Question 1

Use the values of Ka in Table 9.5 in the text to identify the stronger acid in each of these pairs: A)HF and HNO₂ B)NH₄⁺ and HCO₃^- C)HCOOH and CH₃COOH

Accepted Answer

The answer of Use the values of Ka in Table...

Question 2

As pKa increases, the strength of the acid ________.

Accepted Answer

The answer of As pKa increases, the strength of the...

Question 3

Which of the following buffers is the one that is mainly contained in our blood?

Accepted Answer

A) HC2H3O2/C2H3O2- 
B) NH4+/NH3 
C) H2CO3/HCO3- 
D) HPO42-/PO43-

Question 4

What is the pH of a solution that has a [H3O+] = 1.2 × 10-3?

Accepted Answer

A) 1)20 
B) 2)92 
C) 11.08 
D) 12.80

Question 5

Indicate whether the following solutions are acidic, basic or neutral. For each concentration calculate the pH of the solution. A)[H⁺] = 1.1 × 10^-3 M B)[H⁺] = 6.0 × 10^-11 M

Accepted Answer

The answer of Indicate whether the following solutions are acidic,...

Question 6

What is the [H3O+] concentration of a solution that has a pH = 11.61?

Accepted Answer

A) 1)2 × 101 M 
B) 1)0 × 10-14 M 
C) 2)5 × 10-12 M 
D) 4)1 × 1011 M

Question 7

Which of the following is the strongest weak acid?

Accepted Answer

A) H2PO4- pKa = 7.18 
B) NH4+ pKa = 9.20 
C) HC2H3O2 pKa = 4.76 
D) HCO3- pKa = 10.32

Question 8

Which of the following is a weak acid?

Accepted Answer

A) H3PO4 
B) HNO3 
C) NH3 
D) OH-

Question 9

Which of the following cannot act as a Brønsted-Lowry acid?

Accepted Answer

A) HSO4- 
B) H2O 
C) CO32- 
D) HS-

Question 10

Insert the coefficients to balance this equation. ________ Na₂CO₃(s)+ ________ HNO₃(aq)→ ________ NaNO₃(aq)+ ________ H₂O(l)+ ________ CO₂(g)

Accepted Answer

The answer of Insert the coefficients to balance this equation.
________...

Question 11

Write the equation that shows how the weak base NH₃ produces OH^- ions in water.

Accepted Answer

The answer of Write the equation that shows how the...

Question 12

If the pI for a particular amino acid is 7.5, at which pH will the net charge on the molecule be zero?

Accepted Answer

A) 2)5 
B) 5)0 
C) 7)5 
D) 10.0

Question 13

The general expression for the equilibrium constant K is given by:

Accepted Answer

The answer of The general expression for the equilibrium constant...

Question 14

Which of the following properties is not characteristic of a base?

Accepted Answer

A) Has a bitter taste 
B) Produces H+ in water 
C) Has a slippery feel 
D) Is neutralized by an acid

Question 15

The form of an amino acid where the amine group is protonated and the carboxylic group exists an anion is called a ________.

Accepted Answer

The answer of The form of an amino acid where...

Question 16

Consider the weak acid HCO3- whose pKa = 10.32, which form will predominate when the pH of the solution is 12.00?

Accepted Answer

A) HCO3- 
B) CO32- 
C) H2CO3 
D) All of these

Question 17

Calculate the [H3O+] and the pH of a 0.021 M HNO3 solution.

Accepted Answer

A) 4)8 × 10-13 M and 12.32 
B) 4)8 × 10-13 M and -12.32 
C) 0)021 M and 1.68 
D) 0)021 M and -1.68

Question 18

In an acidic solution, pH is ________ and [H3O+] is ________.

Accepted Answer

A) = 7, 1 × 10-7 M 
B) > 7, -7 M 
C)  1 × 10-7 M 
D) -7 M

Question 19

In the following equation which is the proton donor and which is the proton acceptor?
CO32- (aq)+ H2O (l)? HCO3- (aq)+ OH- (aq)

Accepted Answer

A) Donor: CO32-; acceptor: H2O 
B) Donor: H2O; acceptor: CO32- 
C) Donor: HCO3-; acceptor: OH- 
D) Donor: OH-; acceptor: HCO3-

Question 20

What is the [H3O+] concentration of a solution that has a pH = 2.34?

Accepted Answer

A) 2)3 × 10-3 M 
B) 4)6 × 10-3 M 
C) 2)2 × 10-12 M 
D) 1)2 × 101 M

Exam 9: Acids, Bases, and Buffers in the Body

Use the values of Ka in Table 9.5 in the text to identify the stronger acid in each of these pairs: A)HF and HNO₂ B)NH₄⁺ and HCO₃^- C)HCOOH and CH₃COOH

As pKa increases, the strength of the acid ________.

Which of the following buffers is the one that is mainly contained in our blood?

What is the pH of a solution that has a [H₃O⁺] = 1.2 × 10^-3?

Indicate whether the following solutions are acidic, basic or neutral. For each concentration calculate the pH of the solution. A)[H⁺] = 1.1 × 10^-3 M B)[H⁺] = 6.0 × 10^-11 M

What is the [H₃O⁺] concentration of a solution that has a pH = 11.61?

Which of the following is the strongest weak acid?

Which of the following is a weak acid?

Which of the following cannot act as a Brønsted-Lowry acid?

Insert the coefficients to balance this equation. Na₂CO₃(s)+ HNO₃(aq)→ NaNO₃(aq)+ H₂O(l)+ CO₂(g)

Write the equation that shows how the weak base NH₃ produces OH^- ions in water.

If the pI for a particular amino acid is 7.5, at which pH will the net charge on the molecule be zero?

The general expression for the equilibrium constant K is given by:

Which of the following properties is not characteristic of a base?

The form of an amino acid where the amine group is protonated and the carboxylic group exists an anion is called a ________.

Consider the weak acid HCO₃^- whose pKa = 10.32, which form will predominate when the pH of the solution is 12.00?

Calculate the [H₃O⁺] and the pH of a 0.021 M HNO₃ solution.

In an acidic solution, pH is and [H₃O⁺] is .

In the following equation which is the proton donor and which is the proton acceptor? CO₃^2- (aq) + H₂O (l) ? HCO₃^- (aq) + OH^- (aq)

What is the [H₃O⁺] concentration of a solution that has a pH = 2.34?

Exam 9: Acids, Bases, and Buffers in the Body

Use the values of Ka in Table 9.5 in the text to identify the stronger acid in each of these pairs: A)HF and HNO2 B)NH4+ and HCO3- C)HCOOH and CH3COOH

As pKa increases, the strength of the acid ________.

Which of the following buffers is the one that is mainly contained in our blood?

What is the pH of a solution that has a [H3O+] = 1.2 × 10-3?

Indicate whether the following solutions are acidic, basic or neutral. For each concentration calculate the pH of the solution. A)[H+] = 1.1 × 10-3 M B)[H+] = 6.0 × 10-11 M

What is the [H3O+] concentration of a solution that has a pH = 11.61?

Which of the following is the strongest weak acid?

Which of the following is a weak acid?

Which of the following cannot act as a Brønsted-Lowry acid?

Insert the coefficients to balance this equation. ________ Na2CO3(s)+ ________ HNO3(aq)→ ________ NaNO3(aq)+ ________ H2O(l)+ ________ CO2(g)

Write the equation that shows how the weak base NH3 produces OH- ions in water.

If the pI for a particular amino acid is 7.5, at which pH will the net charge on the molecule be zero?

The general expression for the equilibrium constant K is given by:

Which of the following properties is not characteristic of a base?

The form of an amino acid where the amine group is protonated and the carboxylic group exists an anion is called a ________.

Consider the weak acid HCO3- whose pKa = 10.32, which form will predominate when the pH of the solution is 12.00?

Calculate the [H3O+] and the pH of a 0.021 M HNO3 solution.

In an acidic solution, pH is ________ and [H3O+] is ________.

In the following equation which is the proton donor and which is the proton acceptor? CO32- (aq) + H2O (l) ? HCO3- (aq) + OH- (aq)

What is the [H3O+] concentration of a solution that has a pH = 2.34?

Use the values of Ka in Table 9.5 in the text to identify the stronger acid in each of these pairs: A)HF and HNO₂ B)NH₄⁺ and HCO₃^- C)HCOOH and CH₃COOH

What is the pH of a solution that has a [H₃O⁺] = 1.2 × 10^-3?

Indicate whether the following solutions are acidic, basic or neutral. For each concentration calculate the pH of the solution. A)[H⁺] = 1.1 × 10^-3 M B)[H⁺] = 6.0 × 10^-11 M

What is the [H₃O⁺] concentration of a solution that has a pH = 11.61?

Insert the coefficients to balance this equation. Na₂CO₃(s)+ HNO₃(aq)→ NaNO₃(aq)+ H₂O(l)+ CO₂(g)

Write the equation that shows how the weak base NH₃ produces OH^- ions in water.

Consider the weak acid HCO₃^- whose pKa = 10.32, which form will predominate when the pH of the solution is 12.00?

Calculate the [H₃O⁺] and the pH of a 0.021 M HNO₃ solution.

In an acidic solution, pH is and [H₃O⁺] is .

In the following equation which is the proton donor and which is the proton acceptor? CO₃^2- (aq) + H₂O (l) ? HCO₃^- (aq) + OH^- (aq)

What is the [H₃O⁺] concentration of a solution that has a pH = 2.34?