14-10 Colloidal Mixtures

• There are more interionic attractions in solutes.

• The problems can be solved with a theory of electrolyte solutions.
• Each positive ion in a solution is surrounded by a cluster of cations and surrounded by a shell.

• The attraction or drag of the ion in the electric field reduces its mobility.
• The magnitudes of colligative properties are reduced.
• The type of calculations presented in Chapters 4 and 5 can be made with great accuracy.
• If concentrations are used, no calculations involving solution properties are 100% accurate.

• Activities are needed.

• Chapter 13 introduced activities.
• Their importance in chemical equilibrium will be discussed in more detail in Chapter 15.

• The sand settles to the food bottom of the container in a mixture of sand and water.
• The mixture can contain up to 40% industry.
• Many foods are for a long time because of the mass of SiO2 and the dispersion of the silica in the colloids.
• Much larger particles of silica are present, though they are still considerable research effort.

• The particles are of the same size if the dimensions are less than 1 nm.

• Even if the particles are visible under a microscope, they are ordinary, or macroscopic, size.

• When light passes through a true solution, no light can be seen by an observer.
• Light is dispersed in many directions and can be seen.
• Dust particles in a flashlight beam scattering light.

• The particles are spherical.

• Thin films are similar to an oil slick on water.

• The OH2 colloids are randomly coiled.

• The particles have a negative charge.

• The particles repel each other.

• There is a charge on the particles.
• Much larger particles do not adsorb on the surface of the semipermeable membrane, as suggested by Figure 14-28.
• The process is more in the immediate vicinity when carried out in an electric field.
• A human kidneys dialyzes blood, a colloidal mixture, to remove and the particle carries excess electrolytes produced by metabolism.
• Certain diseases can cause a negative charge.
• The fact that a machine outside of the body can function for the kidneys is illustrated here.

• Synthetic gems, blue rock salt, and Ruby glass cannot pass through the black diamond of the membrane.

• Sometimes it is necessary to make clay particles or other suspended materials in water purification.
• The water is usually treated with an appropriate electrolyte.
• Clay sols can be used to distribute pesticides and other organic substances in the environment.

• Solid and liquid particles are suspended.
• Sulfur oxides, nitrogen oxides, and ozone are some of the components of smog.

• The separation of complex mixtures, such as gasoline, can be accomplished using a technique known as chromatography.
• There are many variations of the technique, but they all take advantage of differences in the way different compounds interact with a common material.
• To find out more, you can go to the Focus On feature on the MasteringChemistry site.

• The component is used to separate the volatile components of a solution.

• The curves show the formation of azeotropes in the solution.
• Dilute solutions contain at a constant temperature and produce vapor of the same relatively small amounts of solute and concentrated solu composition as the liquid; they have boiling points that in tions, large amounts.

• The mass percent, volume percent, and rating of the two solutions of different concentration are expressed in the semipermeable membrane centrations.
• mole fraction pressure to the more concentrated solution is the more important factor in determining molarity.

• Section 14-6) is one such property.
• It is possible to identify an osmotic pressure with this approach.

• Most solutions are not ideal.

• The freezing-point depression and boiling-point elevation are colligative properties of a solvent.
• A solution with the maximum amount of practical applications.
• There are certain conditions under which a solution can be pre stants.

• The graphs of ligative properties of electrolyte solutions are more diffi solute than non electrolyte solutions.

• The most familiar phenomena are related to gas.

• It is possible to calculate the solution vapor ble for some unusual phenomena with the help ofoidal mixtures.
• Liquid-vapor equilibrium curves showing either encountered in a broad range of contexts, from fluids solution vapor pressures to pollutants in large air mass points as a function of solution composition.

• The molality of a solution is related to the freezing-point depression in Analyze Equation (14.5).
• The boiling point of the solution can be determined using an equation.

• 128.2 g C 10H8>mol.

• To find the boiling point of the solution is to first solve equation (14.5) for the molality of the solution.

• The molality at the boiling point is the same as at C/Tb.

• The mass of solution can be determined with four significant figures.
• The freezing point of the solution can be established with good accuracy.
• Only one part per hundred is valid for the freezing point depression.
• The actual precision of the calculated quantities is still less than one part per hundred, despite the fact that significant-figure rules permit three significant figures in the remainder of the calculation.
• The final estimate of the boiling point 180.63 degC2 seems reasonable since it required only two figures.
• We assume that the 0.211 m solution is close enough to ideal in behavior to make the equations applicable.

• Water and phenol are only partially miscible at temperatures below 66.8 degC.
• A phase consisting of 92.50% water and 7.50% phenol is obtained in a mixture of 50.0 g water and 50.0 g phenol.
• The water has a saturated solution of phenol in it.

• At a constant temperature of 25.00 degC, a current of dry air was passed through pure water and then through a drying tube, D1, followed by passage through 1.00 m sucrose and another drying tube, D2.

• There is a substance in the follow-up to the Vitamins C and E.

• Some vitamins are water-soluble and some are fat-soluble.

• 1-butanol is fat.
• Explain your reasoning by identifying which.

Would it hold 100 g H2O?

• A brine has 3.81% NaCl by mass.
• How many liters of solu is there?

• You are asked to prepare a large amount of AgNO3.

• A water sample has less chloro in it's solution than it does in the vol form.
• In the same solution, how many grams of CHCl3 would be?

• The density of water is 1.18 g> cm3 at 20 degrees.

• The molarity of CO2 in a liter of ocean water is 75% H3PO4 by mass and has a density of 1.57 g>mL.

• The ocean water has a density of 1027.

• A solution prepared by dissolving 2.65 g C6H4Cl2 in a density of 1.209 g>mL is 34.0% H3PO4 by mass.

• Refer to Figure 14-10 to determine the molality of unsaturated, or what mass of KClO4 can be crystal NH4Cl in a saturated solution at 40 degC.

• One way to recrystallize a solute from a solution is by changing the temperature.
• It is possible to evaporate 0.200 m.

• A solution of 20.0 g KO4 in 500.0 g of water is prepared at a temperature of 40 degrees.

• If the same time as the temperature is reduced from solution is supersaturated, then it is.

• O2(g) is dissolved in 1.00 L H2O.
• What will be Air has a volume of 9689 Ar.

• The molarity equivalent to 87.8 mL CO2(g), measured at 0 degC and of O2 in an aqueous solution at equilibrium with air at 1.00 atm, per 100 mL of water, can be determined using data from Exercise 43.
• The molarity of atmospheric pressure.
• The volume percent of CO2 in water that is at 20 degC and saturated with air at O2 in air is 20%.

• Methane and CH4 are the main components of natural gas.

• When natural gas becomes saturated with air, assume that it's at 20 degC.

• The mass of a gas is stated as Henry's law.

• The amount of O2 in water is 14.2.

• Henry's law states that a given quantity of liquid dissolved at 25 degC and 1.00 atm perature is expelled when water saturated with O2 is volume of gas at all pressures.

• The water has a Vapor Pressure of 23.8mmHg.

• The two solutions pictured are the same substance.
• The temperature and density of methanol are similar.

• Styrene, used in the manufacture of polystyrene plas tics, is made by the removal of hydrogen atoms from ethylbenzene.

• The mixture is separated by water.

• The vapor pressure of ethylbenzene is 182mmHg and that of styrene is 134mmHg.

• The vapor pressure is 62.0 mol % C6H6.

• A orates from solution is a benzene-toluene solution.

• The boiling pure toluene at 98.6 degC is 533mmHg.

• A 20% solution by mass of blood pressure should be verified.

• The flowers are dying because of what approximate pressure is required.

• The basis of these phenomena is explained.

• The mass of hemoglobin is 104 U.

• A 0.50 g sample of polyisobutylene (a poly mer used in synthetic rubber) in 100.0 mL of benzene 14.0 g glycerol in 17.2 g sucrose in solution has an osmotic pressure that supports a 55.2 mL solution.
• Adding 1.00 g of benzene, C6H6, to 80.00 g cyclohexane, point of 75.22 g benzene from 5.53 to 4.92 degC.

• The boiling point of water is 99.60 degrees.

• A compound is composed of 42.9% C, 2.4% H, 16.7% N, and 38.1% 100.068 degC.

• Cooks often add salt to the water.

• Some people say it helps the cooking process by freezing the point at which it starts.
• The molec is raising the boiling point of water.

• The water-soluble vitamins are important in difference.
• The must be added to a liter of water at 1 atm pressure if you have a deficiency in this vitamins.
• This is a typical with 59.0% C, 5.0% H, 22.9% N, and 13.1% O.

• An important test for the purity of an organic com zene, C6H5NO2 is to measure its melting point.
• If the point is between 5.7 to -1.4 degC.

• The freezing point of the ocean is lowered by 1.183 degrees.
• The molecule is 1.94 degC.

What would be in conifers, such as fir trees, if the ocean water consisted of 3.5% salt?

• NH3 conducts electric current weakly.
• It is the same for acetic acid.

• The gas solution conducts electric current very well.

• Four solutions of acetone are solution by mass.

• The solution has 109.2 g KOH>L.

• The solution density is low.
• The task is to find solutions.
• Prepare 0.250 m KOH by estimating the lowest freezing point to 100.0 mL of this solution.

• The term "proof" used to mean 130.0 g of water.

• gunpowder and set afire if the solution is cooled to 0 degC.

• If you have 2.50 L of a solution mum ethanol content for a positive test, that's 13.8%, by volume.
• mass became aware of the 50% solution.
• There is protection to -2.0 degC listed in the table.
• Do you have any data for the solutions of ethanol?

• When the density of pure ethanol is 0.79 g>mL, hydrogen chloride is not a gas.

• Comment on the effec is a common form of fatiguing acids.
• Commercial grades of stearic tiveness of fractional distillation contain palmitic acid as well.
• There are two xylenes separated by a 1.115 g.

• The solution's freezing point is found to be 5.072 degrees.

• The Kf for pure benzene is 5.12 and the freezing point is 5.533 degrees.

• The cooling system against freeze-up at different temper solutions A and B contains 2.50 g sucrose, C12H22O11.
• What are the compositions of 0 degF, 4 qt; -15 degF, 5 qt; -34 degF, 6 qt.

• The molality is not equal to the molarity.

• The amount of O2(g) in water is 28.31 mL under an O2(g) pressure of 1 atm.

• The temperature of N2(g) in water is over a liter.

• The atmosphere has 78.05% N2 and 20.95% O2 in it.

What is the surface area of a single cube?

• Liquid benzene has a density of 0.879 g> cm3 at 20 degrees.

• Plot a graph of density and volume.

• The structures of CuSO # 4 5 H2O are depicted.

• The concentration of Ar in the ocean is always mixed together.
• The Henry's law constant for Ar is 1.5.

• The solution has a volume of 810.0 mL.

• The barometric pressure is equal to the temperature.

• Table 12.5 has HCl given in it.

• The composition changes when the temperature in the container is less than the approximate temperature.

• The phase diagram shows a mixture of the two acids in an acid-base reaction.
• The normal boiling points of solutions of the azeotrope are sent by the red curve repre to determine a more precise value of the composition.

• The device is pictured with boiling solutions.

• Relative humidity within an enclosure begins to be stant by a solution containing xHCl.

• There is no change stance in the boiling of a pure liquid.
• The solution is placed on the platform in the container.

• Every year, oral rehydration therapy saves the lives of countless children worldwide who become severely dehydrated as a result of diarrhea.

• One definition of an isotonic solution is that it has the same osmotic pressure.
• If the material in the bottom compartment is sitting, the solution has a freezing point.

Use the freezing-point definition from part (a) to data for water from Table 12.5, and use the definition of show that an ORT solution containing 3.5 g NaCl, Raoult's law from page 660 and that of relative humid 1.5 g KCl, 2.9 g Na3

• 150.0 g H2O is brought to a temperature of 30 degrees.

• The solution is 0.010 M CH3OH.

• The test tube becomes cold.

• In a saturated solution at 25 degC and 1 bar, for the relationships among the various concentration units lowing solutes, which condition will increase solu presented in Section 14-2.

• CO2 have colligative properties and increase volume.