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 $\mathrm { pH } = - \log _ { 10 } \left[ \mathrm { H } ^ { + } \right]$ . 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.

Question

Quizplus · Accepted Answer

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.

Solution a Has a PH of 4 pH=−log⁡10[H+]\mathrm { pH } = - \log _ { 10 } \left[ \mathrm { H } ^ { + } \right]pH=−log10​[H+]

Solution a Has a PH of 4 $\mathrm { pH } = - \log _ { 10 } \left[ \mathrm { H } ^ { + } \right]$