An acid that does not disassociate completely in solution, that is the protons are not donated completely in solution as a strong acid would be. Some weal acids only donate about 1% of their protons to the solution. They are weak conductors of electricity because of this characteristic.
To determine the pH of a weak acid, you can use a pH meter or pH indicator paper. Alternatively, you can calculate the pH using the concentration of the weak acid and its dissociation constant.
The pH of a weak acid depends on its concentration. A weak acid solution with a higher concentration will have a lower pH, while a lower concentration will result in a higher pH. The pH can be calculated using the acid dissociation constant (Ka) of the weak acid.
It's considered a dilute acid, not a weak acid. That term has a very specific meaning. A strong acid is one that ionizes (many chemistry texts use the word "dissociate") completely in water, and a weak acid is one that doesn't completely ionize. Hydrochloric acid is a "strong" acid; hydrofluoric acid is a "weak" acid even though it's more corrosive than hydrochloric acid is. So...you could take hydrochloric acid (a strong acid) and mix it with a lot of water, get it up to pH 6, and still have a strong acid.
i think a strong acid ionizes completely in water while a weak acid ionizes partiallly in water therefore the pH of a strong acid is greater than that of a weak acid The first part of your answer was correct, but the second was reversed. The pH of a strong acid is lower than the pH of a weak acid.
A weak acid typically has a pH below 7 but greater than 0, due to the partial dissociation of the acid in water. The exact pH value depends on the specific acid and its concentration.
To determine the pH of a weak acid, you can use a pH meter or pH indicator paper. Alternatively, you can calculate the pH using the concentration of the weak acid and its dissociation constant.
The pH of a weak acid depends on its concentration. A weak acid solution with a higher concentration will have a lower pH, while a lower concentration will result in a higher pH. The pH can be calculated using the acid dissociation constant (Ka) of the weak acid.
An acid is weak if it has a PH of seven or higher.
It's considered a dilute acid, not a weak acid. That term has a very specific meaning. A strong acid is one that ionizes (many chemistry texts use the word "dissociate") completely in water, and a weak acid is one that doesn't completely ionize. Hydrochloric acid is a "strong" acid; hydrofluoric acid is a "weak" acid even though it's more corrosive than hydrochloric acid is. So...you could take hydrochloric acid (a strong acid) and mix it with a lot of water, get it up to pH 6, and still have a strong acid.
i think a strong acid ionizes completely in water while a weak acid ionizes partiallly in water therefore the pH of a strong acid is greater than that of a weak acid The first part of your answer was correct, but the second was reversed. The pH of a strong acid is lower than the pH of a weak acid.
A weak acid typically has a pH below 7 but greater than 0, due to the partial dissociation of the acid in water. The exact pH value depends on the specific acid and its concentration.
Not very weak, it is a moderately weak acid.
A weak acid will partially ionize at pH 7, but the extent of ionization will depend on the specific weak acid and its equilibrium constant. The pH of a solution does not determine if a weak acid will ionize, but it can influence the degree of ionization based on the acid's pKa value.
Yes In theory, you could have a very weak solution of a strong acid and a stong solution of a weak acid and they would have the same pH.
6
A weak acid typically has a pH between 3 and 6. This is due to the partial dissociation of the weak acid molecules in water, resulting in a lower concentration of hydronium ions and a slightly acidic pH.
Usually a strong acid will produce a lower pH, but not always. pH is not a measure of the strength of an acid (or base) but the acidity of a solution, which is dependent on both the strength of the acid or base and its concentration in the solution.