Name: ____________________________________________

___ 1) Water containing a dissolved electrolyte conducts electricity because the solution contains mobileA) electrons B) molecules C) atoms D) ions

___ 2) Which compound is an electrolyte?A) C2H5OH B) C6H12O6 C) CH3COOH D) C12H22O11

___ 3) Which compounds are both classified as electrolytes?A) NH4Cl and C6H12O6B) C6H12O6 and CH3OH

C) KCl and CH3OH

D) NH4Cl and KCl

___ 4) Which of the following is a characteristic of a solution of HNO3?

A) It turns phenolphthalein pinkB) It conducts electricity.

C) It turns litmus blue.D) It forms OH- ions.

___ 5) Which of the following is the best conductor of electricity?A) NaCl(s) B) NaCl(aq) C) C6H12O6(s) D) C6H12O6(aq)

___ 6) The water solution of which substance is the best conductor of electricity?A) CO B) CO2 C) KCl D) C6H12O6

___ 7) Which substance dissolves in pure water and produces a solution that is a good conductor of electricity?A) CaCl2 B) N2 C) O2 D) C6H12O6

___ 8) A material will be used to fill an empty beaker to level A, as shown in the diagram below.

Which material, when used to fill the beaker to level A, would cause the bulb to glow brightly?A) C6H12O6(s) B) KCl(s) C) C6H12O6(aq) D) KCl(aq)

4719 - 1 - Page 1

___ 9) Beakers A, B, C, and D shown below each contain a different solution.

The bulb will glow when the conductivity apparatus is placed into which beakers?A) A and B B) A and D C) C and D D) B and C

___ 10) According to the Arrhenius theory, when an acid substance is dissolved in water it will produce a solution containing onlyone kind of positive ion. To which ion does the theory refer?A) hydrogen B) chloride C) sodium D) acetate

___ 11) According to the Arrhenius theory, a substance that yields hydrogen ions as the only positive ion in an aqueous solutionisA) a nonelectrolyteB) a base

C) an acidD) a salt

___ 12) When an Arrhenius acid is dissolved in water, it produces

A) HCO3- as the only negative ion in solution

B) OH- as the only negative ion in solution

C) H+ as the only positive ion in solution

D) NH4+ as the only positive ion in solution

___ 13) In an aqueous solution, which substance yields hydrogen ions as the only positive ions?A) KH B) C2H5OH C) KOH D) CH3COOH

___ 14) When substance X is dissolved in water, the only positive ions in the solution are hydrogen ions. Substance X could beA) NaH B) H2S C) NH3 D) NaOH

___ 15) Which substance can act as an Arrhenius acid in aqueous solution?A) HI B) LiH C) NH3 D) NaI

___ 16) Which species can act as an Arrhenius acid in aqueous solution?

A) Cl- B) HCl C) Li+ D) KH

___ 17) According to the Arrhenius theory, when a base is dissolved in water it will produce a solution containing only one kind ofnegative ion. To which ion does the theory refer?A) hydride B) hydronium C) hydroxide D) hydrogen

___ 18) According to the Arrhenius theory, when a base dissolves in water it produces

A) H+ as the only positive ion in solution

B) NH4+ as the only positive ion in solution

C) CO32- as the only negative ion in solution

D) OH- as the only negative ion in solution

___ 19) Unlike an acid, an aqueous solution of a base

A) contains more OH- ions than H+ ionsB) conducts electricity

C) contains more H+ ions than OH- ionsD) causes some indicators to change color

4719 - 1 - Page 2

___ 20) According to the Arrhenius theory, which list of compounds includes only bases?A) LiOH, Ca(OH)2, and C2H4(OH)2B) NaOH, Ca(OH)2, and CH3COOH

C) KOH, Ca(OH)2, and CH3OH

D) KOH, NaOH, and LiOH

___ 21) Which substance is classified as an Arrhenius base?A) KHCO3 B) NaOH C) LiNO3 D) HCl

___ 22) An aqueous solution of an ionic compound turns red litmus blue, conducts electricity, and reacts with an acid to form a saltand water. This compound could beA) LiOH B) HCl C) NaI D) KNO3

___ 23) According to the Bronsted-Lowry theory, an acid isA) neither a proton donor nor a proton acceptorB) a proton acceptor, only

C) a proton donor and a proton acceptorD) a proton donor, only

___ 24) Which species is classified as a Bronsted acid?A) LiOH B) H2SO4 C) CH3OH D) NaCl

___ 25) Given the reaction:

HX + H2O ‡‡ˆ H3O+(aq) + X-(aq)

Based on the equation, HX would be classified asA) an acid, because it accepts a protonB) a base, because it accepts a proton

C) an acid, because it donates a protonD) a base, because it donates a proton

___ 26) Given the reaction:

HCl(g) + H2O(l) ‡‡ˆ H3O+(aq) + Cl-(aq)

Which reactant acted as a Bronsted-Lowry acid?A) HCl(g), because it donated protonsB) H2O(l), because it accepted protons

C) HCl(g), because it reacted with chloride ionsD) H2O(l), because it produced hydronium ions

___ 27) As HF dissolves in water, the following ionization reaction occurs:

HF + H2O ‰Š‹ H3O+ + F-

In this reaction, a proton is donated to

A) H3O+ by H2O

B) H3O+ by F-

C) H2O by HF

D) HF by F-

___ 28) Given the reaction at equilibrium:

NH4+ + OH- ‰Š‹ H2O + NH3

What species is the Bronsted-Lowry acid in the forward reaction?

A) NH4+ B) NH3 C) H2O D) OH-

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___ 29) Given the reaction:

HF + H2O ‰Š‹ F- + H3O+

What species is the Bronsted acid in the reverse reaction?

A) HF B) H3O+ C) F- D) H2O

___ 30) Given reactions A and B:

(A) HCl + H2O ‡‡ˆ Cl- + H3O+

(B) HCl + HS- ‡‡ˆ Cl- + H2S

In which of the reactions can HCl be classified as a Bronsted-Lowry acid?A) B, onlyB) A, only

C) neither A nor BD) both A and B

___ 31) In the reaction NO2-(aq) + H2O(l) ‡‡ˆ HNO2(aq) + OH-(aq), the NO2

-(aq) acts as

A) an Arrhenius baseB) an Arrhenius acid

C) a Bronsted acidD) a Bronsted base

___ 32) In the reaction H2O + H2O ‡‡ˆ H3O+ + OH-, the water is acting as

A) a proton donor, onlyB) both a proton acceptor and donor

C) a proton acceptor, onlyD) neither a proton acceptor nor donor

___ 33) Given the reaction:

HSO4-(aq) + NH3(g) ‰Š‹ NH4

+(aq) + SO42-(aq)

Which of the following statements best describes the action of NH3(g) in the reaction?

A) It acts as an acid, because it is a proton donor.B) It acts as an acid, because it is a proton acceptor.C) It acts as a base, because it is a proton acceptor.D) It acts as a base, because it is a proton donor.

___ 34) Given the reactions X and Y below:

X: H2O + NH3 ‡‡ˆ NH4+ + OH-

Y: H2O + HSO4- ‡‡ˆ H3O+ + SO4

2-

Which of the following statements best describes the behavior of the H2O in these reactions?

A) Water acts as an acid in both reactions.B) Water acts as a base in reaction X and as an acid in reaction Y.C) Water acts as an acid in reaction X and as a base in reaction Y.D) Water acts as a base in both reactions.

___ 35) Which formula represents a conjugate acid-base pair?

A) CH3COOH and CH3COO-

B) H3O+ and OH-

C) H3PO4 and PO43-

D) H2SO4 and SO42-

___ 36) What is a conjugate acid-base pair in the reaction H2O + HI ‰Š‹ H3O+ + I-?

A) H2O and I- B) H2O and HI C) HI and I- D) HI and H3O+

4719 - 1 - Page 4

___ 37) In the reaction HCl + H2O ‰Š‹ H3O+ + Cl-, a conjugate acid-base pair is

A) HCl and H2O

B) HCl and H3O+

C) H2O and Cl-

D) HCl and Cl-

___ 38) In the reaction HBr + H2O ‰Š‹ H3O+ + Br-, which is a conjugate acid-base pair?

A) HBr and H2O

B) HBr and Br-C) H3O+ and Br-

D) H3O+ and HBr

___ 39) In the reaction H2PO4- + H2O ‰Š‹ H3PO4 + OH-, which pair represents an acid and its conjugate base?

A) H3PO4 and H2PO4-

B) H2O and H2PO4-

C) H3PO4 and OH-

D) H2O and H3PO4

___ 40) In the reaction CH3COOH + H2O ‰Š‹ CH3COO- + H3O+ a conjugate acid-base pair is

A) CH3COO- and H2O

B) CH3COO- and H3O+

C) CH3COOH and H3O+

D) CH3COOH and CH3COO-

___ 41) Given the reaction:

HSO4- + H2O ‰Š‹ H3O+ + SO4

2-

Which is a Bronsted-Lowry conjugate acid-base pair?

A) H2O and SO42-

B) HSO4- and SO4

2-

C) HSO4 and H3O+

D) H2O and HSO4-

___ 42) In the reaction H2SO4 + H2O ‰Š‹ H3O+ + HSO4-, which two are proton donors?

A) H2O and H3O+

B) H2O and HSO4-

C) H2SO4 and H3O+

D) H2SO4 and HSO4-

___ 43) Given the equation:

H2O + HF ‰Š‹ H3O+ + F-

Which pair represents Bronsted-Lowry acids?

A) HF and H3O+

B) HF and F-

C) H2O and H3O+

D) H2O and F-

___ 44) In the reaction H2O + CO32- ‰Š‹ OH- + HCO3

-, the two Bronsted-Lowry acids are

A) CO32- and HCO3

-

B) H2O and HCO3-

C) CO32- and OH-

D) H2O and OH-

___ 45) In the reaction HS- + NH2- ‰Š‹ NH3 + S2-, the two Bronsted bases are

A) HS- and NH2-

B) S2- and NH3

C) HS- and NH3

D) S2- and NH2-

4719 - 1 - Page 5

___ 46) Given the reaction at equilibrium:

HSO4- + H2O ‰Š‹ H3O+ + SO4

2-

The two Bronsted bases are

A) H2O and SO42-

B) H3O+ and SO42-

C) H2O and H3O+

D) H3O+ and HSO4-

___ 47) In the reaction H2S + NH3 ‰Š‹ NH4+ + HS-, the two Bronsted bases are

A) H2S and HS-

B) NH3 and HS-

C) H2S and NH3

D) NH3 and NH4+

___ 48) What is the conjugate base of NH3?

A) NH2- B) NO2

- C) NH4+ D) NO3

-

___ 49) What is the conjugate base of OH-?

A) O2- B) H+ C) H3O+ D) H2O

___ 50) What is the conjugate acid of the HCO3- ion?

A) H3CO3+ B) H+ C) H2CO3 D) CO3

2-

___ 51) What is the conjugate acid of the HSO4- ion?

A) H2SO4 B) SO3 C) H+ D) SO42-

___ 52) Given the reactions:

(A) NH3(g) + H2O(l) ‡‡ˆ NH4+(aq) + OH-(aq)

(B) HCl(aq) + H2O(l) ‡‡ˆ H3O+(aq) + Cl-(aq)

As shown in equations (A) and (B) and based on the Bronsted theory, water is an amphoteric substance because it canA) accept protons, onlyB) neither donate nor accept protons

C) donate protons, onlyD) either donate or accept protons

___ 53) Which equation illustrates the amphiprotic properties of a reactant species?

A) HCl(aq) + H2O(l) ‡‡ˆ H3O+(aq) + Cl-(aq)

B) NH3(aq) + H2O(l) ‡‡ˆ NH4+(aq) + OH-(aq)

C) H2O(l) + H2O(l) ‡‡ˆ H3O+(aq) + OH-(aq)

D) 2H2(g) + O2(g) ‡‡ˆ 2H2O(l)

___ 54) An aqueous solution that has a hydrogen ion concentration of 1.0 x 10-8 mole per liter has a pH ofA) 6, which is basicB) 8, which is acidic

C) 8, which is basicD) 6, which is acidic

___ 55) A water solution that has an H+ ion concentration of 1 x 10-8 mole per liter is classified asA) basic, with a pH less than 7B) basic, with a pH greater than 7

C) acidic, with a pH greater than 7D) acidic, with a pH less than 7

___ 56) If a solution has a hydronium ion concentration of 1 x 10-9 M, the solution isA) basic and has a pH of 9B) basic and has a pH of 5

C) acidic and has a pH of 5D) acidic and has a pH of 9

4719 - 1 - Page 6

___ 57) The H3O+ ion concentration of a solution is 1 x 10-5 mole per liter. This solution is

A) basic and has a pH of 5B) acidic and has a pH of 5

C) basic and has a pH of 9D) acidic and has a pH of 9

___ 58) The H3O+ ion concentration of a solution is 1 x 10-4 mole per liter. This solution is

A) acidic and has a pH of 10B) basic and has a pH of 10

C) basic and has a pH of 4D) acidic and has a pH of 4

___ 59) What is the H+ ion concentration of an aqueous solution that has a pH of 11?

A) 11 x 10-1 mol/L

B) 3.0 x 10-1 mol/L

C) 1.0 x 10-3 mol/L

D) 1.0 x 10-11 mol/L

___ 60) What is the pH of a solution that has a hydronium ion concentration of 1 x 10-8 mole per liter?A) 1 B) 8 C) 7 D) 4

___ 61) What is the pH of a solution whose H3O+ ion concentration is 0.0001 mole per liter?

A) 1 B) 10 C) 14 D) 4

___ 62) What is the pH of a 0.00001 molar HCl solution?A) 1 B) 5 C) 9 D) 4

___ 63) What is the pH of a 0.001 M solution of HCl?A) 1 B) 7 C) 3 D) 11

___ 64) What is the H3O+ ion concentration of a solution whose OH- ion concentration is 1 x 10-3 M?

A) 1 x 10-14 M B) 1 x 10-11 M C) 1 x 10-7 M D) 1 x 10-4 M

___ 65) What is the hydroxide ion concentration of a solution with a pH of 4?

A) 1 x 10-14 B) 1 x 10-7 C) 1 x 10-10 D) 1 x 10-4

___ 66) Which solution will turn litmus from red to blue?A) SO2(aq) B) NH3(aq) C) CO2(aq) D) H2S(aq)

___ 67) Which solution will change red litmus to blue?A) HCl(aq) B) NaCl(aq) C) CH3OH(aq) D) NaOH(aq)

___ 68) Which solution will change litmus paper red?A) NH4OH(aq)

B) NaOH(aq)

C) CH3COOH(aq)

D) CH3OO-(aq)

___ 69) In a solution with a pH of 3, the color ofA) phenophthalein is blueB) litmus is blue

C) phenophthalein is redD) litmus is red

___ 70) In the solution, litmus is blue. The pH of the solution could beA) 10 B) 2 C) 3 D) 4

___ 71) One sample of a solution with a pH of 10 is tested with phenolphthalein and another sample of this solution is tested withlitmus. In this solution the color of the litmus isA) blue and the phenolphthalein is pinkB) red and the phenolphthalein is pink

C) red and the phenolphthalein is colorlessD) blue and the phenolphthalein is colorless

___ 72) In a 0.01 M solution of HCl, litmus will beA) blue and phenolphthalein will be colorlessB) red and phenolphthalein will be colorless

C) red and phenolphthalein will be pinkD) blue and phenolphthalein will be pink

___ 73) What color is phenolphthalein in a solution that has a pH of 9?A) pink B) blue C) colorless D) white

4719 - 1 - Page 7

___ 74) Which solution can turn phenolphthalein pink?A) CH3OH(aq)

B) HCl(aq)

C) CH3COOH(aq)

D) NaOH(aq)

___ 75) The results of testing a colorless solution with three indicators are shown in the table below.

Which formula could represent the solution tested?A) HCl(aq)B) C12H22O11(aq)

C) NaOH(aq)D) C6H12O6(aq)

___ 76) The table below shows the color of an indicator in specific pH ranges.

If this indicator is used when titrating an unknown strong base by adding a strong acid, the color of the indicator willchange fromA) blue to greenB) green to orange

C) orange to greenD) green to blue

___ 77) Methyl orange indicator is added to a beaker containing a solution of HCl with a pH of 2.0. What color change occurs asNaOH(aq) is added to the beaker?A) blue to red B) red to yellow C) yellow to red D) red to blue

___ 78) Which indicators would cause a sodium hydroxide solution with a pH of 10.0 to turn blue?A) litmus and methyl orangeB) litmus and phenolphthalein

C) thymol blue and litmusD) thymol blue and methyl orange

___ 79) Household vinegar has a pH of approximately 3.0. Which would appear yellow when added to a vinegar solution?A) bromcresol greenB) methyl orange

C) litmusD) phenolphthalein

___ 80) Which solution will change bromthymol blue indicator from yellow to blue?A) CH3OH(aq)

B) KOH(aq)

C) CH3COOH(aq)

D) HCl(aq)

___ 81) Which solution will change thymol blue indicator from blue to yellow?A) CH3COOH(aq)

B) CH3OH(aq)

C) KOH(aq)

D) NaOH(aq)

___ 82) What is the pH of a solution that changes both methyl orange and litmus indicators red?A) 6 B) 2 C) 8 D) 4

___ 83) What is the pH of a solution that changes thymol blue indicator yellow and bromthymol blue indicator blue?A) 6.0 B) 3.2 C) 7.8 D) 9.6

4719 - 1 - Page 8

___ 84) Which equation represents a neutralization reaction?A) AgNO3 + NaCl ‡‡ˆ AgCl + NaNO3B) 2Na + 2H2O ‡‡ˆ 2NaOH + H2

C) NaOH + HCl ‡‡ˆ NaCl + H2O

D) Zn + CuSO4 ‡‡ˆ ZnSO4 + Cu

___ 85) Which equation represents a neutralization reaction?A) NaCl(aq) + AgNO3(aq) ‡‡ˆ NaNO3(aq) + AgCl(s)

B) Ag+(aq) + I-(aq) ‡‡ˆ AgI(s)C) Zn(s) + 2HCl(aq) ‡‡ˆ ZnCl2(aq) + H2(g)

D) H+(aq) + OH-(aq) ‡‡ˆ H2O(l)

___ 86) Which of the following is a net ionic equation for a neutralization reaction?

A) Ag+ + Cl- ‡‡ˆ AgCl

B) H+ + HCO3- ‡‡ˆ H2CO3

C) NH4+ + OH- ‡‡ˆ NH4OH

D) H+ + OH- ‡‡ˆ H2O

___ 87) What products are formed when an acid reacts with a base?A) a salt and waterB) a soap and glycerine

C) an alcohol and carbon dioxideD) an ester and water

___ 88) Given the neutralization reaction:

H2SO4 + 2KOH ‡‡ˆ K2SO4 + 2HOH

Which compound is a salt?A) KOH B) H2SO4 C) HOH D) K2SO4

___ 89) Which compound is a salt?A) Na3PO4 B) H3PO4 C) CH3COOH D) Ca(OH)2

___ 90) Which compound is a salt?A) H2C2O4 B) C6H12O6 C) KC2H3O2 D) CH3OH

___ 91) Which formula represents a salt?A) CH3OH B) KOH C) CH3COOH D) KCl

___ 92) Which substance is classified as a salt?A) Ca(OH)2 B) CCl4 C) CaCl2 D) C2H4(OH)2

___ 93) If 50. milliliters of a 1.0 M NaOH solution is needed to exactly neutralize 10. milliliters of an HCl solution, the molarity of theHCl solution isA) 0.20 M B) 5.0 M C) 1.0 M D) 10. M

___ 94) If 50 milliliters (ml) of a 0.01 M HCl solution is required to neutralize exactly 25 milliliters (ml) of NaOH, what is theconcentration of the base?A) 0.02 M B) 0.0005 M C) 0.04 M D) 0.01 M

___ 95) If 50. milliliters of 0.50 M HCl is used to completely neutralize 25 milliliters of KOH solution, what is the molarity of thebase?A) 2.5 M B) 0.25 M C) 1.0 M D) 0.50 M

___ 96) In a titration, the endpoint of a neutralization reaction was reached when 37.6 milliliters of an HCl solution was added to17.3 milliliters of a 0.250 M NaOH solution. What was the molarity of the HCl solution?A) 0.250 M B) 0.115 M C) 0.543 M D) 0.203 M

___ 97) What is the molarity of a KOH solution if it requires 20. milliliters of 2.0 M HCl to exactly neutralize 20. milliliters of the KOHsolution?A) 1.0 M B) 2.0 M C) 10. M D) 20. M

4719 - 1 - Page 9

___ 98) A 3.0-milliliter sample of HNO3 solution is exactly neutralized by 6.0 milliliters of 0.50 M KOH. What is the molarity of theHNO3 sample?

A) 1.0 M B) 0.50 M C) 3.0 M D) 1.5 M

___ 99) If 20. milliliters of 4.0 M NaOH is exactly neutralized by 20. milliliters of HCl, the molarity of the HCl isA) 1.0 M B) 2.0 M C) 5.0 M D) 4.0 M

___ 100) In a titration experiment, 20. milliliters of 1.0 M HCl neutralized 10. milliliters of an NaOH solution of unknownconcentration. What was the concentration of the NaOH solution?A) 1.5 M B) 2.5 M C) 2.0 M D) 0.50 M

___ 101) How many milliliters of 5.0 M NaOH are needed to exactly neutralize 40. milliliters of 2.0 M HCl?A) 16 mL B) 8.0 mL C) 10. mL D) 40. mL

___ 102) How many milliliters of 0.4 M HCl are required to completely neutralize 200 milliliters of 0.16 M potassium hydroxide?A) 30 mL B) 500 mL C) 200 mL D) 80 mL

___ 103) How many milliliters of 2.5 M HCl are required to exactly neutralize 15 milliliters of 5.0 M NaOH?A) 40. mL B) 30. mL C) 10. mL D) 20. mL

___ 104) What volume of a 0.200 M NaOH solution is needed to exactly neutralize 40.0 milliliters of a 0.100 M HCl solution?A) 20.0 mL B) 40.0 mL C) 80.0 mL D) 10.0 mL

___ 105) In the laboratory, a student neutralized 0.20 M HCl with 0.40 M KOH.

(a) Write the balanced equation for the reaction between HCl and KOH.

(b) How many milliliters of 0.20 M HCl are needed to exactly neutralize 40. milliliters of 0.40 M KOH? [Write the correctformula. Show all work. Indicate the correct answer with an appropriate unit.]

___ 106) In the laboratory, a student neutralized 1.5 M HNO3 with 0.50 M KOH.

(a) Write the balanced equation for the reaction between HNO3 and KOH.

(b) How many milliliters of 0.50 M KOH are needed to exactly neutralize 10. milliliters of 1.5 M HNO3? [Write the correctformula. Show all work. Indicate the correct answer with an appropriate unit.]

___ 107) In the laboratory, a student titrated HNO3 with 0.50 M LiOH until the indicator changed from colorless to pink.

(a) Write the balanced equation for the reaction between HNO3 and LiOH.

(b) If 50. milliliters of 0.50 M LiOH is required to exactly neutralize 100. milliliters of an HNO3 solution, what is themolarity of the HNO3 solution? [Write the correct formula. Show all work. Indicate the correct answer with anappropriate unit.]

(c) What indicator was used in the titration?

4719 - 1 - Page 10

___ 108) In the laboratory, a student titrated NaOH with 3.0 M HNO3.

(a) Write the balanced equation for the reaction between HNO3 and NaOH.

(b) If 50. milliliters of 3.0 M HNO3 completely neutralized 150 milliliters of NaOH, what was the molarity of the NaOHsolution? [Write the correct formula. Show all work. Indicate the correct answer with an appropriate unit.]

___ 109) In the laboratory, a student titrated NaOH with 1.0 M HCl.

(a) Write the balanced equation for the reaction between HCl and NaOH.

(b) If 20. milliliters of a 1.0 M solution of HCl is exactly neutralized by 40. milliliters of NaOH, what is the molarity of theNaOH solution? [Write the correct formula. Show all work. Indicate the correct answer with an appropriate unit.]

___ 110) In the laboratory, a student titrated HCl with 1.0 M NaOH.

(a) Write the balanced equation for the reaction between HCl and NaOH.

(b) If 50. milliliters of a 1.0 M NaOH solution is needed to exactly neutralize 10. milliliters of an HCl solution, what is themolarity of the HCl solution? [Write the correct formula. Show all work. Indicate the correct answer with anappropriate unit.]

___ 111) In the laboratory, a student neutralized 0.10 M LiOH with 0.20 M HCl.

(a) Write the balanced equation for the reaction between HCl and LiOH.

(b) What is the maximum volume of 0.10 M LiOH that can be completely neutralized by 25 milliliters of 0.20 M HCl?[Write the correct formula. Show all work. Indicate the correct answer with an appropriate unit.]

___ 112) In the laboratory, a student neutralized 1.0 M H2SO4 with 1.0 M NaOH.

(a) Write the balanced equation for the reaction between H2SO4 and NaOH.

(b) How many milliliters of 1 M NaOH are needed to exactly neutralize 100 milliliters of 1 M H2SO4? [Write the correctformula. Show all work. Indicate the correct answer with an appropriate unit.]

4719 - 1 - Page 11

___ 113) In the laboratory, a student performed an acid-base titration. The diagram below shows NaOH(aq) being added toHCl(aq).

The following data was collected:

Volume of the acid, HCl = 20.0 mLMolarity of the acid = 0.50 MVolume of the base, NaOH = 40.0 mL

(a) Write the balanced equation for the reaction between HCl and NaOH.

(b) Based on the data above, calculate the molarity of the NaOH. [Write the correct formula. Show all work. Indicatethe correct answer with an appropriate unit.]

(c) What color does the indicator appear at the endpoint of the titration?

(d) What name is given to the reaction between equivalent quantities of an acid and a base?

___ 114) The compound HNO3 can be described as an

A) Arrhenius acid and a nonelectrolyteB) Arrhenius base and an electrolyte

C) Arrhenius acid and an electrolyteD) Arrhenius base and a nonelectrolyte

___ 115) Which substance is an Arrhenius acid?A) Mg(OH)2(aq)

B) HBr(aq)

C) CH3CHO

D) LiF(aq)

___ 116) How are HNO3(aq) and CH3COOH(aq) similar?

A) They are Arrhenius acids and they turn red litmus blue.B) They are Arrhenius bases and they turn red litmus blue.C) They are Arrhenius bases and they turn blue litmus red.D) They are Arrhenius acids and they turn blue litmus red.

4719 - 1 - Page 12

___ 117) Given the following solutions:

Solution A: pH of 10Solution B: pH of 7Solution C: pH of 5

Which list has the solutions placed in order of increasing H+ concentration?A) C, B, A B) A, B, C C) C, A, B D) B, A, C

___ 118) When the pH of a solution changes from a pH of 5 to a pH of 3, the hydronium ion concentration isA) 100 times the original contentB) 10 times the original content

C) 0.1 of the original contentD) 0.01 of the original content

___ 119) A student was given four unknown solutions. Each solution was checked for conductivity and tested withphenolphthalein. The results are shown in the data table below.

Based on the data table, which unknown solution could be 0.1 M NaOH?A) A B) B C) C D) D

___ 120) A student tested a 0.1 M aqueous solution and made the following observations:

d conducts electricityd turns blue litmus to redd reacts with Zn(s) to produce gas bubbles

Which compound could be the solute in this solution?A) LiBr B) CH3OH C) HBr D) LiOH

___ 121) Which equation represents a neutralization reaction?A) NaCl + AgNO3 ‚ AgCl + NaNO3B) H2SO4 + Mg(OH)2 ‚ MgSO4 + 2H2O

C) Ni(NO3)2 + H2S ‚ NiS + 2HNO3D) Na2CO3 + CaCl2 ‚ 2NaCl + CaCO3

___ 122) Which chemical equation represents the reaction of an Arrhenius acid and an Arrhenius base?A) Zn(s) + 2HCl(aq) ‚ ZnCl2(aq) + H2(g)

B) C3H8(g) + 5O2(g) ‚ 3CO2(g) + 4H2O(l)

C) BaCl2(aq) + Na2SO4(aq) ‚ BaSO4(s) + 2NaCl(aq)

D) HC2H3O2(aq) + NaOH(aq) ‚ NaC2H3O2(aq) + H2O(l)

___ 123) Which compound could serve as a reactant in a neutralization reaction?A) CH3OH B) KOH C) NaCl D) CH3CHO

___ 124) If 5.0 milliliters of a 0.20 M HCl solution is required to neutralize exactly 10. milliliters of NaOH, what is the concentrationof the base?A) 0.20 M B) 0.30 M C) 0.10 M D) 0.40 M

___ 125) What volume of 0.500 M HNO3(aq) must completely react to neutralize 100.0 milliliters of 0.100 M KOH(aq)?

A) 50.0 mL B) 500. mL C) 10.0 mL D) 20.0 mL

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___ 126) A truck carrying concentrated nitric acid overturns and spills its contents. The acid drains into a nearby pond. The pH ofthe pond water was 8.0 before the spill. After the spill, the pond water is 1,000 times more acidic.

(a) What is the new pH of the pond water after the spill?

(b) What color would bromthymol blue be at this new pH?

___ 127) Calcium hydroxide is commonly known as agricultural lime and is used to adjust the soil pH. Before the lime was added toa field, the soil pH was 5. After the lime was added, the soil underwent a 100-fold decrease in hydronium ionconcentration.

What is the new pH of the soil in the field described?

___ 128) A student is given two beakers, each containing an equal amount of clear, odorless liquid. One solution is acidic and theother is basic.

(a) State two safe methods of distinguishing the acid solution from the base solution.

(b) For each method, state the results of both the testing of the acid solution and the testing of the base solution.

___ 129) Four flasks each contain 100 milliliters of aqueous solutions of equal concentrations at 25DC and 1 atm.

(a) Which solutions contain electrolytes?

(b) Which solution has the lowest pH?

(c) What causes some aqueous solutions to have a low pH?

(d) Which solution is most likely to react with an Arrhenius acid to form a salt and water?

(e) Which solution has the lowest freezing point? [Explain your answer.]

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Questions 130 through 132 refer to the following:

The graph below shows the relationship between pH value and hydronium ion concentration for common aqueous solutions andmixtures.

___ 130) According to the graph, what is the hydronium ion concentration of tomato juice?

___ 131) Based on the graph shown, what color is thymol blue when added to milk of magnesia?

___ 132) According to the graph, which mixture is approximately 100 times more acidic than milk of magnesia?

Questions 133 and 134 refer to the following:

In a titration experiment, a student uses a 1.4 M HBr(aq) solution and the indicator phenolphthalein to determine the concentration of aKOH(aq) solution. The data for trial 1 is recorded in the table below.

___ 133) Show a correct numerical setup for calculating the molarity of the KOH(aq) solution shown in the data table.

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___ 134) Why is it better to use several trials of a titration rather than one trial to determine the molarity of a solution of anunknown concentration?

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1) D 2) C 3) D 4) B 5) B

6) C 7) A 8) D 9) B 10) A

11) C 12) C 13) D 14) B 15) A

16) B 17) C 18) D 19) A 20) D

21) B 22) A 23) D 24) B 25) C

26) A 27) C 28) A 29) B 30) D

31) D 32) B 33) C 34) C 35) A

36) C 37) D 38) B 39) A 40) D

41) B 42) C 43) A 44) B 45) D

46) A 47) B 48) A 49) A 50) C

51) A 52) D 53) C 54) C 55) B

56) A 57) B 58) D 59) D 60) B

61) D 62) B 63) C 64) B 65) C

66) B 67) D 68) C 69) D 70) A

71) A 72) B 73) A 74) D 75) C

76) A 77) B 78) C 79) A 80) B

81) A 82) B 83) C 84) C 85) D

86) D 87) A 88) D 89) A 90) C

91) D 92) C 93) B 94) A 95) C

96) B 97) B 98) A 99) D 100) C

101) A 102) D 103) B 104) A

105) (a) HCl + KOH ‡‡ˆ KCl + H2O;(b) 80. mL

WORK SHOWN: MAVA = MBVB, (0.20 M)VA = (0.40 M)(40. mL), VA = 80. mL

106) (a) HNO3 + KOH ‡‡ˆ KNO3 + H2O;(b) 30. mL

WORK SHOWN: MAVA = MBVB, (1.5 M)(10. mL) = (0.50 M)(VB), VB = 30. mL

107) (a) HNO3 + LiOH ‡‡ˆ LiNO3 + H2O;(b) 0.25 M

WORK SHOWN: MAVA = MBVB, (MA)(100. mL) = (0.50 M)(50. mL), MA = 0.25 M;(c) phenolphthalein

108) (a) HNO3 + NaOH ‡‡ˆ NaNO3 + H2O;

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(b) 1.0 MWORK SHOWN: MAVA = MBVB, (3.0 M)(50. mL) = MB(150 mL), MB = 1.0 M

109) (a) HCl + NaOH ‡‡ˆ NaCl + H2O;(b) 0.50 M

WORK SHOWN: MAVA = MBVB, (1.0 M)(20. mL) = (MB)(40. mL), MB = 0.50 M

110) (a) HCl + NaOH ‡‡ˆ NaCl + H2O;(b) 5.0 M

WORK SHOWN: MAVA = MBVB, (MA)(10. mL) = (1.0 M)(50. mL), MA = 5.0 M

111) (a) HCl + LiOH ‡‡ˆ LiCl + H2O;(b) 50. mL

WORK SHOWN: MAVA = MBVB, (0.20 M)(25 mL) = (0.10 M)(VB), VA = 50. mL

112) (a) H2SO4 + 2NaOH ‡‡ˆ Na2SO4 + 2H2O;(b) 200. mL

WORK SHOWN: 2MAVA = MBVB, 2(1.00 M)(100. mL) = (1.00 M)(VB), VA = 200. mL

113) (a) HCl + NaOH ‡‡ˆ NaCl + H2O;(b) 0.25 M

WORK SHOWN: MAVA = MBVB, (0.50 M)(20.0 mL) = (MB)(40.0 mL), MB = 0.25 M;(c) pink;(d) neutralization

114) C 115) B 116) D 117) B 118) A

119) C 120) C 121) B 122) D 123) B

124) C 125) D

126) (a) 5; (b) yellow OR allow credit for a response consistent with student's answer to part (a)

127) 7

128) SAMPLE ANSWERS:(a) Test with an indicator OR use pH paper OR check for reactivity;(b) The base will turn phenolphthalein pink and the acid will not. OR The acid will turn blue litmus paper red and the base will

turn red litmus paper blue. OR Bromthymol blue will turn yellow in the acid and blue in the base. OR The acid will reactwith an active metal like magnesium and the base will not. OR The acid will have a pH less than 7 and the base will have apH greater than 7.

129) (a) KCl, Ba(OH)2, and CH3COOH;(b) CH3COOH;

(c) SAMPLE ANSWERS: They yield H+ (H3O+) in solution. OR They are acids. OR [H+] > [OH-];(d) Ba(OH)2;(e) Ba(OH)2

SAMPLE ANSWERS: It has the greatest number of particles dissolved. OR It dissociates into the greatest number ofparticles. OR It has the highest van't Hoff factor (i).

130) 10-4 M OR 0.0001 M

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131) blue

132) seawater

133) SAMPLE ANSWERS: OR (1.4 M)(15.40 mL) = MB(22.10 mL) OR (1.4)(15.40) = X(22.10)

134) SAMPLE ANSWERS: Multiple trials improve precision of results. OR to see if results are repeatable OR more trials, less error

Answer Key 4719 - 1 - Page 3