8. Please help is due in 30 mins, will rate, Thank you!
Answer:
Given that t
freezing point depression constant, Kf = 0.777 C/m
Normal freezing point = 39.8 degree centigrade
Concentration in molality = 1.42 × 100 = 1.42 m
So, (delta T) = Kf × m = 0.777 × 1.42 = 1.103
So, the freezing point is lowered by 1.103 degree centigrade.
So the predicted freezing point is = 39.8 - 1.103
= 38.69 degree centigrade.
8. Please help is due in 30 mins, will rate, Thank you! A certain pure solvent...
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...
9. Please help is due in 30 mins, will rate, Thank you! When (8.8800x10^1) g of a non-electrolyte is dissolved in (5.84x10^2) 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 molar mass (in g/mol) of the non- electrolyte solute?
A pure solvent freezes at 6.35 degrees Celsius and a pure solute freezes at 832.0 degrees Celsius. The molar mass of the solvent is 96.4 g/mol and the molar mass of the solute is 78.5 g/mol. The freezing point depression constant for the solvent is 6.33 degrees/m. A solution is made of 1.012 g of the solute and 15.280 g of the solvent, determine its freezing point in degrees Celsius.
10. Please help is due in 30 mins, will rate, Thank you! How many grams of Mg(NO3)2 (MM = 148.33 g/mol) would it take to lower the freezing point of (4.60x10^2) grams of water by 4.00°C? The freezing point depression constant of water is Kf = 1.86°C/m.
6. Please help is due in 30 mins, will rate, Thank you! At an unknown temperature a solution made of (6.550x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.21x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (4.080x10^1) g/mol.
3. Please help is due in 30 mins, will rate, Thank you! An aqueous solution has a molality of (2.610x10^-1) m. The density of the solution is (1.4100x10^0) g/mL and the solute has a molar mass of (1.68x10^2) g/mol. What is the mole fraction of solute of this solution?
The freezing point of 53.37 g of a pure solvent is measured to be 49.20 ºC. When 2.74 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 47.05 ºC. Answer the following questions ( the freezing point depression constant of the pure solvent is 7.83 ºC·kg solvent/mol solute). What is the molality of the solution? m How many moles of solute are present? mol...
The freezing point of 53.48 g of a pure solvent is measured to be 41.91 ºC. When 2.94 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 39.86 ºC. Answer the following questions ( the freezing point depression constant of the pure solvent is 7.33 ºC·kg solvent/mol solute). -What is the molality of the solution?___ m -How many moles of solute are present? ___mol...
4. Please help is due in 30 mins, will rate, Thank you! An aqueous solution has a mass percent of solute of (2.630x10^1)%. The density of the solution is (1.41x10^0) g/mL and the solute has a molar mass of (1.7000x10^2) g/mol. What is the molality of solute of this solution?
5. Please help is due in 30 mins, will rate, Thank you! An aqueous solution has a mole fraction of solute of (2.5200x10^-2). The density of the solution is (1.2100x10^0) g/mL and the solute has a molar mass of (9.44x10^1) g/mol. What is the Molarity of solute of this solution?