Question 1

Which species is the conjugate acid of HS-?

Accepted Answer

A) H2S 
B) S2- 
C) HSO2- 
D) H+ 
A) H2S 
B) S2- 
C) HSO2- 
D) H+

Question 2

The pH of an aqueous solution of HCl labeled 0.015 M is ________.

Accepted Answer

The answer of The pH of an aqueous solution of...

Question 3

What are the products of the acid-base reaction of sodium carbonate with acetic acid?

Accepted Answer

A) CO2(g)+ H2O(l)+ 2 NaCH3COO(aq) 
B) 5 CO2(g)+ 2 H2O(l)+ 2 NaOH(aq) 
C) H2CO3(aq)+ H2O(l)+ 2 NaOH(aq) 
D) CO(g)+ H2O(l)+ 2 NaCH3COO(aq) 
A) CO2(g)+ H2O(l)+ 2 NaCH3COO(aq) 
B) 5 CO2(g)+ 2 H2O(l)+ 2 NaOH(aq) 
C) H2CO3(aq)+ H2O(l)+ 2 NaOH(aq) 
D) CO(g)+ H2O(l)+ 2 NaCH3COO(aq)

Question 4

The pH of a 1.0 × 10-6 M -OH solution is 6.00.

Accepted Answer

A) True 
 B)False

Question 5

Which solution has the lowest pH?

Accepted Answer

A) 1.3 × 10-8 M -OH 
B) 1.0 × 10-7 M -OH 
C) 5.1 × 10-2 M -OH 
D) 3.9 × 10-8 M -OH 
E) 2.3 × 10-3 M -OH 
A) 1.3 × 10-8 M -OH 
B) 1.0 × 10-7 M -OH 
C) 5.1 × 10-2 M -OH 
D) 3.9 × 10-8 M -OH 
E) 2.3 × 10-3 M -OH

Question 6

Which species can act as a Brønsted-Lowry base?

Accepted Answer

A) NO3- 
B) HBr 
C) H2CO3 
D) NH4+ 
A) NO3- 
B) HBr 
C) H2CO3 
D) NH4+

Question 7

The reaction of a Brønsted-Lowry acid (HA)with the metal salt of a hydroxide base (MOH)is an example of a neutralization reaction-an acid-base reaction that produces a ________ and ________ as products.

Accepted Answer

The answer of The reaction of a Brønsted-Lowry acid (HA)with...

Question 8

Which solution containing an equal number of moles of each of the substances is a buffer?

Accepted Answer

A) HCl and NaCl 
B) HNO2 and HNO3 
C) CH3COOH and NaCH3COO 
D) H2CO3 and CO32- 
E) More than one of the solutions is a buffer. 
A) HCl and NaCl 
B) HNO2 and HNO3 
C) CH3COOH and NaCH3COO 
D) H2CO3 and CO32- 
E) More than one of the solutions is a buffer.

Question 9

The stronger the acid,the (larger/smaller)________ the value of Ka.

Accepted Answer

Question 10

An aqueous solution of NaHCO3 is basic.

Accepted Answer

A) True 
 B)False

Question 11

The principal buffer in the blood is carbonic acid/bicarbonate (H2CO3/HCO3-),keeping the normal blood pH of a healthy individual in the range of 7.35 to 7.45.

Accepted Answer

A) True 
 B)False

Question 12

The addition of an acid to water increases the [H3O+] of the solution and increases the solution pH.

Accepted Answer

A) True 
 B)False

Question 13

Which species is a diprotic acid?

Accepted Answer

A) Mg(OH)2 
B) CH3COOH 
C) H2 
D) H2CO3 
A) Mg(OH)2 
B) CH3COOH 
C) H2 
D) H2CO3

Question 14

If two solutions differ in their [H3O+] by a factor of 2.0,the difference in their pH will be 2.0.

Accepted Answer

A) True 
 B)False

Question 15

Which acid is the weakest?

Accepted Answer

A) Hydrogen sulfate ion HSO4- (Ka = 1.2 × 10-2) 
B) Hydrocyanic acid HCN (Ka = 4.9 × 10-10) 
C) Hydrofluoric acid HF (Ka = 7.2 × 10-4) 
D) Ammonium ion NH4+ (Ka = 5.6 × 10-10) 
A) Hydrogen sulfate ion HSO4- (Ka = 1.2 × 10-2) 
B) Hydrocyanic acid HCN (Ka = 4.9 × 10-10) 
C) Hydrofluoric acid HF (Ka = 7.2 × 10-4) 
D) Ammonium ion NH4+ (Ka = 5.6 × 10-10)

Question 16

Which solution has the highest pH?

Accepted Answer

A) 4.3 × 10-8 M H3O+ 
B) 1.0 × 10-7 M H3O+ 
C) 5.1 × 10-2 M H3O+ 
D) 1.9 × 10-8 M H3O+ 
E) 1.0 × 10-2 M H3O+ 
A) 4.3 × 10-8 M H3O+ 
B) 1.0 × 10-7 M H3O+ 
C) 5.1 × 10-2 M H3O+ 
D) 1.9 × 10-8 M H3O+ 
E) 1.0 × 10-2 M H3O+

Question 17

A Brønsted-Lowry base must contain a lone pair of electrons.

Accepted Answer

A) True 
 B)False

Question 18

What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are needed to titrate a 25.0 mL sample of the acid according to the equation below? KOH(aq)+ HCl(aq)→ H2O(l)+ KCl(aq)

Accepted Answer

A) 0.218 M HCl 
B) 0.573 M HCl 
C) 0.0717 M HCl 
D) 4.58 M HCl 
E) 1.74 M HCl 
A) 0.218 M HCl 
B) 0.573 M HCl 
C) 0.0717 M HCl 
D) 4.58 M HCl 
E) 1.74 M HCl

Question 19

What is the net ionic equation for the acid-base reaction of hydrobromic acid with sodium hydroxide?

Accepted Answer

A) NaOH(aq)+ HBr(aq)→ H2O(l)+ NaBr(aq) 
B) Na+(aq)+ -OH(aq)+ H+(aq)+ Br-(aq)→ H2O(l)+ Na+(aq)+ Br-(aq) 
C) Na+(aq)+ -OH(aq)+ H+(aq)+ Br-(aq)→ H+(aq)+ -OH(aq)+ Na+(aq)+ Br-(aq) 
D) .-OH(aq)+ H+(aq)→ H2O(l) 
A) NaOH(aq)+ HBr(aq)→ H2O(l)+ NaBr(aq) 
B) Na+(aq)+ -OH(aq)+ H+(aq)+ Br-(aq)→ H2O(l)+ Na+(aq)+ Br-(aq) 
C) Na+(aq)+ -OH(aq)+ H+(aq)+ Br-(aq)→ H+(aq)+ -OH(aq)+ Na+(aq)+ Br-(aq) 
D) .-OH(aq)+ H+(aq)→ H2O(l)

Question 20

Which salt forms a basic solution when dissolved in water?

Accepted Answer

A) KCl 
B) NH4Br 
C) LiNO3 
D) Na3PO4 
A) KCl 
B) NH4Br 
C) LiNO3 
D) Na3PO4

Exam 9: Acids and Bases

Which species is the conjugate acid of HS-?

The pH of an aqueous solution of HCl labeled 0.015 M is ________.

What are the products of the acid-base reaction of sodium carbonate with acetic acid?

The pH of a 1.0 × 10-6 M -OH solution is 6.00.

Which solution has the lowest pH?

Which species can act as a Brønsted-Lowry base?

The reaction of a Brønsted-Lowry acid (HA)with the metal salt of a hydroxide base (MOH)is an example of a neutralization reaction-an acid-base reaction that produces a ________ and ________ as products.

Which solution containing an equal number of moles of each of the substances is a buffer?

The stronger the acid,the (larger/smaller)________ the value of Ka.

An aqueous solution of NaHCO3 is basic.

The principal buffer in the blood is carbonic acid/bicarbonate (H2CO3/HCO3-),keeping the normal blood pH of a healthy individual in the range of 7.35 to 7.45.

The addition of an acid to water increases the [H3O+] of the solution and increases the solution pH.

Which species is a diprotic acid?

If two solutions differ in their [H3O+] by a factor of 2.0,the difference in their pH will be 2.0.

Which acid is the weakest?

Which solution has the highest pH?

A Brønsted-Lowry base must contain a lone pair of electrons.

What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are needed to titrate a 25.0 mL sample of the acid according to the equation below? KOH(aq)+ HCl(aq)→ H2O(l)+ KCl(aq)

What is the net ionic equation for the acid-base reaction of hydrobromic acid with sodium hydroxide?

Which salt forms a basic solution when dissolved in water?

Matter and Measurement

Atoms and the Periodic Table

Ionic Compounds

Covalent Compounds

Chemical Reactions

Energy Changes,reaction Rates,and Equilibrium

Gases,liquids,and Solids

Solutions

Nuclear Chemistry

Introduction to Organic Molecules and Functional Groups

Alkanes

Unsaturated Hydrocarbons

Organic Compounds That Contain Oxygen,halogen,or Sulfur

The Three-Dimensional Shape of Molecules

Aldehydes and Ketones

Carboxylic Acids,esters,and Amides

Amines and Neurotransmitters

Lipids

Carbohydrates

Amino Acids,proteins,and Enzymes

Nucleic Acids and Protein Synthesis

Metabolism and Energy Production

Carbohydrate,lipid,and Protein Metabolism

Filters

Which species is the conjugate acid of HS^-?

The pH of a 1.0 × 10^-6 M ^-OH solution is 6.00.

The reaction of a Brønsted-Lowry acid (HA)with the metal salt of a hydroxide base (MOH)is an example of a neutralization reaction-an acid-base reaction that produces a and as products.

The stronger the acid,the (larger/smaller)________ the value of K_a.

An aqueous solution of NaHCO₃ is basic.

The principal buffer in the blood is carbonic acid/bicarbonate (H₂CO₃/HCO₃^-),keeping the normal blood pH of a healthy individual in the range of 7.35 to 7.45.

The addition of an acid to water increases the [H₃O⁺] of the solution and increases the solution pH.

If two solutions differ in their [H₃O⁺] by a factor of 2.0,the difference in their pH will be 2.0.

What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are needed to titrate a 25.0 mL sample of the acid according to the equation below? KOH(aq)+ HCl(aq)→ H₂O(l)+ KCl(aq)