HA +H2O ---> A- +H3O+
In the equation is HA a strong acid?
The question states: Based on the picture and the equation beneath it, which of the following best describes chemical HA?
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There is this picture above with a magnifying glass (magnifying a 1L container). Below the picture, it lists the equation and these colored molecules on top.
HA is this dark gray molecule
H2O is light gray
A- is a blue molecule
H3O+ is this huge orange molecule
There are more H3O molecules than A- molecules. And you can't see any of the gray molecules.
And I know that the answer is not a weak acid so... I'm confused... The options are weak base, strong base, weak acid and strong acid.
It's confusing to me too. It points to a strong acid to me BUT not all of it fits.
If HA is a strong acid, then you should have no HA molecules on the right and that fits. You should have an equal number of H3O^+ ions and A^- ions.which doesn't fit. If you know it isn't a weak acid that points even stronger to strong acid. I would rule out a base because
HA + H2O ==> HAH^+ + OH^- would be the equation and from your description there are no different colors that would indicate the H2A^+. It MUST be an acid to get H3O^+.
I hesitate to answer because I don't know the context of the question.
GENERALLY, I see HA written for ionization constants and that usually is done in which HA is a weak acid. Strictly speaking, if HCl is written as HA, then the products are H3O^+ and A^-. If HA is a weak acid, the products are H3O^+ + A^- but there is some HA remaining. Confused? I hope not. I can be more specific if you tell me how this is used.
To determine whether HA is a strong acid, you can start by looking at the equation.
In the equation HA + H2O -> A- + H3O+, HA is the acid molecule that donates a proton (H+) to water (H2O). The result is the formation of the conjugate base A- and the hydronium ion (H3O+).
To assess whether HA is a strong acid, you can look at its tendency to dissociate or ionize completely in water. Strong acids are acids that completely dissociate into their ions in water, whereas weak acids only partially dissociate.
Therefore, to determine if HA is a strong acid, you will need to consult a reliable source or reference that provides information about the strengths of various acids. Various textbooks, online databases, or chemistry references can provide a list of strong and weak acids.
For instance, if you have access to a periodic table or an acid strength chart, you can locate HA and check its dissociation behavior. If HA is listed as a strong acid, it means it completely dissociates into its ions (A- and H+) in water. On the other hand, if HA is listed as a weak acid, it means it only partially dissociates in water, forming a small amount of A- and H3O+ ions.
It is essential to note that simply looking at the equation alone does not provide enough information to determine the strength of HA. Consulting reliable sources is crucial for accurate information about acid strengths.