When 9.45 g of is added to 500 mL of water, its freezing point drops by 0.5°C. The dissociation constant of is . The value of x is (round off to the nearest integer). []

Question

When 9.45 g of  is added to 500 mL of water, its freezing point drops by 0.5°C. The dissociation constant of  is . The value of x is (round off to the nearest integer). []

Canvas Classes · Accepted Answer

Strategy:
 Calculate the van't Hoff factor from the freezing point depression, determine the degree of dissociation , and use the equilibrium expression for .

Step 1: Calculate molality ()
- Mass of .
- Molar Mass .
- .
- Solvent .

Step 2: Determine van't Hoff factor ()

Step 3: Calculate } \alpha 	ext{ and } Ka

Rounding to : .

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