A 0.95 m aqueous solution of an ionic compound with the formula MX has a freezing point of -3.0 °C. Calculate the van’t Hoff factor (i) for MX at this concentration.

Verified step by step guidance

1. <insert step 1> Determine the freezing point depression (\( \Delta T_f \)) using the formula \( \Delta T_f = T_f^0 - T_f \), where \( T_f^0 \) is the freezing point of pure water (0 °C) and \( T_f \) is the freezing point of the solution (-3.0 °C).>
2. <insert step 2> Use the formula for freezing point depression: \( \Delta T_f = i \cdot K_f \cdot m \), where \( K_f \) is the cryoscopic constant for water (1.86 °C/m) and \( m \) is the molality of the solution (0.95 m).>
3. <insert step 3> Rearrange the formula to solve for the van’t Hoff factor \( i \): \( i = \frac{\Delta T_f}{K_f \cdot m} \).>
4. <insert step 4> Substitute the known values into the equation: \( i = \frac{3.0}{1.86 \times 0.95} \).>
5. <insert step 5> Calculate the value of \( i \) to determine the van’t Hoff factor for the ionic compound MX.>