How does one calculate the pH of a solution that is only 1.84% ionised?
determine the concentration of the H+, which will be in a monoprotic acid, concentration * decimal percent.
then determing pH in the normal way.
To calculate the pH of a solution that is only 1.84% ionized, you'll need to follow these steps:
1. Determine the concentration of H+ ions: Since the solution is only 1.84% ionized, it means that only 1.84% of the acid molecules have dissociated to produce H+ ions. Therefore, you'll need to find the concentration of H+ ions by multiplying the concentration of the acid by 1.84% (or 0.0184 as a decimal).
2. Determine the pH using the concentration of H+ ions: Once you have determined the concentration of H+ ions, you can calculate the pH using the formula:
pH = -log[H+]
Make sure to take the negative logarithm (base 10) of the concentration of H+ ions. This will give you the pH value of the solution.
So, to summarize:
1. Multiply the concentration of the acid by 1.84% to determine the concentration of H+ ions.
2. Take the negative logarithm of the concentration of H+ ions to find the pH value of the solution.