains after a base has given up a proton. b) is formed by the addition of a proton to a base. c) is formed by the addition of a proton to an acid. d) remains after an acid has given up a proton.

b) is formed by the addition of a proton to a base.

Which acid is used mainly in the manufacture of explosives, rubber, plastics, dyes, and drugs? a) hydrochloric acid b) nitric acid c) sulfuric acid d) phosphoric acid

b) nitric acid

Which acid is used in batteries? a) phosphoric acid b) sulfuric acid c) nitric acid d) hydrochloric acid

b) sulfuric acid

In the reaction represented by the equation H3PO4 + H2O ⇔ H3O+ + H2PO4-, the ion H2PO4- acts as a(n)... a) spectator species. b) salt. c) base. d) acid.

base.

Stirring increases the rate of dissolution because it... a) lowers the temperature. b) decreases the surface area of the solute. c) brings fresh solvent into contact with the solute. d) raises the temperature.

brings fresh solvent into contact with the solute.

Whenever ammonia donates an electron pair to form a covalent bond, it acts as a(n) a) Arrhenius acid. b) Lewis acid. c) Lewis base. d) Brønsted-Lowry base.

c) Lewis base.

A binary acid contains a) two hydrogen atoms. b) hydrogen and three other elements. c) hydrogen and one other element. d) hydrogen and two other elements.

c) hydrogen and one other element.

Which indicator is used to study neutralization of a strong acid with a weak base? a) phenolphthalein b) bromthymol blue c) methyl orange d) None of the above

c) methyl orange

Suppose that two gases with unequal molar masses were injected into opposite ends of a long tube at the same time and allowed to diffuse toward the center. They should begin to mix... a) closer to the end that held the lighter gas. b) in approximately five minutes. c) closer to the end that held the heavier gas. d) exactly in the middle.

closer to the end that held the heavier gas.

What is the pH of a 0.00162 M NaOH solution? a) 3.841 b) 5.332 c) 9.923 d) 11.210

d) 11.210

What is the pH of a neutral solution at 25ºC? a) 0 b) 14 c) 1 d) 7

d) 7

Which of the following is chloric acid? a) HClO2 b) HClO c) HClO4 d) HClO3

d) HClO3

Whose acid definition is the broadest? a) Faraday b) Brønsted-Lowry c) Arrhenius d) Lewis

d) Lewis

The separation of ions that occurs when an ionic compound dissolves is called... a) dissociation. b) oxidation. c) ionization. d) precipitation.

dissociation.

A Lewis base is a(n) producer of OH- ions. electron-pair donor. electron-pair acceptor. proton acceptor.

electron-pair donor.

Which acid is produced in the stomach? a) phosphoric acid b) hydrochloric acid c) sulfuric acid d) nitric acid

hydrochloric acid

When added to water, acids produce __________ ion in solution. ANSWER USING A WORD, NOT A FORMULA.

hydronium

What is the key substance found in all basic solutions?

hydroxide

When added to water, bases produce __________ ion in solution.

hydroxide

Dyes with pH-sensitive colors are used as indicators. primary standards. titrants. None of the above

indicators

If [H3O+] of a solution is less than [OH-], the solution is always acidic. is always basic. might be acidic, basic, or neutral. is always neutral.

is always basic.

An acid-base titration involves a neutralization reaction. decomposition reaction. composition reaction. single-displacement reaction.

neutralization reaction.

Which acid turns yellowish on standing? a) acetic acid b) hydrochloric acid c) nitric acid d) phosphoric acid

nitric acid

An acid-base titration is carried out by monitoring pH. temperature. pressure. density.

pH

What is the transition interval for phenolphthalein? pH 3.1-4.4 pH 6.4-8.0 pH 8.0-10.0 pH 6.2-7.6

pH 8.0-10.0

Which indicator is used to study neutralization of a weak acid with a strong base? phenolphthalein None of the above methyl orange bromthymol blue

phenolphthalein

The two members of a conjugate acid-base pair differ by a proton. hydroxide ion. hydronium ion. water molecule.

proton

A Brønsted-Lowry base is a(n)... a) producer of OH- ions. b) proton acceptor. c) electron-pair donor. d) electron-pair acceptor.

proton acceptor.

The conjugate of a weak base is a... a) weak acid. b) strong base. c) weak base. d) strong acid.

strong acid.

What process measures the amount of a solution of known concentration required to react with a measured amount of a solution of unknown concentration? hydrolysis titration neutralization autoprotolysis

titration

Which quantity is directly measured in a titration? mass volume concentration density

volume

When titrating a weak acid with a strong base, the equivalence point will be above a pH of 7.0. cannot be determined by pH. will be below a pH of 7.0. will be at a pH of 7.0.

will be above a pH of 7.0.