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=−log10[H+]\mathrm { pH } = - \log _ { 10 } \left[ \mathrm { H } ^ { + } \right]pH=−log10[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.
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 TejedaAug 03, 2024
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.