Calculate the molality of a 2.92 M potassium nitrate solution in which methanol, not water, is the solvent(!).  You might need some of these numbers: density of potassium nitrate (s) = 2.1 g/mL, density of pure methanol (l) = 0.79 g/mL, density of potassium nitrate (methanol) solution = 0.86 g/mL. concentration (mol/kg)

Moving to another question Wll tion 10 Calculate the molality of C2H5OH (molar mass = 46.068 g mol-1) in a water solution that is prepared by mixing 40.17 g of C2H5OH with 441.6 mL of H2U at 20 °C. (Density of water 1.00 g mL) (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) K Question 10 of 29 A Moving to another question will save this response. 211 * LO, %23 24 & 2. 3 8 delete 4 E R Y [O P ente S D F G K L. ret C- V alt alt option n command command option

A sucrose solution is prepared to a final concentration of 0.300 M . Convert this value into terms of g/L, molality, and mass %. (Use the following values: molecular weight MWsucrose = 352.296 g/mol ; density ρsol′n = 1.03 g/mL ; and mass of water, mwat = 961.5 g ). Note that the mass of solute is included in the density of the solution. -Express the concentrations in grams per liter, molality, and mass percent to three significant figures separated by commas.

(a) A 2.300 molal solution of KCl is prepared. How many grams of KCl are present in a sample containing 5.000 kg of water? (b) Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86°C/m and Kb = 0.512°C/m.