How do temperature changes lead to solubility changes for salt dissolved in water?(1 point)

Question

Responses

High temperatures mean more of the salt will be in the liquid form as it gradually melts, increasing solubility.
High temperatures mean more of the salt will be in the liquid form as it gradually melts, increasing solubility.

High temperatures mean that sodium and chlorine ions will be moving faster, increasing the odds that they will collide and combine. This reduces solubility.
High temperatures mean that sodium and chlorine ions will be moving faster, increasing the odds that they will collide and combine. This reduces solubility.

High temperatures mean more kinetic energy, which keeps sodium and chlorine ions from combining, which increases solubility.
High temperatures mean more kinetic energy, which keeps sodium and chlorine ions from combining, which increases solubility.

High temperatures mean more of the salt will be in the gas form, causing it to evaporate out of the solution, decreasing solubility.
High temperatures mean more of the salt will be in the gas form, causing it to evaporate out of the solution, decreasing solubility.

Answer 1

The correct response regarding how temperature changes lead to solubility changes for salt dissolved in water is:

High temperatures mean sodium and chlorine ions will be moving faster, increasing the odds that they will collide and combine. This reduces solubility.

However, this statement is not completely accurate; warmer temperatures typically increase the solubility of most salts in water due to the increased kinetic energy of the particles, which helps break the ionic bonds in the salt and facilitates solvation by water molecules. Nevertheless, the response can be simplified to say that at higher temperatures, solubility generally increases for solid salts due to the increased movement of ions and water molecules enhancing interactions.

So in reality, you might expect a response like this but, as provided, the correct focus is on increased kinetic energy enhancing the process rather than reducing solubility.