A solution is prepared by adding 50.0 g of glucose (C,H120, molar mass 180.18 g/mole) into 250.0 g of water. What is the freezing point of this solution? Kf of water is 1.86 °C/m. O 2.55 °C O -2.06 °C O -2.55 °C O 2.06 °C O 105. 09 °C

A solution is made by dissolving 7.80 grams of MgCl2 in 420.0 mL of water. What is the freezing point of this solution (in °C)? Express you answer to 3 significant digits.   Density of water 1.00 g/mL Kf of water 1.86oC/m

A sample of an ionic solid is dissolved in 1.00 kg of water. The freezing point of the water is -0.01 °C. If three times the mass of ionic solid is dissolved in 1.00 kg of water and the resulting freezing point of the solution is -0.09 °C, which of the following would be possible formulas for the solid: MX, MX2, or MX3, where M represents a metal cation and X an anion with a 1- charge? Explain your reasoning.

The freezing point of water is 0.00 °C at 1 atmosphere. How many grams of cobalt(II) acetate (177.0 g/mol), must be dissolved in 245.0 grams of water to reduce the freezing point by 0.300 °C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Mass Water H₂O Ethanol CH3 CH₂OH 1.22 Chloroform CHC13 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 Kb (°C/m) Kf(°C/m) 0.512 g 1.86 1.99 5.12

What would be the theoretical freezing point of a solution made by dissolving 10.43 g of NiCl 2 in 365.0 g of water? The freezing point constant of water is 1.86 °C/molal. The molar mass of NiCl 2 is 129.5994 g/mol.     1.230 °C     1.506 °C     0.8128 °C     -1.230 °C     1.022 °C

Calculate the freezing point of a solution that contains 168.4 g of sucrose (table sugar) in 300. g of water. One mole of sucrose is 342 g. Kf for H2O = 1.86°C/m -0.185 oC -3.05 oC -0.558 oC -0.744 oC -1.24 oC

The freezing point of CCI4 is -22.3°C and the freezing point depression constant is 29.8 °C/m. If a solution of C5H12 in CCI4 freezes at -37.6°C, what is the molality of this solution? O 0.513 0.722 O 2.01 O 5.01 O 1.26

An aqueous solution has a normal boiling point of 103.5°C. What is the freezing point of this solution? For water Kb = 0.51°C/m and Kf = 1.86°C/m. O +13°C -3.5°C O-0,96°C +3.6°C -13°C

23. An ethylene glycol solution contains 28.3 g of ethylene glycol, C2H602 in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.

Which solution has the lowest freezing point? 0.10 moles of NaSO_4 in 1 kg of water 0.10 moles of KCl in 1 kg of water 0.10 moles of BaCl_2 in 1 kg of water 0.10 moles of glucose in 1 kg of water