In which solution (acidic, basic, neutral water, or doesn't matter) is sodium acetate most soluble?

acidic solution
Basic solution
neutral
doesn't matter

I already tried basic solution and got it wrong.

The acetate ion is hydrolyzed to give

C2H3O2^- + HOH ==> HC2H3O2 + OH^-
So adding acid will neutralize the OH^- on the right and make the reaction shift to the right. I think an acid solution is the correct answer.

To determine in which solution sodium acetate is most soluble, we need to consider its chemical properties. Sodium acetate is the sodium salt of acetic acid, and its solubility can be influenced by the pH of the solution.

In general, sodium acetate is more soluble in acidic solutions compared to basic solutions. This is because acetic acid is a weak acid, and its conjugate base (acetate ion) is more stable in acidic conditions.

Therefore, the correct answer is an acidic solution.

If you already attempted the basic solution and it was incorrect, it means that you have ruled out one option. Now, you can focus on analyzing the other options: neutral water and doesn't matter.

For neutral water, you should consider that water is neither acidic nor basic by itself, but it can contain various dissolved substances that may affect the solubility of sodium acetate. However, since sodium acetate is more soluble in acidic solutions, and neutral water is neither acidic nor basic, the solubility of sodium acetate might be lower in neutral water compared to an acidic solution.

Regarding the option "doesn't matter," this suggests that the solubility of sodium acetate would be similar regardless of the solution's pH. However, based on the properties of sodium acetate and its relationship with acetic acid, it is more likely that pH does matter.

With this information, we can deduce that the most plausible answer is an acidic solution, as sodium acetate is generally more soluble in such conditions.