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• ### Enter your answer in the provided box. The formula that governs the depression of freezing point...

Enter your answer in the provided box. The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: where:AT = the temperature change between a pure solvent and its solution i = the number of species per mole of solute that are dissolved in the solvent (e.g., i = 1 for a non-ionic solute that does not break apart into ions, i = 2 for...

• ### solve please. Enter your answer in the provided box. The formula that governs the depression of...

solve please. Enter your answer in the provided box. The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: AT=ix ky Xm Book where: AT = the temperature change between a pure solvent and its solution erences i = the number of species per mole of solute that are dissolved in the solvent (e.g., i=1 for a non-ionic solute that does not break apart...

• ### 1.The presence of a dissolved nonvolatile solute in a solution causes the freezing point to be...

1.The presence of a dissolved nonvolatile solute in a solution causes the freezing point to be _____________ (raised, lowered) compared to that of the pure solvent. The change in freezing point of the solvent can be calculated using the equation: 2.The presence of a dissolved nonvolatile solute in a solution causes the boiling point to be _____________ (raised, lowered) compared to that of the pure solvent. The change in boiling point of the solvent can be calculated using the equation:...

• ### Enter your answer in the provided box. The formula that governs the concentration of gas dissolved...

Enter your answer in the provided box. The formula that governs the concentration of gas dissolved in a solvent based on its pressure is given by Henry's Law: C= KP Where: C = solubility of a gas at a fixed temperature (in mol/L, M) k= Henry's Law constant (in units of mol/L • atm) P = partial pressure of the gas (in units of atm) How many grams of carbon dioxide gas is dissolved in a 290-ml can of cola...

• ### 1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf...

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...

• ### The freezing point depression of a solution made by the addition of a nonionic unknown solute...

The freezing point depression of a solution made by the addition of a nonionic unknown solute to benzophenone was used to determine the molar mass of the unknown. Data was collected for a solution containing 500. g of benzophenone with 5.0 ml of the unknown solute added. The density of the unknown solute was 6.18 g/ml. The K_f of benzophenone is 9.8 degree C M^-1. The freezing point of the benzophenone was determined to be 7.19 degree C. The freezing...

• ### A Review Constants Periodic Table The changes in boiling point (AT) or freezing point (AT) in...

A Review Constants Periodic Table The changes in boiling point (AT) or freezing point (AT) in degrees Celsius from a pure solvent can be determined from the equations given here, respectively: AT) = m x K = moles of solute XK K. kilograms of solvent Since pure water boils at 100.00 °C, and since the addition of solute increases boiling point, the boiling point of an aqueous solution, Th, will be T - (100.00+AT) 'C Since pure water freezes at...

• ### Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute...

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...

• ### Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a...

Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a solution of 57.6 g ethylene glycol (C2H602) in 734 g H20. Kffor H20 is 1.86 °C kg/mol. °C -2.53 1 homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries A solution which contains 71.9 g of an unknown molecular compound in 363 g of water freezes at -3.85°C. What is the molar mass of the unknown? g/mol 1homework pts Submit Answer Tries 0/5 Molar...

• ### Molar mass determination by depression of freezing point lab I'm stuck on calculating the moles of...

Molar mass determination by depression of freezing point lab I'm stuck on calculating the moles of solute.. How do I calculate it? Also can u please check if I've done everything else correctly.. The data I collected: Measured freezing point of pure water: 0.0 degrees Celsius Actual mass of solute used: 10.12g Freezing point of solution (observed): -3.4 Celsius Mass of solution: 84.7g Freezing point of a Solution of liqud unknown Freezing point depression: Trial #1. 0.0℃ (-3.4°C)= 3.4℃ Molality...