Question

You are given a 1.00 molal solution of an unknown solute dissolved in water and told that you must determine if the solute is a strong electrolyte, a weak electrolyte, or a nonelectrolyte. On testing, you find that the freezing point of the solution is -2.05 degrees Celsius. Is this enough information to answer the question? The molal freezing point depression constant for water is 1.86 °C/m. O No, this is not enough information O Yes, the solute is a nonelectrolyte Yes, the solute is a weak electrolyte Yes, the solute is a strong electrolyte

Answer 1

Answer: Yes, the solute is a weak electrolyte

Step-by-step explanation:

Depression in freezing point is given by:

`\Delta T_f=i* K_f* m`

`\Delta T_f=T_f^0-T_f=(0-(-2.05))^0C=2.05^0C` = Depression in freezing point

i= vant hoff factor = ?

`K_f` = freezing point constant =
`1.86^0C/m`

m= molality

`\Delta T_f=i* K_f* m`

`2.05=i* 1.86* 1`

`i=1.10`

As i for non electrolytes is 1, the given compound must be an electrolyte and a weak electrolyte as the value is only slightly greater than 1.