The pH of a 0.0642 M solution of a monoprotic acid is 3.86. s this a strong acid?
the answer is no,
can you explain why??
The pH is 3.86.
If the acid were a strong acid, it would be completely ionized and the (H) would be 0.0642. The pH would be pH = -log(0.0642) = 1.19. It is 3.86 which means the (H^+) is smaller so it isn't ionized completely.
To determine whether the acid is strong or weak, we need to understand the concept of pH and its relation to acid strength.
The pH scale measures the acidity or alkalinity of a solution. It ranges from 0 to 14, with 7 being neutral, values below 7 indicating acidity, and values above 7 indicating alkalinity.
In the case of acids, low pH values indicate high acidity. Strong acids completely ionize in water, releasing a high concentration of hydrogen ions (H+), resulting in a low pH. Whereas weak acids only partially dissociate, producing a lower concentration of H+ ions and resulting in a higher pH.
Given that the pH of the 0.0642 M solution of the monoprotic acid is 3.86, we can conclude that it is not a strong acid. A pH of 3.86 suggests that the solution has a moderate acidity but not as strong as a strong acid.
Therefore, the answer is no, the monoprotic acid in the given solution is not classified as a strong acid.