Calculate the molality of an aqueous solution of KBr whose freezing point is -4.95 degrees celsius. The Kf of water is 1.86 degrees C/m. Calculate the ideal Van't Hoff factor for KBr? Show work
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Calculate the molality of an aqueous solution of KBr whose freezing point is -4.95 degrees celsius....
An aqueous solution of a nonvolatile solute has a boiling point of 102.45 degrees Celsius. Knowing that for water, Kfp = 1.86 degrees Celsius m^-1 and Kbp= 0.51 degrees Celsius m^-1. What is the molality of the solution? and what is the freezing point of the solution? Please show work.
You have a aqueous solution of NaCl that has a freezing point of -9.35°C. Assuming a van't Hoff factor of 1.9 for NaCl, what is the mass percent of chloride ion in the solution? (Kf for water is 1.86°C kg/mol).
van't Hoff Factor Chem 202 Freezing Point of Aqueous Solutions Results Experimental freezing point values determined from graphs (sce directions on p. 3-5, steps 2,3): Sample Ty measured /°C AT measured / °C Distilled Water (solvent) -0.1°C Follow your instructor's Solution D (Naci) -1.8°C 1.7°C directions for submitting these values Solution G (lalla) -1.0°C 0.9°C before you leave lab! van't Hoff factor values (see directions on p. 3-6, steps 4-5): Solution D Solute Compound Naci Molality 0.505 mol/kg Ideal van't...
Calculate the molality and van't Hoff factor (i) for the following aqueous solution: 0.775 mass % KCl, freezing point = −0.364°C m = m KCl i =
Calculate the molality and van't Hoff factor (i) for the following aqueous solution: 2.460 mass % H2SO4, freezing point = −1.056°C m = m H2SO4? i = ?
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...
Calculate the change in the freezing point of an aqueous solution of 6.44 grams of glucose in 122 grams of water. The cryoscopic constant of water is 1.86 degrees centigrade / molality
2. What is the freezing point of an aqueous solution containing 69.5g NaNO3 (MM=85.00g/mol) dissolved in 175g water? Kf=1.86°C/m for water and assume "ideal" behavior. 10. An RV antifreeze is an aqueous solution containing 5.68 M proplyene glycol (MM=76.09 g/mol). If the density of the antifreeze is 1.080 g/mL, what is the molality of the solution?
The freezing point of a hypothetical liquid is -35 degrees C and its empirical freezing point constant is 2.5 K*kg/mol a) What is the freezing point of a 0.055 m glucose solution of this liquid? Show work b) Assuming complete dissociation of the salt, what is the freezing point of a 0.15 m MgCl2 solution of this liquid? Show work c) The freezing point of a 0.15m MgCl2 solution of this liquid is found to be -35.88 degrees C. What...
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