d) The following diagram shows how reverse osmosis works. One tank is charged with 0.50 M NaCl and the other tank is empty but it is separated by a semipermeable membrane that only allows water to p through. Pressure = ? 0.50 M NaCl Using the equation II = /MRT determine the pressure II that needs to be applied on the tank containin the NaCl solution to make reverse osmosis occur at 25 °C. The term i, the van't Hoff factor is the numb of particles made by dissolving NaCl in water, M is concentration in mol/L, R is the gas constant R (0.08 L*atm/K*mol) and K is temperature in K.

d) The following diagram shows how reverse osmosis works. One tank is charged with 0.50 M NaCl and the other tank is empty but it is separated by a semipermeable membrane that only allows water to p through. Pressure = ? 0.50 M NaCl Using the equation II = /MRT determine the pressure II that needs to be applied on the tank containin the NaCl solution to make reverse osmosis occur at 25 °C. The term i, the van't Hoff factor is the numb of particles made by dissolving NaCl in water, M is concentration in mol/L, R is the gas constant R (0.08 Latm/Kmol) and K is temperature in K.

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter8: Solutions

Section: Chapter Questions

Problem 8.5EP: For each of the following pairs of solutions, select the solution for which solute solubility is...

See similar textbooks

Similar questions

Define the terms in Raoults law. Figure 10-9 illustrates the net transfer of water molecules from pure water to an aqueous solution of a nonvolatile solute. Explain why eventually all of the water from the beaker of pure water will transfer to the aqueous solution. If the experiment illustrated in Fig. 10-9 was performed using a volatile solute, what would happen? How do you calculate the total vapor pressure when both the solute and solvent are volatile?
The dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 102 nm. (a) What are the volume (V=43r2) and surface area (A = r2) of each sphere? (b) How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters?
A solution is made by dissolving 0.455 g of PbBr2 in 100 g of H2O at 50C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.
A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
Consider two solutions, A and B, separated by an osmotic semipermeable membrane that allows only water to pass through, as shown in the diagram in Problem 8-113. Based on each of the following identities for solutions A and B, indicate whether the liquid level in compartment A, with time, will increase, decrease, or not change. a. A = 1.0 M glucose solution and B = 2.0 M glucose solution b. A = 5.0%(m/v) NaCl solution and B = 4.0%(m/v) NaCl solution c. A = 2.0 M Na2SO4 solution and B = 3.0 M KNO3 solution d. A = 2.0 M glucose solution and B = 1.0 M NaCl solution
Which solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium chloride (SrCl2) or 150.0 g of carbon tetrachloride (CCl4) ? Justify youranswer.
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 200. 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 moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
Consider 2 vapor pressure curves A and B. They are the vapor pressure curves of pure benzene and a contaminated solution of benzene with a nonvolatile solute. (a) Which graph shows the vapor pressure curve for pure benzene? (b) What is the boiling point of the contaminated benzene solution? (c) Estimate the molality of the contaminated solution (k b=2.53C/m).
Solutions Introduced directly into the bloodstream have to be isotonic with blood; that is, they must have the same osmotic pressure as blood. An aqueous NaCl solution has to be 0.90% by mass to be isotonic with blood. What is the molarity of the sodium ions in solution? Take the density of the solution to be 1.00 g/mL.
Distinguish between dispersion methods and condensation methods for preparing colloidal systems.
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C