Which solution will provide the LOWEST freezing point?Group of answer choices1.2 M NaCl1.0 M KCl1.0 M Na2CO32.0 M KI

The freezing point of a solution is determined by the colligative property of freezing point depression, which states that the freezing point of a solution is lower than that of the pure solvent. This property depends on the number of solute particles in solution, not their identity.

Here are the steps to determine which solution will have the lowest freezing point:

1. Identify the number of particles each solute will produce in solution. Sodium chloride (NaCl) and potassium iodide (KI) are both strong electrolytes and will each dissociate into two ions in solution (Na+ and Cl- for NaCl, K+ and I- for KI). Potassium chloride (KCl) will also dissociate into two ions (K+ and Cl-). Sodium carbonate (Na2CO3) is also a strong electrolyte and will dissociate into three ions (2 Na+ and CO3 2-).

2. Multiply the molarity of each solution by the number of particles produced to find the total concentration of particles in each solution. For NaCl, this is 1.2 M * 2 = 2.4. For KCl, this is 1.0 M * 2 = 2.0. For Na2CO3, this is 1.0 M * 3 = 3.0. For KI, this is 2.0 M * 2 = 4.0.

3. The solution with the highest total concentration of particles will have the lowest freezing point. In this case, that is the 2.0 M KI solution, with a total particle concentration of 4.0.