Rubbing alcohol (Isopropanol) has a boiling point of 82.3 °C. A student experimentally measured the boiling temperature of a mixture of isopropanol and water to be less than 100 °C. He repeated the experiment but again it was less than 100 °C. Does his results look right to you? O a. Yes, boiling point elevation pertains only to non volatile solutes. O b. Yes. Boiling point elevation constant for isopropanol is low. O c. No, boiling point elevation occurs for all solutions. O d. Yes, boiling point depression occurs for all solutions. O e. No, boiling point elevation pertains only to ionic solutes.

Rubbing alcohol (Isopropanol) has a boiling point of 82.3 °C. A student experimentally measured the boiling temperature of a mixture of isopropanol and water to be less than 100 °C. He repeated the experiment but again it was less than 100 °C. Does his results look right to you? O a. Yes, boiling point elevation pertains only to non volatile solutes. O b. Yes. Boiling point elevation constant for isopropanol is low. O c. No, boiling point elevation occurs for all solutions. O d. Yes, boiling point depression occurs for all solutions. O e. No, boiling point elevation pertains only to ionic solutes.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

An aqueous solution contains 12.5% NaCl by mass. What mass of water (in grams) is contained in 2.5 L of the vapor above this solution at 55 °C? The vapor pressure of pure water at 55 °C is 118 torr. (Assume complete dissociation of NaCl.)
29.06 g butane, C4H10, is added to 225 g CCl4. Assume the components are nonvolatile and that the solution is ideal. The kb for CCl4 is 5.26 °C/m and the normal boiling point of CCl4 is 76.8 °C. What is the new boiling point of the solution? BP = [? ]°C Boiling Point (°C) Enter
12. Glycerin, C3H8O3, is a nonvolatile liquid. What is the vapor pressure of a solution made by adding glycerin to H₂O at 39.8°C such that the mole fraction of glycerin is 0.0873? The vapor pressure of pure water at 39.8°C is 54.74 torr. a. 50.0 torr b. 60.0 torr c. 4.76 torr d. 70.0 torr e. None of the above Page 6
10.Give one example in which a high concentration of a solute is beneficial and one example in which it is harmful 11. Many chemicals that are potentially toxic or harmful to the environment have maximum allowable concentration levels set by government legislation. (a) If the chemical is dangerous, should the limit be zero? (b) Is a zero level theoretically possible? (c) Is a zero-level measurable? (d) If a nonzero limit is set, in your opinion, how should this limit be chosen?
18) A solution is made by dissolving 0.840 moles of sodium hydroxide in 300.0 g of water. If the van't Hoff factor, i, for this particular concentration is 1.70, what is the expected freezing point of this solution? Kf = 1.86 °C m-1. A) +0.80°C B)-2.66°C C) -9.97°C D) -8.85°C E) +3.06°C 18)
1. Calculate the freezing point and normal boiling points of each of the following aqueous solutions. a. 2.63m acetic acid b. 33.0% by mass lactose, C12 H22 O11 c. 32.15 mL of ethylene glycol, C2 H6 O2 (d = 1.113 g/mL) in 624 mL of water (d = 1.00g/mL) 2. Estimate the freezing and normal boiling points of 0.25 m aqueous solutions of NH4NO3 and NiCl3
The normal boiling point of methanol is 64.7°C. A solution containing a nonvolatile solute dissolved in methanol has a vapor pressure of 670. torr at 64.7°C. What is the mole fraction of methanol in this solution? Mole fraction =
A solution is made using 16.7 percent by mass CH2Cl2 in CHCl3. At 30 °C, the vapor. pressure of pure CH2Cl2 is 490 mm Hg, and the vapor pressure of pure CHCl3 is 260 mm Hg. The normal boiling point of CHCl3 is 61.7 °C. What is the molality of CH2Cl2 in the solution?
Assume that you were assigned calcium nitrate in lab. The water in your test tube weighed 22.096 g. Following the procedure in the lab manual, you determined that freezing point of water is 0.24°C.You weighed out 1.080 g of salt and added it to the original test tube, then determined that the freezing point was -0.83°C. Based on these experimental parameters, calculate the van't Hoff factor for calcium nitrate. Report your answer with 3 places after the decimal. Note that these are made-up numbers, and do not reflect a true experiment.
In the lab, a student needs to determine the van't Hoff factor for a deicer in water. Using the same deicer, he prepares six solutions at different concentrations. The freezing point depression constant for water is 1.86°C/m. Identify the deicer used to prepare the solution. A. Magnesium chloride, MgCl2 B. Aluminum chloride, AlCl3 C. Potassium nitrate, KNO3 D. Sodium acetate, NaC2H3O2
An ethylene glycol solution contains 30.4 g of ethylene glycol (C2H6O2) in 94.4 mL of water. (Assume a density of 1.00 g/mL for water.) a. Determine the freezing point of the solution. b. Determine the boiling point of the solution.
1. Calculate the freezing point of a solution made by dissolving 3.60 g of NaCl in 75.0 g of H2O. Kf of water is 1.86oC/m. Use the formula of NaCl to determine the van't Hoff factor. Answer with 2 decimal places. 2. Calculate the boiling point of a solution made by dissolving 2.32 g of Na2SO4 in 79.2 g of H2O. Kb of water is 0.512oC/m. Use the formula of Na2SO4 to determine the van't Hoff factor. Answer with 1 decimal place. 3. The real van't Hoff factor is typically not the theoretical based on chemical formula. Calculate the van't Hoff factor for MgCl2 if freezing point of an aqueous solution of MgCl2 is -3.07oC. The MgCl2 solution was prepared by mixing 5.90 g of MgCl2 with 98.6 g of H2O. The Kf for H2O is 1.86oC/mol. Answer to 2 decimal places.