How do you accurately measure the solubility of a solute?

To accurately measure the solubility of a solute, adding a known excess mass of solute to a fixed volume of water at room temperature is the correct method. This process allows for the establishment of an equilibrium where the maximum amount of solute that can dissolve is determined.

The key steps involved include ensuring that the solute is in excess, which means that some of it will remain undissolved, indicating that the system has reached saturation. By measuring how much solute has been added to the water and knowing the volume of the solvent, the solubility can be calculated based on the amount of solute that is able to dissolve in that given volume.

In contrast, using cold water or heating the water prior to dissolving the solute could lead to inaccuracies in measuring solubility. Cold water may not dissolve the solute efficiently, especially if the solute has better solubility at higher temperatures. Similarly, heating water could introduce variables such as increased kinetic energy, which also affects solubility. Lastly, using an excess amount of water without controlling the volume does not allow for precise calculations of solubility, making it less reliable for measurement. Therefore, the selected method of using a fixed volume of water at room