the same amount of substance was added to four beakers of water. the treatments were placed in the chart…

Answer:

The solubility of a gas in a liquid is directly proportional to the pressure and inversely proportional to the temperature. High - pressure (Solution W) and low - temperature (Solution X) conditions increase the solubility of a gas in a liquid. High - temperature (Solution Y) and low - pressure (Solution Z) conditions decrease the solubility. So, Solutions X and Z have lower solubility compared to Solutions W and Y. The correct answer is: Solutions X and Z have greater solubility than solutions W and Y is incorrect; Solutions Y and Z have greater solubility than solutions W and X is incorrect; Solutions W and Y have greater solubility than solutions X and Z is incorrect; Solutions W and Z have greater solubility than solutions X and Y is incorrect. There seems to be an error in the provided options as the correct relationship is that Solutions W and X (high pressure and low temperature) have greater solubility than Solutions Y and Z (high temperature and low pressure).

Explanation:

Step1: Recall solubility rules

Solubility of gas in liquid: $S\propto P$ (pressure) and $S\propto\frac{1}{T}$ (temperature).

Step2: Analyze each solution

Solution W (high pressure) - high solubility. Solution X (low temperature) - high solubility. Solution Y (high temperature) - low solubility. Solution Z (low pressure) - low solubility.

Step3: Evaluate options

None of the given options correctly describe the solubility relationships based on the rules.