The pH of a 0.0642 M solution of a monoprotic acid
is 3.86. Is this a strong acid?
figure the pH of a strong acid..
HX>>H + X
so pH= log (.0642)=1.2 which is considerably lower than 3.86. Probably not a strong acid. Lets look further.
work backwards.
concentration H= antilog 3.86
H=.00014
WEll, the acid is .00014/.0642 * 100 percent ionized, or .21 percent ionized.
check my work.
To determine if the acid is strong or weak, we need to compare the pH value to the pH values of strong acids and weak acids.
A strong acid is defined as an acid that completely ionizes in water, resulting in a high concentration of hydrogen ions (H+). Strong acids typically have a pH value less than 3.
A weak acid, on the other hand, only partially ionizes in water, leading to a lower concentration of hydrogen ions. Weak acids generally have a pH value greater than 3.
In this case, the pH of the solution is 3.86, which is greater than 3. This indicates that the acid is a weak acid rather than a strong acid.
To determine if a monoprotic acid is strong or weak, we need to compare the pH of its solution to the pH range of strong acids. The pH scale ranges from 0 to 14, with values below 7 considered acidic, 7 being neutral, and values above 7 being basic.
In this case, we are given that the pH of a 0.0642 M solution of a monoprotic acid is 3.86. To determine if the acid is strong or weak, we need to compare its pH to the range of strong acids. Strong acids typically have a pH value less than 3.
Since the pH of the acid solution is 3.86, which is greater than 3, we can conclude that this monoprotic acid is a weak acid rather than a strong acid.