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- At 20°C, the solubility of potassium carbonate, K2CO3, is 110.3 g/100. mL of water. In the laboratory, a student mixes 215 g of K2CO3 with 175. g of H2O at a temperature of 20°C. (9.3) a) How much of the K2CO3 will dissolve? b) Is the solution saturated or unsaturated? c) What is the mass, in grams, of any solid K2CO3 left undissolved on the bottom of the container?(Q68) What mass (in grams) of ethylene glycol (C2H,O2) must be added to 1,312 grams of water to lower the freezing point to -1.70 °C? (3 sf)A) Potassium chloride is soluble in water. Calculate the molality (m) of a solution made by adding 10.00 g of potassium chloride to 200. g of water. (6 pts.) B) Calculate the freezing point of this solution.ΔTF = i x m x KFKF (water) = 1.86 °C/mFreezing point of water is 0.00 °C
- 4. (5 pts) When 0.258 g of a molecular compound, benzoic acid, was dissolved in 40.0 g of benzene, the freezing point of the solution was lowered to 5.23 °C. What is the molecular weight of the benzoic acid? Freezing point of pure benzene = 5.46 °Celsius Kf of benzene = 5.12 °C/molal27. What is the mole fraction of ascorbic acid, C6H8O6 , in a solution containing 80.5 g of ascorbic acid and 210 g of water? (6,8,6 are subscript)(Q60) Consider a solution in which 20.1 grams of scandium phosphate (SCPO4) has been added to 520 grams of water. What is the mole fraction of the solvent for this solution? (4 sf)
- 8. 9. 10. A solution is prepared by dissolving 27.0 g urea (NH2)2CO, in 150.0 g of water. Calculate the boiling point of the solution if the Kb of water is 0.50 °C kg/mol. What mass of glycerin (C3H8O3), a nonelectrolyte, must be dissolved in 200.0 g of water to give a solution with a freezing point of -1.50 °C? The Kf for water is 1.86 °C kg/mol. A 0.500 g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 2.50 atm at 25 °C. If each molecule of the solute dissociates into two particles (in this solvent), what is the molar mass of this solute?(10) Which of the following should have the largest Henry's law constant (kH) in water? A) Ne B) CO C) Br2 D) CH3CH3 E) CO2(Q59) What is the molality of a solution that contains 73.7 grams of strontium fluoride that has been added to and dissolves in 3.13 liters of water? The density of water is 1.00 kg/L. (3 sf)
- (Q65) Calculate the vapor pressure (in torr) at 30°C of a solution containing 155.1 grams of the nonelectrolyte glucose (C6H1206) dissolved in 821.4 grams of water. The vapor pressure of pure water at this temperature is 31.80 torr. (4 sf)The Normality of concentrated sulphuric acid is ---(when p% =96% , d = 1.84 g./ml) O 3.6 O 18.02 36.045. At 25 "C, you make a homogeneous solution of 90.9 g of dextrose in 100 mL of water. Is this solution saturated, unsaturated, or supersaturated (13.2)? Saturated 6. If you then cool this solution to 5 °C, and the solution remains homogeneous, would the solution then be saturated, unsaturated, or supersaturated (13.2)? Supersaturated 7. Is DSW a saturated, unsaturated, or supersaturated solution of dextrose in water (13.2)? 8. Calculate the mole fraction of water in the solution described in Q5. The density of pure water at 25 °C is 0.997 g mL (13.3). 9. Calculate the molality of a solution of DSW (13.3). 10. Calculate the molarity of a solution of D5W (13.3). 11. Calculate the osmotic pressure Il of the solution of D5W (13.4). 2. Calculate the osmotic pressure II of the solution of dextrose from Q5 (13.4). 3. What would happen to your patient's blood if you administered an IV containing a solution of dextrose in water from Q5 (13.4)? Be specific. The osmotic pressure of human blood…