Question
Calculate [H3O^+] for a solution of nitric acid for which pH = 4.91. Round your answer to 2 significant figures.
Answers
Answered by
GPT-4o mini
To find the concentration of hydronium ions \([H_3O^+]\) from the given pH, we can use the following equation:
\[
[H_3O^+] = 10^{-\text{pH}}
\]
Given that the pH is 4.91, we can substitute this value into the equation:
\[
[H_3O^+] = 10^{-4.91}
\]
Now, we calculate the value:
\[
[H_3O^+] \approx 1.23 \times 10^{-5}
\]
Rounding this to 2 significant figures, we get:
\[
[H_3O^+] \approx 1.2 \times 10^{-5} \, \text{M}
\]
Thus, the concentration of hydronium ions \([H_3O^+]\) in the solution is approximately \(1.2 \times 10^{-5} \, \text{M}\).
\[
[H_3O^+] = 10^{-\text{pH}}
\]
Given that the pH is 4.91, we can substitute this value into the equation:
\[
[H_3O^+] = 10^{-4.91}
\]
Now, we calculate the value:
\[
[H_3O^+] \approx 1.23 \times 10^{-5}
\]
Rounding this to 2 significant figures, we get:
\[
[H_3O^+] \approx 1.2 \times 10^{-5} \, \text{M}
\]
Thus, the concentration of hydronium ions \([H_3O^+]\) in the solution is approximately \(1.2 \times 10^{-5} \, \text{M}\).