Question

Solubility limit of CaCl₂⋅2H₂O in boiling water is 152 g CaCl₂⋅2H₂O in 100 g water. If you dissolved enough CaCl₂⋅2H₂O in water to reach this solubility limit, would the water boil if the water was initially 20°C?

Answer 1

Dissolving CaCl₂·2H₂O in water to its solubility limit will result in an elevated boiling point due to boiling point elevation. However, dissolving the substance in water at 20°C does not guarantee it will boil without additional heat.

Step-by-step explanation:

The question involves determining whether the water that has had enough CaCl₂·2H₂O dissolved in it to reach its solubility limit at boiling temperature would actually boil if the initial temperature of the water was 20°C. When the solubility limit of CaCl₂·2H₂O in boiling water is reached, which is 152 g in 100 g of water, we need to evaluate if the dissolution process will heat the water up to its boiling point. The normal boiling point of water is 100°C. Each mole of dissolved CaCl₂ will raise the boiling point of the solution by 0.51°C due to boiling point elevation, a colligative property. Since each CaCl₂ dissociates into three ions, the actual increase in boiling point would be higher than the given 0.51°C for a singular mole of solute. However, simply dissolving CaCl₂·2H₂O in water does not inherently ensure the water will reach the elevated boiling point if the initial temperature is significantly lower than 100°C.