The effect of temperature on the solubility of salt in water is generally a direct relationship, meaning that as the temperature increases, the solubility of the salt also increases. This is because higher temperatures provide more energy to break the ionic bonds between the salt molecules and facilitate their dissolution in water.Experimental evidence to support this claim can be obtained by performing a simple solubility experiment. Here's a step-by-step guide to conducting the experiment:1. Prepare three beakers with equal volumes of water e.g., 100 mL each and label them as A, B, and C.2. Heat the water in beaker A to a low temperature e.g., 10C , the water in beaker B to a medium temperature e.g., 25C , and the water in beaker C to a high temperature e.g., 50C . Use a thermometer to ensure the desired temperatures are reached and maintained.3. Weigh out equal amounts of salt e.g., 5 grams for each beaker.4. Add the salt to each beaker and stir the solution until no more salt dissolves. Record the time it takes for the salt to dissolve in each beaker.5. If the salt completely dissolves in any of the beakers, add more salt in small increments e.g., 1 gram and continue stirring until no more salt dissolves.6. Record the total amount of salt dissolved in each beaker.7. Compare the solubility of the salt in each beaker. The beaker with the highest temperature should have the highest solubility, while the beaker with the lowest temperature should have the lowest solubility.This experiment demonstrates that the solubility of salt in water increases with increasing temperature. The higher temperature provides more energy to break the ionic bonds between the salt molecules, allowing more salt to dissolve in the water.