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

The normal freezing point of a certain liquid X is −9.10 °C, but when 8.7 g of potassium bromide (KBr) are dissolved in 100. g of X the solution freezes at - 12.2 °C instead. Use this information to calculate the molal freezing point depression constant K of X. Round your answer to 2 significant digits. K₁ = °C.kg mol x10 X

When 0.52 g of an unknown nonelectrolyte are dissolved in 35.0 g cyclohexane, the freezing point of the solution is 5.1ºC.  Pure cyclohexane freezes at 6.6ºC and has a Kf of 20.0ºC/m. What is the molar mass of the unknown in g/mol? Enter your answer with no decimal places (round to the nearest whole number). Do not include units. Do not worry about significant figures. Example: 2

A solution that contains 5.50 g of ferrocene [a non-electrolyte, molar mass = 186.0 g/mol] dissolved in 75.0 g of an unknown solvent has a freezing point of 3.11°C. The normal freezing point of the solvent is 4.90°C. What is the freezing point depression constant, kf, for this solvent?

A certain liquid X has a normal freezing point of -6.90 °C and a freezing point depression constant K=3.91 °C·kgmol . Calculate the freezing point of a solution made of 146.g of iron(III) chloride (FECI,) dissolved in 900. g of X. Round your answer to 3 significant digits.

A certain liquid X has a normal freezing point of -3.00 °C and a freezing point depression constant 2.24 °C.kg mol . A solution is prepared by dissolving some ammonium chloride (NH,Cl) in 450. g of X. This K=2 solution freezes at -4.2 °C. Calculate the mass of NH Cl that was dissolved, Be sure your answer is rounded to the correct number of significiant digits. Oxto S.

A student dissolves 1.3 g of resveratrol (C₁4H₁203) in 275. mL of a solvent with a density of 1.18 g/mL. The student notices that the volume of the solvent does not change when the resveratrol dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. molarity = molality = 0 x10 0x0 3

A solution of 4.63 g of anhydrous aluminum chloride (AlCl3) in 59.08 g of water freezes at -4.37 degrees celsius. Kf (AlCl3) =1.86 degrees celsius/m part 1: calculate the molar mass of AlCl3 from the formula. Round the answer to the hundredths place. ___ g/mol Part 2: Calculate the molar mass from the freezing point depression, assuming AlCl3 does not dissociate in ions. Round to 3 Significant digits. Part 3: Comparing the two values, how many ions will AlCl3 form? Round the answer to the nearest whole number.

What volume of ethylene glycol (C2 H, O2), a nonelectolyte, must be added to 18.0 L water to produce an antifreeze solution with a freezing point of –19.0°C? (The density of ethylene glycol is 1.11 g/cm, and the density of water is 1.00 g/cm ) Volume = | L What is the boiling point of this solution? Boiling point = | °C

Calculate the molality of each of the following aqueous solutions. Part 1 of 2 2.80 M NaCl (density of solution Part 2 of 2 m x10 m X x10 - X 1.08 51.7 percent by mass KBr solution. Round your answer to 3 significant digits. Ś g −). Round your answer to 2 significant digits. mL Ś