Question 1

In the Brønsted theory,both acids and bases are defined in terms of how substances lose or gain

Accepted Answer

A)  OH-. 
B)  H3O+. 
C)  H+. 
D)  Cl- 
A)  OH-. 
B)  H3O+. 
C)  H+. 
D)  Cl-

Question 2

What is the pKa of an acid with a Ka of 1.82 *10-5?

Accepted Answer

A)  4.74 
B)  (-4.74) 
C)  9.26 
D)  (-9.26) 
A)  4.74 
B)  (-4.74) 
C)  9.26 
D)  (-9.26)

Question 3

pH changes can be determined with a(n)___.

Accepted Answer

A)  pH meter 
B)  chemical indicator 
C)  indicating paper 
D)  all of the above 
A)  pH meter 
B)  chemical indicator 
C)  indicating paper 
D)  all of the above

Question 4

The reason pure water has a pH of 7 is that there is the same concentration of hydrogen and hydroxide ions on the self-ionization of water.

Accepted Answer

A) True 
 B)False

Question 5

Identify the Brønsted acid(s)in the reaction.
HIO3(aq)+ H2O (l)  
H3O+ (aq)+ IO3- (aq)

Accepted Answer

A)  HIO3 
B)  HIO3 and H3O+ 
C)  H2O 
D)  H2O and HIO3 
A)  HIO3 
B)  HIO3 and H3O+ 
C)  H2O 
D)  H2O and HIO3

Question 6

Which of the following is a weak acid?

Accepted Answer

A)  HNO3 
B)  HCl 
C)  H2CO3 
D)  H2SO4 
A)  HNO3 
B)  HCl 
C)  H2CO3 
D)  H2SO4

Question 7

The molar concentration of OH in a water solution is 1.0 *10-9.The pH of the solution is _____ .

Accepted Answer

A) 9.00 B) 5.00 C) > 9.00 D) < 5.00 A) 9.00 B) 5.00 C) > 9.00 D) < 5.00

Question 8

A solution for which [OH-] = 3.0 *10-10 is classified as _____ .

Accepted Answer

A)  acidic 
B)  basic 
C)  neutral 
D)  More than one response is correct. 
A)  acidic 
B)  basic 
C)  neutral 
D)  More than one response is correct.

Question 9

Sodium nitrate in water will produce a basic solution.

Accepted Answer

A) True 
 B)False

Question 10

Ammonium chloride in water will produce an acidic solution.

Accepted Answer

A) True 
 B)False

Question 11

A solution for which [H+] = 1.0 *10-3 will have a pH of _____ .

Accepted Answer

A)  5.00 
B)  3.00 
C)  (-5.00) 
D)  (-9.00) 
A)  5.00 
B)  3.00 
C)  (-5.00) 
D)  (-9.00)

Question 12

Solutions with a pH less than 7.00 are basic.

Accepted Answer

A) True 
 B)False

Question 13

Which of the following salts would produce a basic solution (pH higher than 7)upon being dissolved in pure,distilled water?

Accepted Answer

A)  NaCl 
B)  Na2CO3 
C)  Mg(NO3)2 
D)  NH4Cl 
A)  NaCl 
B)  Na2CO3 
C)  Mg(NO3)2 
D)  NH4Cl

Question 14

A solution has a pH of 8.72.What is the value of [H+]?

Accepted Answer

A)  5.2 * 10-6 
B)  1.9 *10-9 
C)  5.2* 10-8 
D)  1.9 * 10-5 
A)  5.2 * 10-6 
B)  1.9 *10-9 
C)  5.2* 10-8 
D)  1.9 * 10-5

Question 15

Consider the following list of pKa values for a series of acids.Which is the strongest acid?

Accepted Answer

A)  5.74 
B)  3.21 
C)  10.6 
D)  Cannot be determined. 
A)  5.74 
B)  3.21 
C)  10.6 
D)  Cannot be determined.

Question 16

The salt of a weak base with a weak base could behave as a buffer.

Accepted Answer

A) True 
 B)False

Question 17

When a solution of HNO3 is added to a solution of NaHCO3,the net ion equation for reaction that occurs is which of the following?

Accepted Answer

A) 
  
B) 
  
C) 
  
D) 
  
A) 
  
B) 
  
C) 
  
D)

Question 18

A 25.00 mL sample of hydrochloric acid solution,HCl,is titrated with 0.0512 M NaOH solution.The volume of NaOH solution required is 21.68 mL.What is the molarity of the HCl solution?

Accepted Answer

A)  0.0444 
B)  0.0590 
C)  0.0295 
D)  0.0148 
A)  0.0444 
B)  0.0590 
C)  0.0295 
D)  0.0148

Question 19

A 25.00 mL sample of H2SO4 acid solution requires 17.35 mL of 0.118 N base for titration.What is the normality of the acid solution?

Accepted Answer

A)  0.0819 N 
B)  0.164 N 
C)  0.0409 N 
D)  0.236 N 
A)  0.0819 N 
B)  0.164 N 
C)  0.0409 N 
D)  0.236 N

Question 20

A Brønsted base is a proton donor.

Accepted Answer

A) True 
 B)False

Exam 9: Acids,bases,and Salts

In the Brønsted theory,both acids and bases are defined in terms of how substances lose or gain

What is the pKa of an acid with a Ka of 1.82 *10-5?

pH changes can be determined with a(n)___.

The reason pure water has a pH of 7 is that there is the same concentration of hydrogen and hydroxide ions on the self-ionization of water.

Identify the Brønsted acid(s)in the reaction. HIO3(aq)+ H2O (l) H3O+ (aq)+ IO3- (aq)

Which of the following is a weak acid?

The molar concentration of OH in a water solution is 1.0 *10-9.The pH of the solution is _____ .

A solution for which [OH-] = 3.0 *10-10 is classified as _____ .

Sodium nitrate in water will produce a basic solution.

Ammonium chloride in water will produce an acidic solution.

A solution for which [H+] = 1.0 *10-3 will have a pH of _____ .

Solutions with a pH less than 7.00 are basic.

Which of the following salts would produce a basic solution (pH higher than 7)upon being dissolved in pure,distilled water?

A solution has a pH of 8.72.What is the value of [H+]?

Consider the following list of pKa values for a series of acids.Which is the strongest acid?

The salt of a weak base with a weak base could behave as a buffer.

When a solution of HNO3 is added to a solution of NaHCO3,the net ion equation for reaction that occurs is which of the following?

A 25.00 mL sample of hydrochloric acid solution,HCl,is titrated with 0.0512 M NaOH solution.The volume of NaOH solution required is 21.68 mL.What is the molarity of the HCl solution?

A 25.00 mL sample of H2SO4 acid solution requires 17.35 mL of 0.118 N base for titration.What is the normality of the acid solution?

A Brønsted base is a proton donor.

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What is the pK_a of an acid with a K_a of 1.82 *10^-5?

Identify the Brønsted acid(s)in the reaction. HIO₃(aq)+ H₂O (l) H₃O⁺ (aq)+ IO₃^- (aq)

The molar concentration of OH in a water solution is 1.0 *10^-⁹.The pH of the solution is _____ .

A solution for which [OH^-] = 3.0 *10^-¹⁰ is classified as _____ .

A solution for which [H⁺] = 1.0 *10^-³ will have a pH of _____ .

A solution has a pH of 8.72.What is the value of [H⁺]?

Consider the following list of pK_a values for a series of acids.Which is the strongest acid?

When a solution of HNO₃ is added to a solution of NaHCO₃,the net ion equation for reaction that occurs is which of the following?

A 25.00 mL sample of H₂SO₄ acid solution requires 17.35 mL of 0.118 N base for titration.What is the normality of the acid solution?