IDNLearn.com provides a user-friendly platform for finding and sharing knowledge. Discover the information you need quickly and easily with our reliable and thorough Q&A platform.
Sagot :
To determine the approximate difference in the concentration of hydrogen ions between the two solutions, we follow these steps:
1. Understanding the pH formula:
The pH of a solution is given by the equation:
[tex]\[ pH = -\log [H^+] \][/tex]
where [tex]\([H^+]\)[/tex] is the concentration of hydrogen ions.
2. Calculate the concentration of hydrogen ions ([tex]\([H^+]\)[/tex]) for the basic solution:
Given that the pH of the basic solution is 11.2, we can calculate the concentration of hydrogen ions as follows:
[tex]\[ [H^+]_{\text{basic}} = 10^{-\text{pH}_{\text{basic}}} = 10^{-11.2} \approx 6.31 \times 10^{-12} \][/tex]
This is the concentration of hydrogen ions in the basic solution.
3. Calculate the concentration of hydrogen ions ([tex]\([H^+]\)[/tex]) for the acidic solution:
Given that the pH of the acidic solution is 2.4, we can calculate the concentration of hydrogen ions as follows:
[tex]\[ [H^+]_{\text{acidic}} = 10^{-\text{pH}_{\text{acidic}}} = 10^{-2.4} \approx 3.98 \times 10^{-3} \][/tex]
This is the concentration of hydrogen ions in the acidic solution.
4. Determine the difference in concentration:
The difference in the concentration of hydrogen ions between the acidic solution and the basic solution is given by comparing [tex]\([H^+]_{\text{acidic}}\)[/tex] and [tex]\([H^+]_{\text{basic}}\)[/tex]:
[tex]\[ \text{Difference} = \frac{[H^+]_{\text{acidic}}}{[H^+]_{\text{basic}}} = \frac{3.98 \times 10^{-3}}{6.31 \times 10^{-12}} \approx 6.31 \times 10^8 \][/tex]
5. Conclusion:
The approximate difference in the concentration of hydrogen ions between the two solutions is:
[tex]\[ 6.31 \times 10^8 \approx 630957344.4801924 \][/tex]
This is closest to the option:
[tex]\[ 1.6 \times 10^{11} \][/tex]
Hence, the correct answer is [tex]\(1.6 \times 10^{11}\)[/tex].
1. Understanding the pH formula:
The pH of a solution is given by the equation:
[tex]\[ pH = -\log [H^+] \][/tex]
where [tex]\([H^+]\)[/tex] is the concentration of hydrogen ions.
2. Calculate the concentration of hydrogen ions ([tex]\([H^+]\)[/tex]) for the basic solution:
Given that the pH of the basic solution is 11.2, we can calculate the concentration of hydrogen ions as follows:
[tex]\[ [H^+]_{\text{basic}} = 10^{-\text{pH}_{\text{basic}}} = 10^{-11.2} \approx 6.31 \times 10^{-12} \][/tex]
This is the concentration of hydrogen ions in the basic solution.
3. Calculate the concentration of hydrogen ions ([tex]\([H^+]\)[/tex]) for the acidic solution:
Given that the pH of the acidic solution is 2.4, we can calculate the concentration of hydrogen ions as follows:
[tex]\[ [H^+]_{\text{acidic}} = 10^{-\text{pH}_{\text{acidic}}} = 10^{-2.4} \approx 3.98 \times 10^{-3} \][/tex]
This is the concentration of hydrogen ions in the acidic solution.
4. Determine the difference in concentration:
The difference in the concentration of hydrogen ions between the acidic solution and the basic solution is given by comparing [tex]\([H^+]_{\text{acidic}}\)[/tex] and [tex]\([H^+]_{\text{basic}}\)[/tex]:
[tex]\[ \text{Difference} = \frac{[H^+]_{\text{acidic}}}{[H^+]_{\text{basic}}} = \frac{3.98 \times 10^{-3}}{6.31 \times 10^{-12}} \approx 6.31 \times 10^8 \][/tex]
5. Conclusion:
The approximate difference in the concentration of hydrogen ions between the two solutions is:
[tex]\[ 6.31 \times 10^8 \approx 630957344.4801924 \][/tex]
This is closest to the option:
[tex]\[ 1.6 \times 10^{11} \][/tex]
Hence, the correct answer is [tex]\(1.6 \times 10^{11}\)[/tex].
We appreciate every question and answer you provide. Keep engaging and finding the best solutions. This community is the perfect place to learn and grow together. Find precise solutions at IDNLearn.com. Thank you for trusting us with your queries, and we hope to see you again.