Let's find the hydrogen ion concentration [tex]\([\text{H}^+]\)[/tex] for each of the given solutions using the formula [tex]\(\left[ \text{H}^+\right]=10^{-\text{pH}}\)[/tex]. Here are the step-by-step calculations for the given acids:
1. Hydrochloric Acid (HCl):
- Given pH value: [tex]\( \text{pH} = 1 \)[/tex]
- Using the formula [tex]\(\left[ \text{H}^+\right]=10^{-\text{pH}}\)[/tex]:
[tex]\[
\left[\text{H}^+\right] = 10^{-1} = 0.1
\][/tex]
- Therefore, the hydrogen ion concentration for Hydrochloric acid is [tex]\(0.1\)[/tex] M.
2. Nitric Acid (HNO3):
- Given pH value: [tex]\( \text{pH} = 1 \)[/tex]
- Using the formula [tex]\(\left[ \text{H}^+\right]=10^{-\text{pH}}\)[/tex]:
[tex]\[
\left[\text{H}^+\right] = 10^{-1} = 0.1
\][/tex]
- Therefore, the hydrogen ion concentration for Nitric acid is [tex]\(0.1\)[/tex] M.
3. Acetic Acid (CH3COOH):
- Given pH value: [tex]\( \text{pH} = 4.75 \)[/tex]
- Using the formula [tex]\(\left[ \text{H}^+\right]=10^{-\text{pH}}\)[/tex]:
[tex]\[
\left[\text{H}^+\right] = 10^{-4.75} \approx 1.778 \times 10^{-5}
\][/tex]
- Therefore, the hydrogen ion concentration for Acetic acid is approximately [tex]\(1.778 \times 10^{-5}\)[/tex] M.
4. Formic Acid (HCOOH):
- Given pH value: [tex]\( \text{pH} = 3.75 \)[/tex]
- Using the formula [tex]\(\left[ \text{H}^+\right]=10^{-\text{pH}}\)[/tex]:
[tex]\[
\left[\text{H}^+\right] = 10^{-3.75} \approx 1.778 \times 10^{-4}
\][/tex]
- Therefore, the hydrogen ion concentration for Formic acid is approximately [tex]\(1.778 \times 10^{-4}\)[/tex] M.
Here is the hydrogen ion concentration in scientific notation for each solution:
[tex]\[
\begin{array}{|l|l|}
\hline
\text{Hydrochloric acid} & 0.1 \, \text{M} \\
\hline
\text{Nitric acid} & 0.1 \, \text{M} \\
\hline
\end{array}
\][/tex]
[tex]\[
\begin{array}{|l|l|}
\hline
\text{Acetic acid} & 1.778 \times 10^{-5} \, \text{M} \\
\hline
\text{Formic acid} & 1.778 \times 10^{-4} \, \text{M} \\
\hline
\end{array}
\][/tex]
