Asked by Isaiah Estilien on Jul 29, 2024

Verified

Solution A has a pH of 4.9 and solution B has a pH of 8.8. The acidity (pH) is a measure of the hydrogen ion concentration H + (measured in moles of hydrogen per liter) of solution. Acidity is modeled by $pH=−g_{10}[H_{+}]$ . The hydrogen ion concentration of solution A is how many times the concentration of solution B.

A) The concentration of solution A is approximately 7,943 times the concentration of solution B.

B) The concentration of solution A is approximately 3.9 times the concentration of solution B.

C) The concentration of solution A is approximately 20 times the concentration of solution B.

D) The concentration of solution A is approximately 3.6 times the concentration of solution B.

E) The concentration of solution A is approximately 1.8 times the concentration of solution B.

A) The concentration of solution A is approximately 7,943 times the concentration of solution B.

B) The concentration of solution A is approximately 3.9 times the concentration of solution B.

C) The concentration of solution A is approximately 20 times the concentration of solution B.

D) The concentration of solution A is approximately 3.6 times the concentration of solution B.

E) The concentration of solution A is approximately 1.8 times the concentration of solution B.

Hydrogen Ion Concentration

A measure of the acidity or alkalinity of a solution, denoted by pH, which corresponds to the negative logarithm of the concentration of hydrogen ions in the solution.

pH

A measure of the acidity or alkalinity of an aqueous solution, ranging from 0 to 14.

- Understand the relationship between pH values, hydrogen ion concentrations, and their implications in solution acidity.

Verified Answer

MT

Marileidy Tejeda

2 days ago

Final Answer :

A

Explanation :

First, we need to calculate the hydrogen ion concentration (H+) of each solution using the pH value:

For Solution A:

pH = -log[H+]

4.9 = -log[H+]

log[H+] = -4.9

[H+] = 7.94 x 10^(-5) moles/L

For Solution B:

pH = -log[H+]

8.8 = -log[H+]

log[H+] = -8.8

[H+] = 1.58 x 10^(-9) moles/L

Now we can calculate the ratio of the hydrogen ion concentrations of Solution A and Solution B:

[H+]_A/[H+]_B = (7.94 x 10^(-5))/(1.58 x 10^(-9)) = 7.94 x 10^(-5 + 9) = 7.94 x 10^4

So the hydrogen ion concentration of Solution A is approximately 7,943 times the concentration of Solution B. Therefore, the correct choice is A.

For Solution A:

pH = -log[H+]

4.9 = -log[H+]

log[H+] = -4.9

[H+] = 7.94 x 10^(-5) moles/L

For Solution B:

pH = -log[H+]

8.8 = -log[H+]

log[H+] = -8.8

[H+] = 1.58 x 10^(-9) moles/L

Now we can calculate the ratio of the hydrogen ion concentrations of Solution A and Solution B:

[H+]_A/[H+]_B = (7.94 x 10^(-5))/(1.58 x 10^(-9)) = 7.94 x 10^(-5 + 9) = 7.94 x 10^4

So the hydrogen ion concentration of Solution A is approximately 7,943 times the concentration of Solution B. Therefore, the correct choice is A.

## Learning Objectives

- Understand the relationship between pH values, hydrogen ion concentrations, and their implications in solution acidity.