At the beginning of this lesson, there was a question about two acids. Vinegar, which contains acetic acid, is used in foods and
has few safety concerns. Hydrochloric acid is used in chemistry labs and requires the use of safety goggles and gloves. Why do the safety concerns for these two acids differ?
Acetic acid is a weak acid and an organic compound and as such is not corrosive and therefore is acceptable to be used in food in the form of vinegar whereas hydrochloric acid is a strong mineral acid (partially derived from rock salt) and it is corrosive and from the author's experience it can be used in dilute form ie 10% by volume to react with limestone as a diagnostic test for that rock type (the limestone fizzes upon reaction with the dilute HCL.
Acetic acid is a weak acid, and hydrochloric acid is a strong acid.
As a weak acid, acetic acid does not dissociate much. As a strong acid, hydrochloric acid dissociates completely.
The stronger the acid, the more hydrogen ions will be in a solution at a given concentration.
Because they donate hydrogen ions, acids can react with other materials that accept hydrogen ions. A stronger acid will be more reactive than a weak acid at the same concentration.
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Boyle's Law is the pressure-volume law and it relates pressure and volume at constant temperature. Boyle's law states that pressure and volume vary inversely, meaning that as one goes up, the other one goes down.
