a) If 1.95 mol of calcium chloride is added to 2.30 kg of water then what is the freezing point lowering and the freezing point of the solution (Kf = 1.86 ºC/m)?
b) If 0.500 mol of NaCl is added to 500 mL of water then what is the boiling point elevation and the boiling point of the solution (Kb = 0.52 ºC/m)?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
a) If 1.95 mol of calcium chloride is added to 2.30 kg of water then what...
Some ethylene glycol (OHCH2CH2OH) was added to your car's cooling system along with 5.0 kg of water.a. if the freezing point of the solution is -15.0 degrees celcius, what mass in grams of glycol must have been added? Kf(H2O)=1.86 degrees celcius kg mol^-1.b. What is the boiling point of the coolant mixture? Kb(H20) = 0.52 degrees celcius kg mol^-1.
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g of cyclohexane freezes at a temperature 9.50 ºC below the freezing point of pure cyclohexane. Calculate the molar freezing point depression constant, Kf, for cyclohexane. 2. The molar boiling point elevation constant for water is 0.512 ºC/m. What is the boiling point of a solution containing 673 g of water and 78.0 g of CaCl2? 3. A solution containing 32.0 g of an unknown...
4. Calculate the freezing point of a 0.5 m solution of calcium nitrate in water. Ca(NO₃)₂. (Kf = 1.86 °C kg/mol; Kb = 0.51 °C kg/mol)
Part 4. Molality of the calcium chloride solution Molality is defined as mol solute Calculate the molality of your assigned calcium chloride solution. Assume that the density of kg solvent water is 1g/mL. Questions (SHOW ALL WORK) 1. Calculate the molarity (M) of a solution when 12.80 g of glycerol (CHsOs) is added to 40.70 g of water. The density of the solution is 1,052g/ml Colligative properties like boiling point elevation depend on the number of solute particles in solution....
- Boiling point and Freezing point Elevation Calculate the boiling point and freezing points of water solutions that are 1.50 Min the KCl, a strong electrolyte. (the kb for water is 0.52", kf = 1.86)
The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 12.54 grams of chromium(II) acetate, Cr(CH3COO)2 (170.1 g/mol), in 158.2 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C....
6. Explain how you prepare the following dilute solution from more concentration.(Dilution) 5.00L of 6.00 M H2SO4 from a 18.0 M H2SO4 solution 7. 250 mL of 0.500 M CaCl2 from a 3.00 M CaCl2 solution.(Dilution) 8. Boiling point and Freezing point Elevation Calculate the boiling point and freezing points of water solutions that are 1.50 Min the KCl, a strong electrolyte. (the kb for water is 0.520, kf = 1.86)
Calculate the boiling point of a solution of CaCl2 in water. The freezing point depression of the same solution is -1.420 °C (kf = 1.86 °c/m, kb = 0.52°C/m).
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of 9.78% of ethylene glycol with a density of 1.0108 g/mL. The freezing point depression constant for water (solvent for all solutions) is Kf=-1.86 percent celsius kg/mol and the boiling point elevation constant is Kb=0.512 degrees celsius kg/mol. The density of neat water at 20.0 degrees celsius is 0.9982 g/mL. Answer the following: 1. What is the molarity of the solution? 2. What is the...
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water by calculating the freezing point depression of solutions containing 230. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is, it absorbs...