The boiling point of water is 100.0°C at 1 atmosphere. How many grams of aluminum chloride (133.3 g/mol), must be dissolved in 253.0 grams of water to raise the boiling point by 0.450 °C? Refer to the table for the necessary boiling or freezing point constant. Solvent Kb (°C/m) Kf(°C/m) Water H₂O 0.512 Ethanol CH3 CH ₂ OH 1.22 Chloroform CHC13 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 g aluminum chloride Mass= Formula 1.86 1.99 5.12

The boiling point of water is 100.00 °C at 1 atmosphere. A student dissolves 11.57 grams of manganese(II) iodide, MnI, (308.7 g/mol), in 221.5 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kp (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH,OH 1.22 1.99 Chloroform CHCI3 3.67 Benzene 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is m. The boiling point of the solution is °C.

A certain liquid X has a normal freezing point of −6.30°C and a freezing point depression constant Kf=7.40·°C·kgmol−1. Calculate the freezing point of a solution made of 31.g of benzamide (C7H7NO) dissolved in 800.g of X. Round your answer to 2 significant digits.

The freezing point of water is 0.00 °C at 1 atmosphere. How many grams of iron(III) bromide (295.6 g/mol), must be dissolved in 227.0 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 Water Ethanol Formula H₂O 0.512 CH3 CH₂OH 1.22 Chloroform CHC13 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 Mass= K₁(°C/m) Kƒ(°C/m) g 1.86 1.99 5.12

The boiling point of water is 100.0°C at 1 atmosphere. How many grams of nickel(II) bromide (218.5 g/mol), must be dissolved in 275.0 grams of water to raise the boiling point by 0.400°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kp (°C/m) Kf (°C/m) Water H20 0.512 1.86 Ethanol CH3CH,OH 1.22 1.99 Chloroform CHCI3 3.67 Benzene 2.53 5.12 Diethyl ether CH;CH,OCH2CH3 2.02 g nickel(II) bromide.

Calculate the molality of a solution formed by adding 3.159 g of methanol (CH3OH) to 100.00 mL of water. The density of water is 0.9982 g/mL. DO not include units. The lattice energy for KF is 821 kJ/mol. The enthalpy of hydration for K+ is -336 kJ/mol and the enthalpy of hydration for F- is -431 kJ/mol. What is the enthalpy in kJ when 14.91 g of KF forms an aqueous solution? (Hint: start by finding the enthalpy of solution)

Determine the freezing point of a solution consisting of 0.350 m KCl in water. The freezing point depression constant, Kf, of water is 1.86 °C/m. Freezing temperature of water is 0.00°C. Assume 100% dissociation of KCl.

You are analyzing 100 g of a solution that contains 12.5 g of the ionic compound KBr (MM = 119.0 g/mol) in water.  Here is some useful information:  KFP of water is 1.86 °C/m; KBP for water is 0.512 °C/m.  The density of the solution is 1.094 g/mL. Calculate the boiling point of this solution (bp of water is 100.0°C).   Calculate the osmotic pressure (in atm) of this solution at 25°C.

A 83.5 g sample of a nonelectrolyte is dissolved in 206.1 g of water. The solution is determined to have a boiling point of 102.3 °C. What is the molar mass of the compound? (Kb for water is 0.510 °C/m).

The names and chemical formulae of some chemical compounds are written in the first twa columns of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. Then, write down in the third column of the table the chemical formula of the major chemical species that will be present in this solution. For example, you know water itself will be present, so you can begin each list with the chemical formula for water (H,O).