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43 Cards in this Set
- Front
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The process of solute particles being surrounded by solvent particles is known as a. salutation b. agglomeration c. solvation d. agglutination e. dehydration |
c. solvation |
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Pairs of liquids that will mix in all proportions are called _______ liquids. a. miscible b. unsaturated c. polar liquids d. saturated e. supersaturated |
a. miscible |
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Which of the following vitamins is water soluble? a. A b. B c. K d. D e. E |
b. B |
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The dissolution of water in octane (C8H18) is prevented by _______. a. London dispersion forces between octane molecules b. hydrogen bonding between water molecules c. dipole-dipole attraction between octane molecules d. ion-dipole attraction between water and octane molecules e. repulsion between like-charged water and octane molecules |
b. hydrogen bonding between water molecules |
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When argon is placed in a container of neon, the argon spontaneously disperses throughout the neon because ______. a. of the large attractive forces between argon and neon atoms b. of hydrogen bonding c. a decrease in energy occurs when the two mix d. the dispersion of argon atoms produces an increase in disorder e. of solvent-solute interactions |
d. the dispersion of argon atoms produces an increase in disorder |
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Hydration is a specific example of the phenomenon known generally as _______. a. salutation b. disordering c. solvation d. condensation e. dilution |
c. solvation |
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The dissolution of gases in water is virtually always exothermic because _______. a. one of the two endothermic steps (separation of solute particles) in the solution-formation process is unnecessary b. the exothermic step in the solution-formation process is unnecessary c. gases react exothermically with water d. neither of the two endothermic steps in the solution-formation process is necessary e. all three steps in the solution-formation process are exothermic |
a. one of the two endothermic steps (separation of solute particles) in the solution-formation process is unnecessary |
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Formation of solutions where the process is endothermic can be spontaneous provided that _______. a. they are accompanied by another process that is exothermic b. they are accompanied by an increase in order c. they are accompanied by an increase in disorder d. the solvent is a gas and the solute is a solid e. the solvent is water and the solute is a gas |
c. they are accompanied by an increase in disorder |
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The phrase "like dissolve like" refers to the fact that _____. a. gases can only dissolve other gases b. polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes c. solvents can only dissolve solutes of similar molar mass d. condensed phases can only dissolve other condensed phases e. polar solvents dissolve nonpolar solutes and vice versa |
b. polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes |
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Ammonium nitrate (NH4NO3) dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because ________. a. the vapor pressure of water decreases upon addition of the solute b. osmotic properties predict this behavior c. of the decrease in enthalpy upon addition of the solute d. of the increase in enthalpy upon dissolution of this strong electrolyte e. of the increase in disorder upon dissolution of this strong electrolyte |
e. of the increase in disorder upon dissolution of this strong electrolyte |
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When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are described as a case of _______. a. hydration b. supersaturation c. cyrstallization d. dehydration e. saturation |
a. hydration |
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When two nonpolar organic liquids are mixed, a solution forms and the enthalpy of solution is quite small. Label the two organic liquids as A (solvent) and B (solute). The fromation of solution is favored by ______. a. hydration of the solute, B b. the equal enthalpy of the solvent and solute c. the highly negative enthalpy of the solution process d. solvation of the solvent, A e. an increase in disorder, since A-A, B-B, and A-B interactions are similar |
e. an increase in disorder, since A-A, B-B, and A-B interactions are similar |
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A saturated solution ______. a. contains as much solvent as it can hold b. contains no double bonds c. contains dissolved solute in equilibrium with undissolved solute d. will rapidly precipitate if a seed crystal is added e. cannot be attained |
c. contains dissolved solute in equilibrium with undissolved solute
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In a saturated solution of a salt in water, ______. a. the rate of crystallization > the rate of dissolution b. the rate of dissolution > the rate of crystallization c. seed crystal addition may cause massive crystallization d. the rate of crystallization = the rate of dissolution e. addition of more water causes massive crystallization |
d. the rate of crystallization = the rate of dissolution
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Compounds composed of a salt and water combined in definite proportions are known as a. clathrates b. homogenates c. ionic solids d. molecular solids e. hydrates |
e. hydrates |
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An unsaturated solution is one that ______. a. has no double bonds b. contains the maximum concentration of solute possible, and is in equilibrium with undissolved solute c. has a concentration lower than the solubility d. contains more dissolved solute than the solubility allows e. contains no solute |
c. has a concentration lower than the solubility
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A solution with a concentration higher than the solubility is ____________. a. not possible b. unsaturated c. supercritical d. saturated e. supersaturated |
e. supersaturated |
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A supersaturated solution _____. a. is one with more than one solute b. is one that has been heated c. is one with a higher concentration than the solubility d. must be in contact with undissolved solid e. exists only in theory and cannot actually be prepared |
c. is one with a higher concentration than the solubility |
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The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the _______. a. strong solvent-solute interactions b. hydrogen bonding in C6H6 c. strength of the covalent bond in NaCl d. weak solvation on Na+ and Cl- by C6H6 e. increased disorder due to mixing of solute and solvent |
d. weak solvation on Na+ and Cl- by C6H6
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Which one of the following substances would be the most soluble in CCl4? a. CH3CH2OH b. H2O c. NH3 d. C10H22 e. NaCl |
d. C10H22 |
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Which of the following substances is more likely to dissolve in water? a. HOCH2CH2CH2OH b. CHCl3 c. O | CH3(CH2)9CH d. CH3(CH2)8CH2OH e. CCL4 |
a. HOCH2CH2CH2OH
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Which of the following substances is more likely to dissolve in CH3OH? a. CCl4 b. Kr c. N2 d. CH3CH2OH e. H2 |
d. CH3CH2OH
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Which of the following substances is more likely to dissolve in CCl4? a. CBr4 b. HBr c. HCl d. CH3CH2OH e. NaCl |
a. CBr4 |
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Which one of the following substances is more likely to dissolve in benzene (C6H6)? a. CH3CH2OH b. NH3 c. NaCl d. CCl4 e. HBr |
d. CCl4 |
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Which one of the following is most soluble in water? a. CH3OH b. CH3CH2CH2OH c. CH3CH2OH d. CH3CH2CH2CH2OH e. CH3CH2CH2CH2CH2OH |
a. CH3OH |
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Pressure has an appreciable effect on the solubility of ________ in liquids. a. gases b. solids c. liquids d. salts e. solids and liquids |
a. gases |
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Which of the following statements is false? a. nonpolar liquids tend to be insoluble in polar substances b. the weaker the attraction between the solute and solvent molecules, the greater the solubility c. substances with similar intermolecular attractive forces tend to be soluble in one another d. the solubility of a gas increases in direct proportion to its partial pressure above the solution e. the solubility of gases in water decrease with increasing temperature |
b. the weaker the attraction between the solute and solvent molecules, the greater the solubility
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Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble) a. CCl4 < CHCl3 < NaNO3 b. CH3OH < CH4 c. CH4 < NaNO3 < CHCl3 d. LiF < NaNO3 < CHCl3 e. CH3OH < Cl4 3 |
a. CCl4 < CHCl3 < NaNO3
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The Proctor & Gamble Company product called olestra is formed by combining a sugar molecule with _____. a. alcohols b. vitamin A c. fatty acids d. protein e. cholesterol |
c. fatty acids |
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Which component of air is the primary problem in a condition known as "the bends"? a. O2 b. CO2 c. He d. N2 e. CO |
d. N2 |
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If the partial pressure of oxygen in the air a diver breathes is too great, _______. a. respiratory tissue is damaged by oxidation b hyperventilation results c. the urge to breathe is increased and excessive CO2 is removed from the body d. the urge to breath is increased and not enough CO2 is removed from the body e. no problems result from this situation |
d. the urge to breath is increased and not enough CO2 is removed from the body
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A solution contains 28% phosphoric acid by mass. This means that _______. a. 1 ml of this solution contains 28 g of phosphoric acid b. 1 L of this solution has a mass of 28 g c. 100 g of this solution contains 28 g of phosphoric acid d. 1 L of this solution contains 28 ml of phosphoric acid e. the density of this solution is 2.8g/ml |
c. 100 g of this solution contains 28 g of phosphoric acid
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Molality is defined as the _______. a. moles solute/moles solvent b. moles solute/Liters solution c. moles solute/kg solution d. moles solute/kg solvent e. none (dimensionless) |
d. moles solute/kg solvent |
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Which one of the following concentration units varies with temperature? a. molarity b. mass percent c. mole fraction d. molality e. all of the above |
a. molarity |
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Of the concentration units below, only _____ is temperature dependent. a. mass % b. ppm c. ppb d. molarity e. molality |
d. molarity |
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A solution contains 11% by mass of sodium chloride. This means that _______. a. there are 11g of sodium chloride in 1.0 ml of this solution b. 100g of the solution contains 11g of sodium chloride c. 100 ml of the solution contains 11g of sodium chloride d. the density of the solution is 11g/ml e. the molality of the solution is 11 |
b. 100g of the solution contains 11g of sodium chloride
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The magnitudes of Kf and Kb depend on the identity of the _______. a. solute b. solvent c. solution d. solvent and on temperature e. solute and solvent |
b. solvent |
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As the concentration of a solute in a solution increases, the freezing point of the solution _______ and the vapor pressure of the solution ______. a. increases, increases b. increases, decreases c. decreases, increases d. decreases, decreases e. decreases, is unaffected |
d. decreases, decreases |
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The ratio of the actual yield of a colligative property to the value calculated, assuming the substance to be a nonelectrolyte, is refered to as ________. a. Henry's law b. vapor pressure lowering c. the van't Hoff factor d. freezing point depression e. osmotic pressure |
c. the van't Hoff factor
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Colligative properties of solutions include all of the following except _______.
a. depression of vapor pressure upon addition of a solute to a solvent b. elevation of the boiling point of a solution upon addition of a solute to a solvent c. depression of the freezing point of a solution upon addition of a solute to a solvent d. an increase in the osmotic pressure of a solution upon the addition of more solute e. the increase of reaction rates with increase in temperature |
e. the increase of reaction rates with increase in temperature
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The process of a substance sticking to the surface of another is called a. absorption b. diffusion c. effusion d. adsorption e. coagulation |
d. adsorption |
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Which of the following cannot be a colloid? a. en emulsion b. an aerosol c. a homogeneous mixture d. a foam e. all of the above are colloids |
c. a homogeneous mixture |
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Hydrophobic colloids _______. a. are those that contain water b. can be stabilized by absorption of ions c. are those that do not contain water d. can be stabilized by coagulation e. will separate into two phases if they are stabilized |
b. can be stabilized by absorption of ions |
