To find the hydrogen ion concentration, denoted as [tex]\(\left[ H^+ \right]\)[/tex], given the pH of a solution is 11.3, we can use the relationship between pH and [tex]\(\left[ H^+ \right]\)[/tex]. The pH of a solution is the negative logarithm (base 10) of the hydrogen ion concentration:
[tex]\[ \text{pH} = -\log \left[ H^+ \right] \][/tex]
Rearranging this equation to solve for [tex]\(\left[ H^+ \right]\)[/tex] gives:
[tex]\[ \left[ H^+ \right] = 10^{-\text{pH}} \][/tex]
Given the pH is 11.3, we have:
[tex]\[ \left[ H^+ \right] = 10^{-11.3} \][/tex]
To express this in scientific notation, we find that:
[tex]\[ 10^{-11.3} = 5.011872336272715 \times 10^{-12} \][/tex]
Therefore, the hydrogen ion concentration [tex]\(\left[ H^+ \right]\)[/tex] can be expressed as:
[tex]\[ \left[ H^+ \right] = 5.011872336272715 \times 10^{-12} \][/tex]
So [tex]\(\left[ H^+ \right]\)[/tex] is approximately [tex]\(5.011872336272715 \times 10^{-12} \, \text{M}\)[/tex], where the coefficient is 5.011872336272715, and the exponent is -12.
