colligative properties: freezing point depression. Gen chem 2 HINKI Acetic acid is known as a weak acid (electrolyte) when it is dissolved in water. A solution was prepared by dissolving acetic ac...
13. A 0.230 m solution of an unknown electrolyte depresses the freezing point of water by 0.821°C. What is the Van't Hoff factor for this electrolyte? The freezing point depression constant for water is 1.86 °C/m. a. 0.521 b. 1.92 c. 2.00 d. 2.30 e. 4.41
The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved in 45.0 g H, O, the freezing point is changed by -9.71 *C. Calculate the van't Hoff factor for Naci. Select one: O a. 1,00 . OOOO c. 1.83
1. What is the freezing point depression for the unknown solution for each trial? 2. How do you determine the van't Hoff factor for each trial, and what is the average van't Hoff factor? Trial 1: 18mL of 0.200 m unknown, ionic compound solution initial temp: 17.90 degrees C. observed freezing point of solution: -1.55 degrees C. Observed freezing point of water: -0.84 degrees C. Trial 2: 20 mL of 0.200 m unknown, ionic compound solution initial temp: 17.66 degrees...
2. A solution was prepared by dissolving 0.817g of a substance in 100.0g of acetic acid, HC2H302. The solution then froze at 14.50 degrees Celcium. Calculate the molecular weight of the substance. The freezing point for pure acetic acid is 16.60 °C. K = 3.59 C/m.
What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of in 115 g of water? [Use these Molar Masses: Ca = 40, N = 14, O = 16. Also, the molal freezing point depression constant for water is 1.86 °C/m.]
Colligative properties, such as boiling point elevation, depend on the number of dissolved particles in solution. For nonelectrolytes, no dissociation occurs, and so you can use the number of moles of solute to calculate both molality and molarity. In contrast, electrolytes dissociate, and therefore the molality and molarity must be calculated based on the number of moles of dissociated particles or ions. There are two ions per formula unit of NaCl. Therefore, we would expect the freezing-point depression ΔTf of...
When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the freezing point of the solution is -1.86o C. Given that the freezing point of pure water is 0o C and that the freezing-point depression constant for water is 1.86 o C/mol/kg, calculate the molecular mass (g/mol) of the unknown compound.
1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf = 0.777°C/m. What is the predicted freezing point (in °C) of a solution made from this solvent that is (1.90x10^0) m in a non-electrolyte solute? 1i. When (8.23x10^1) g of a non-electrolyte is dissolved in (5.2600x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the...
1 point What is the freezing point of an aqueous solution prepared by dissolving 113 g potassium carbonate (K,CO3, 138 g/mol) in 2.50 kg water. Use the ideal van 't Hoff factor. [K (water) - 1.86 °C/m) -1.83 °C +1.83 °C -0.609 °C -1.23 °C Previous Submit
A solute that conducts electricity when dissolved in water. a. colligative property b. electrolyte c. endothermic d. exothermic e. osmosis f. saturated solution g. solute h. solution i. solvent j. supersaturated solution A process where heat is released. a. colligative property b. electrolyte c. endothermic d. exothermic e. osmosis f. saturated solution g. solute h. solution i. solvent j. supersaturated solution