how do the colligative properties of the salt(s) effect the freezing point temperature
Depression
title: Freezing-point depression text: Freezing-point depression Freezing-point depression is the decrease of the freezing point of a solvent on addition of a non-volatile solute. Examples include salt in water, alcohol in water, or the mixing of two solids such as impurities into a finely powdered drug. In the last case, the added compound is the solute, and the original solid is thought of as the solvent. The resulting solution or solid–solid mixture has a lower freezing point than the pure solvent or solid. This phenomenon is what causes sea water, (a mixture of salt [and other things] in water) to remain liquid at temperatures title: Freezing-point depression text: parameters are available for many single salts. Freezing-point depression Freezing-point depression is the decrease of the freezing point of a solvent on addition of a non-volatile solute. Examples include salt in water, alcohol in water, or the mixing of two solids such as impurities into a finely powdered drug. In the last case, the added compound is the solute, and the original solid is thought of as the solvent. The resulting solution or solid–solid mixture has a lower freezing point than the pure solvent or solid. This phenomenon is what causes sea water, (a mixture of salt [and other things] title: Colligative properties text: pure solvent is lowered by the addition of a solute which is insoluble in the solid solvent, and the measurement of this difference is called "cryoscopy". It is found that Here "K" is the cryoscopic constant (equal to 1.86 °C kg/mol for the freezing point of water), "i" is the van 't Hoff factor, and "m" the molality. In the liquid solution, the solvent is diluted by the addition of a solute, so that fewer molecules are available to freeze. Re-establishment of equilibrium is achieved at a lower temperature at which the rate of freezing becomes equal to the rate title: Freezing-point depression text: a result of freezing-point depression, radiators do not freeze in winter (unless it is extremely cold, e.g. ). Road salting takes advantage of this effect to lower the freezing point of the ice it is placed on. Lowering the freezing point allows the street ice to melt at lower temperatures, preventing the accumulation of dangerous, slippery ice. Commonly used sodium chloride can depress the freezing point of water to about . If the road surface temperature is lower, NaCl becomes ineffective and other salts are used, such as calcium chloride, magnesium chloride or a mixture of many. These salts are title: Salt text: in water. When dissolved in water it separates into Na and Cl ions, and the solubility is 359 grams per litre. From cold solutions, salt crystallises as the dihydrate NaCl·2HO. Solutions of sodium chloride have very different properties from those of pure water; the freezing point is −21.12 °C (−6.02 °F) for 23.31 wt% of salt, and the boiling point of saturated salt solution is around 108.7 °C (227.7 °F). Salt is essential to the health of humans and other animals, and it is one of the five basic taste sensations. Salt is used in many cuisines around the world,