Question 1

What is the pH of 1×10 - 6 M HCl?

Accepted Answer

A)  6.00 
B)  6.98 
C)  7.98 
D)  8.00 
E)  need K a 
A)  6.00 
B)  6.98 
C)  7.98 
D)  8.00 
E)  need K a

Question 2

What is the base ionization constant , K b, for iodate, IO31 - , if the acid ionization constant of HIO3 equals 1.6×10 - 1?

Accepted Answer

A)  K b = 1.6×10 - 15 
B)  K b = 6.3×10 - 14 
C)  K b = 8.0×10 - 1 
D)  K b = 1.3×101 
E)  K b = 1.6×1013 
A)  K b = 1.6×10 - 15 
B)  K b = 6.3×10 - 14 
C)  K b = 8.0×10 - 1 
D)  K b = 1.3×101 
E)  K b = 1.6×1013

Question 3

Which aqueous solution listed below would have a pH = 1.00?
I. 0.10 M HBr (aq)
II. 0.10 M HOBr (aq)
III. 0.10 M NaBr (aq)

Accepted Answer

A)  I only 
B)  II only 
C)  I and II 
D)  I and III 
E)  All of these 
A)  I only 
B)  II only 
C)  I and II 
D)  I and III 
E)  All of these

Question 4

Employing a neutralization reaction , which reactants are used to prepare the salt Sodium cyanide, NaCN? reactants?
→NaCN

Accepted Answer

A)  NaCl and HCN 
B)  NaNO3 and HCN 
C)  NaCl and LiCN 
D)  Na, C, and N2 
E)  NaOH and HCN 
A)  NaCl and HCN 
B)  NaNO3 and HCN 
C)  NaCl and LiCN 
D)  Na, C, and N2 
E)  NaOH and HCN

Question 5

When comparing Bronsted-Lowery acid strengths , which one of the items listed below is falsely labeled?

Accepted Answer

A)  HBOS1U1B13S1U1B0S1U1P1 - 2S1S1P0 
B)  HIO < HClO 
C)  CHS1U1B14S1U1B0 < NHS1U1B13S1U1B0 
D)  HClOS1U1B13S1U1B0 < HClOS1U1B12S1U1B0 
E)  HCl < HBr 
A)  HBOS1U1B13S1U1B0S1U1P1 - 2S1S1P0 
B)  HIO < HClO 
C)  CHS1U1B14S1U1B0 < NHS1U1B13S1U1B0 
D)  HClOS1U1B13S1U1B0 < HClOS1U1B12S1U1B0 
E)  HCl < HBr

Question 6

The pH of a diet Coca Cola solution is 3.12. What is the concentration of [OH - ] present in this solution?

Accepted Answer

A)  [OH - ] = 1.3×10 - 25 M 
B)  [OH - ] = 7.6×10 - 18 M 
C)  [OH - ] = 1.3×10 - 11 M 
D)  [OH - ] = 7.6×10 - 4 M 
E)  [OH - ] = 7.6×1010 M 
A)  [OH - ] = 1.3×10 - 25 M 
B)  [OH - ] = 7.6×10 - 18 M 
C)  [OH - ] = 1.3×10 - 11 M 
D)  [OH - ] = 7.6×10 - 4 M 
E)  [OH - ] = 7.6×1010 M

Question 7

Acid strengths are measured and compared how?

Accepted Answer

A)  By measuring the concentration of the acid. 
B)  By measuring the pH of the aqueous solution. 
C)  By measuring the extent of ionization as determined by the reaction's K a. 
D)  By measuring how corrosive the acid is. 
E)  All of these. 
A)  By measuring the concentration of the acid. 
B)  By measuring the pH of the aqueous solution. 
C)  By measuring the extent of ionization as determined by the reaction's K a. 
D)  By measuring how corrosive the acid is. 
E)  All of these.

Question 8

Exhibit 15-4 Consider dissolving NaF in water as shown in the equation below to answer the following question(s):
NaF (s) + H₂ O (   )   HF (aq) + NaOH (aq)
-Refer to Exhibit 15-4. What is the molar concentration of hydroxide, OH - , if the initial concentration of NaF is 0.100 M?

Accepted Answer

A)  [OH - ] = 1.47×10 - 12 M 
B)  [OH - ] = 1.21×10 - 6 M 
C)  [OH - ] = 6.8×10 - 5 M 
D)  [OH - ] = 8.25×10 - 3 M 
E)  [OH - ] = 8.25×104 M 
A)  [OH - ] = 1.47×10 - 12 M 
B)  [OH - ] = 1.21×10 - 6 M 
C)  [OH - ] = 6.8×10 - 5 M 
D)  [OH - ] = 8.25×10 - 3 M 
E)  [OH - ] = 8.25×104 M

Question 9

What species are formed in the hydrolysis reaction of NH ₄Cl with water?
NH ₄Cl + H₂ O   ??

Accepted Answer

A)  N2 + H3O+ + H2 + Cl -  
B)  NH4+ + OH -  + Cl2 
C)  H3O+ + NH3 + Cl -  
D)  NH52+ + Cl -  + OH -  
E)  NH4+ + ClOH + H -  
A)  N2 + H3O+ + H2 + Cl -  
B)  NH4+ + OH -  + Cl2 
C)  H3O+ + NH3 + Cl -  
D)  NH52+ + Cl -  + OH -  
E)  NH4+ + ClOH + H -

Question 10

The weak acid HA dissociates with K a = 1.0×10 - 4. The pH of a 0.50 M solution of HA is:

Accepted Answer

A)  - 0.3 
B)  0.3 
C)  0.65 
D)  1.65 
E)  2.15 
A)  - 0.3 
B)  0.3 
C)  0.65 
D)  1.65 
E)  2.15

Question 11

Exhibit 15-4 Consider dissolving NaF in water as shown in the equation below to answer the following question(s):
NaF (s) + H₂ O (   )   HF (aq) + NaOH (aq)
-Refer to Exhibit 15-4. What is the base ionization constant , K b , for this reaction?
K a (HF) = 6.8 10 - 4

Accepted Answer

A)  K b = - 6.8×10 - 4 
B)  K b = 6.8×10 - 18 
C)  K b = 1.47×10 - 11 
D)  K b = 1.47×10 - 4 
E)  K b = 6.8×1010 
A)  K b = - 6.8×10 - 4 
B)  K b = 6.8×10 - 18 
C)  K b = 1.47×10 - 11 
D)  K b = 1.47×10 - 4 
E)  K b = 6.8×1010

Question 12

What is the pH of a solution prepared by dissolving 0.13 grams of HI (molar mass HI = 127.9 g/mol) in 300 mL of solution?

Accepted Answer

A)  5.48 
B)  2.47 
C)  0.37 
D)  3.37 
E)  not enough information is given 
A)  5.48 
B)  2.47 
C)  0.37 
D)  3.37 
E)  not enough information is given

Question 13

Which of the following salts is(are) considered acidic when dissolved in water?
I. [(CH3)2NH2]+Br - 
II. Na+CH3COO - 
III. LiCN

Accepted Answer

A)  I only 
B)  II only 
C)  I and II 
D)  I and III 
E)  II and III 
A)  I only 
B)  II only 
C)  I and II 
D)  I and III 
E)  II and III

Question 14

Which salt(s) listed below form(s) an acidic aqueous solution when dissolved in water?
I. NH4NO3
II. KCN
III. CH3COONa

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  I and II 
E)  All of these. 
A)  I only 
B)  II only 
C)  III only 
D)  I and II 
E)  All of these.

Question 15

Which substance in the reaction below behaves as a Lewis base ?
Ag 1+ (aq) + 2 NH₃(aq)   Ag(NH ₃) 2 1+ (aq)

Accepted Answer

A)  Ag1+ 
B)  NH3 
C)  [Ag(NH3)2]1+ 
D)  OH1 -  
E)  H2O 
A)  Ag1+ 
B)  NH3 
C)  [Ag(NH3)2]1+ 
D)  OH1 -  
E)  H2O

Question 16

A 0.20 M solution of the weak acid HA is found to have a pH of 3.25. What is the K a for this acid?

Accepted Answer

A)  10 - 3.25 
B)  3.2×10 - 6 
C)  0.12 
D)  1.6×10 - 6 
E)  3.2×10 - 7 
A)  10 - 3.25 
B)  3.2×10 - 6 
C)  0.12 
D)  1.6×10 - 6 
E)  3.2×10 - 7

Question 17

According to the definition of pH, what would be the pH of a 10 M solution of HCl?

Accepted Answer

A)  1 
B)  0 
C)  - 1 
D)  0.30 
E)  - 0.30 
A)  1 
B)  0 
C)  - 1 
D)  0.30 
E)  - 0.30

Question 18

Which of the following substances would not behave as a Lewis acid in the presence of H2O?

Accepted Answer

A)  Fe3+ 
B)  BF3 
C)  H+ 
D)  NH3 
E)  CO2 
A)  Fe3+ 
B)  BF3 
C)  H+ 
D)  NH3 
E)  CO2

Question 19

Two anions act as bases. Anion A -  has a stronger attraction for protons than does anion B - . Which statement best describes the acid-base character of these anions?

Accepted Answer

A)  A -  is a stronger base than B -  
B)  B -  is a stronger base than A -  
C)  A -  is a proton donor 
D)  B -  is an electron acceptor 
E)  A -  reacts with B -  
A)  A -  is a stronger base than B -  
B)  B -  is a stronger base than A -  
C)  A -  is a proton donor 
D)  B -  is an electron acceptor 
E)  A -  reacts with B -

Question 20

What is the H3O+ ion concentration in an aqueous solution having an OH -  concentration of 1.0×10 - 2 M?

Accepted Answer

A)  1.0×10 - 2 M 
B)  13×10 - 2 M 
C)  12×10 - 2 M 
D)  1.0×10 - 12 M 
E)  12×10 - 12 M 
A)  1.0×10 - 2 M 
B)  13×10 - 2 M 
C)  12×10 - 2 M 
D)  1.0×10 - 12 M 
E)  12×10 - 12 M

Exam 15: Solutions of Acids and Bases

What is the pH of 1×10 - 6 M HCl?

What is the base ionization constant , K b, for iodate, IO31 - , if the acid ionization constant of HIO3 equals 1.6×10 - 1?

Which aqueous solution listed below would have a pH = 1.00? I. 0.10 M HBr (aq) II. 0.10 M HOBr (aq) III. 0.10 M NaBr (aq)

Employing a neutralization reaction , which reactants are used to prepare the salt Sodium cyanide, NaCN? reactants? →NaCN

When comparing Bronsted-Lowery acid strengths , which one of the items listed below is falsely labeled?

The pH of a diet Coca Cola solution is 3.12. What is the concentration of [OH - ] present in this solution?

Acid strengths are measured and compared how?

Exhibit 15-4 Consider dissolving NaF in water as shown in the equation below to answer the following question(s): NaF (s) + H₂ O ( ) HF (aq) + NaOH (aq) -Refer to Exhibit 15-4. What is the molar concentration of hydroxide, OH - , if the initial concentration of NaF is 0.100 M?

What species are formed in the hydrolysis reaction of NH ₄Cl with water? NH ₄Cl + H₂ O ??

The weak acid HA dissociates with K a = 1.0×10 - 4. The pH of a 0.50 M solution of HA is:

Exhibit 15-4 Consider dissolving NaF in water as shown in the equation below to answer the following question(s): NaF (s) + H₂ O ( ) HF (aq) + NaOH (aq) -Refer to Exhibit 15-4. What is the base ionization constant , K b , for this reaction? K a (HF) = 6.8 10 - 4

What is the pH of a solution prepared by dissolving 0.13 grams of HI (molar mass HI = 127.9 g/mol) in 300 mL of solution?

Which of the following salts is(are) considered acidic when dissolved in water? I. [(CH3)2NH2]+Br - II. Na+CH3COO - III. LiCN

Which salt(s) listed below form(s) an acidic aqueous solution when dissolved in water? I. NH4NO3 II. KCN III. CH3COONa

Which substance in the reaction below behaves as a Lewis base ? Ag 1+ (aq) + 2 NH₃(aq) Ag(NH ₃) 2 1+ (aq)

A 0.20 M solution of the weak acid HA is found to have a pH of 3.25. What is the K a for this acid?

According to the definition of pH, what would be the pH of a 10 M solution of HCl?

Which of the following substances would not behave as a Lewis acid in the presence of H2O?

Two anions act as bases. Anion A - has a stronger attraction for protons than does anion B - . Which statement best describes the acid-base character of these anions?

What is the H3O+ ion concentration in an aqueous solution having an OH - concentration of 1.0×10 - 2 M?

Introduction to Chemistry

Atoms, Molecules, and Ions

Equations, the Mole, and Chemical Formulas

Chemical Reactions in Solution

Thermochemistry

The Gaseous State

Electronic Structure

The Periodic Table: Structure and Trends

Chemical Bonds

Molecular Structure and Bonding Theories

Liquids and Solids

Solutions

Chemical Kinetics

Chemical Equilibrium

Reactions Between Acids and Bases

Chemical Thermodynamics

Electrochemistry

Transition Metals, Coordination Chemistry and Metallurgy

The Chemistry of Hydrogen, Elements in Groups 3A Through 6A, and the Noble Gases

Nuclear Chemistry

Organic Chemistry and Biochemistry

Filters

What is the pH of 1×10^{- 6} M HCl?

What is the base ionization constant , K _b, for iodate, IO₃^{1 -}, if the acid ionization constant of HIO₃ equals 1.6×10^{- 1}?

The pH of a diet Coca Cola solution is 3.12. What is the concentration of [OH^-] present in this solution?

The weak acid HA dissociates with K _a = 1.0×10^{- 4}. The pH of a 0.50 M solution of HA is:

Which of the following salts is(are) considered acidic when dissolved in water? I. [(CH₃)₂NH₂]⁺Br^- II. Na⁺CH₃COO^- III. LiCN

Which salt(s) listed below form(s) an acidic aqueous solution when dissolved in water? I. NH₄NO₃ II. KCN III. CH₃COONa

A 0.20 M solution of the weak acid HA is found to have a pH of 3.25. What is the K _a for this acid?

Which of the following substances would not behave as a Lewis acid in the presence of H₂O?

Two anions act as bases. Anion A^- has a stronger attraction for protons than does anion B^-. Which statement best describes the acid-base character of these anions?

What is the H₃O⁺ ion concentration in an aqueous solution having an OH^- concentration of 1.0×10^{- 2} M?