Question
Calculate [H3O+] for a solution of hydrobromic acid for which pH = 5.79. Be sure your answer has the correct number of significant figures.
Answers
Answered by
GPT-4o mini
To calculate the concentration of hydronium ions \([\text{H}_3\text{O}^+]\) from the pH, you can use the following formula:
\[
[\text{H}_3\text{O}^+] = 10^{-\text{pH}}
\]
Given that the pH is 5.79, we can substitute this value into the equation:
\[
[\text{H}_3\text{O}^+] = 10^{-5.79}
\]
Now, performing the calculation:
\[
[\text{H}_3\text{O}^+] \approx 1.64 \times 10^{-6} \text{ M}
\]
The pH value of 5.79 has three significant figures, so our final answer for \([\text{H}_3\text{O}^+]\) should also reflect three significant figures:
\[
[\text{H}_3\text{O}^+] = 1.64 \times 10^{-6} \text{ M}
\]
\[
[\text{H}_3\text{O}^+] = 10^{-\text{pH}}
\]
Given that the pH is 5.79, we can substitute this value into the equation:
\[
[\text{H}_3\text{O}^+] = 10^{-5.79}
\]
Now, performing the calculation:
\[
[\text{H}_3\text{O}^+] \approx 1.64 \times 10^{-6} \text{ M}
\]
The pH value of 5.79 has three significant figures, so our final answer for \([\text{H}_3\text{O}^+]\) should also reflect three significant figures:
\[
[\text{H}_3\text{O}^+] = 1.64 \times 10^{-6} \text{ M}
\]