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Q:
A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water to make 100.0 mL of solution. If the density of the solution is 1.1094 g/mL, what is the molality?
A) 0.1775 m H2SO4
B) 0.1810 m H2SO4
C) 1.810 m H2SO4
D) 1.940 m H2SO4
Q:
A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water to make 100.0 mL of solution. If the density of the solution is 1.1094 g/mL, what is the molarity?
A) 0.1775 M H2SO4
B) 0.1810 M H2SO4
C) 1.810 M H2SO4
D) 1.940 M H2SO4
Q:
A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water to make 100.0 mL of solution. If the density of the solution is 1.1094 g/mL, what is the mole fraction H2SO4 in the solution?
A) 0.0181
B) 0.0338
C) 0.0350
D) 19.0
Q:
What is the mole fraction of oxygen in a gas mixture that is 22% oxygen and 78% nitrogen by volume?
A) 0.20
B) 0.22
C) 0.25
D) 0.28
Q:
What is the mole fraction of I2 in a solution made by dissolving 27.8 g of I2 in 245 g of hexane, C6H14?
A) 0.0371
B) 0.0385
C) 0.0715
D) 0.0770
Q:
What is the molality of ethanol in a solution made by dissolving 14.6 g of ethanol, C2H5OH, in 53.6 g of water?
A) 0.00591 m
B) 0.272 m
C) 5.91 m
D) 272 m
Q:
What is the mole fraction of ethanol in a solution made by dissolving 14.6 g of ethanol, C2H5OH, in 53.6 g of water?
A) 0.0964
B) 0.106
C) 0.214
D) 0.272
Q:
Which concentration becomes smaller as the temperature is increased from 20C to 80C?
A) mass %
B) molality
C) molarity
D) mole fraction
Q:
Molality is defined as moles of solute per
A) kilogram of solvent.
B) liter of solution.
C) mole of solvent.
D) total moles present.
Q:
Molarity is defined as moles of solute per
A) kilogram of solvent.
B) liter of solution.
C) mole of solvent.
D) total moles present.
Q:
The dose of amoxicillin given to a young child is 40 mg/kg of body weight/day. If the amoxicillin is administered as a suspension having a concentration of 400 mg/5 mL, how many mL of amoxicillin must be administered per dose for a child weighing 18 pounds?
A) 2.0 mL
B) 4.1 mL
C) 4.5 mL
D) 9.9 mL
Q:
Formaldehyde is a carcinogenic volatile organic compound with a permissible exposure level of 0.75 ppm. At this level, how many grams of formaldehyde are permissible in a 6.0-L breath of air having a density of 1.2 kg/m3?
A) 3.8 10-2 g formaldehyde
B) 5.4 10-6 g formaldehyde
C) 3.8 g formaldehyde
D) 5.4 g formaldehyde
Q:
Fresh air contains approximately 400 ppm CO2, whereas the breath of an intoxicated person contains about 4 percent CO2. The amount of CO2 in the breath of an intoxicated person is ________ times the amount of CO2 in fresh air.
A) 10-2
B) 10-1
C) 101
D) 102
Q:
A solution has a density of 1.023 g/mL and a concentration of 0.0800 g/dL. What is the concentration in parts per million?
A) 700 ppm
B) 782 ppm
C) 800 ppm
D) 818 ppm
Q:
Substances with high lattice energies tend to be less soluble than substances with low lattice energies. On that basis predict the relative aqueous solubility at 20C, from highest to lowest, of the following ionic compounds: Ce2(SO4)3, K2SO4, KBr, NaCl.
A) Ce2(SO4)3 > K2SO4 > KBr > NaCl
B) Ce2(SO4)3 > K2SO4 > NaCl > KBr
C) KBr > NaCl > K2SO4 > Ce2(SO4)3
D) NaCl > KBr > K2SO4 > Ce2(SO4)3
Q:
What are the major solute-solvent interactions created when HOCH2CH2OH dissolves in water?
A) dipole-dipole
B) dispersion
C) hydrogen bonding
D) ion-dipole
Q:
What are the major solute-solvent interactions created when KBr dissolves in water?
A) dipole-dipole
B) dispersion
C) hydrogen bonding
D) ion-dipole
Q:
Which should be least soluble in water?
A) B) C) D)
Q:
Which of the following should most favor the solubility of an ionic solid in water?
A) a low lattice energy for the solid and a low hydration energy for its ions
B) a low lattice energy for the solid and a high hydration energy for its ions
C) a high lattice energy for the solid and a low hydration energy for its ions
D) a high lattice energy for the solid and a high hydration energy for its ions
Q:
Arrange the following compounds in order of their expected increasing solubility in water:
KCl, CH3CH2-O-CH2CH3, CH3CH2CH2CH2-OH, CH3CH2CH2CH2CH3.
A) CH3CH2CH2CH2CH3 < KCl < CH3CH2-O-CH2CH3 < CH3CH2CH2CH2-OH
B) KCl < CH3CH2-O-CH2CH3 < CH3CH2CH2CH2-OH < CH3CH2CH2CH2CH3
C) CH3CH2CH2CH2CH3 < CH3CH2-O-CH2CH3 < KCl < CH3CH2CH2CH2-OH
D) CH3CH2CH2CH2CH3 < CH3CH2-O-CH2CH3 < CH3CH2CH2CH2-OH < KCl
Q:
Most gases become less soluble in water as the temperature increases. What can be concluded about the signs of Hsoln and Ssoln in this case?A) Hsoln is negative and Ssoln is negative.B) Hsoln is negative and Ssoln is positive.C) Hsoln is positive and Ssoln is negative.D) Hsoln is positive and Ssoln is positive.
Q:
For the process of dissolving a solid in a liquid, which of the following statements is true?A) Hsoln is always negative and Ssoln is usually positive.B) Hsoln is always positive and Ssoln is usually negative.C) Hsoln is either positive or negative and Ssoln is usually positive.D) Hsoln is either positive or negative and Ssoln is usually negative.
Q:
The change in the Gibbs free energy for dissolving solute in a saturated solution is
A) negative.
B) zero.
C) positive.
D) positive at low temperatures and negative at high temperatures.
Q:
The change in the Gibbs free energy for dissolving more solute in a supersaturated solution is
A) negative.
B) zero.
C) positive.
D) positive at low temperatures and negative at high temperatures.
Q:
When an ionic solute dissolves in water to form an unsaturated solution, the free energy change (Gsoln) isA) negative.B) zero.C) positive.D) either A or C, depending on the ionic compound
Q:
When two similar liquids mix to form a solution, the entropy of solution (Ssoln) is expected to beA) negative.B) zero.C) positive.D) negative at low temperatures but positive at high temperatures.
Q:
Although there are exceptions, which is most likely to be true for the dissolving of a solid in a liquid?A) Hsoln is positive.B) Hsoln is negative.C) Ssoln is positive.D) Ssoln is negative.
Q:
Which cation in each set would be expected to have the larger (more negative) hydration energy?
I. Fe2+ or Fe3+
II. Li+ or NH4+
A) Fe2+ in set I and Li+ in set II
B) Fe2+ in set I and NH4+ in set II
C) Fe3+ in set I and Li+ in set II
D) Fe3+ in set I and NH4+ in set II
Q:
Which cation in each set is expected to have the larger (more negative) hydration energy?I. Mg2+ or Ba2+II. K+ or Al3+A) Mg2+ in set I and K+ in set IIB) Mg2+ in set I and Al3+ in set IIC) Ba2+ in set I and K+ in set IID) Ba2+ in set I and Al3+ in set II
Q:
One reason ionic compounds do not dissolve well in nonpolar solvents is that
A) ion-dipole interactions are too large for effective solvation to occur.
B) ion-solvent interactions are not strong enough to solvate the ions in solution.
C) not all cations and anions have the same magnitude of charge and therefore do not form neutral ion pairs.
D) there are no forces of attraction between ions and nonpolar molecules.
Q:
In the process of dissolving ionic compounds, the cations and anions are separated from the crystal lattice and surrounded by an ordered shell of solvent molecules. If the solvent is water, the dissolved ions are said to be
A) halogenated.
B) homogenized.
C) hybridized.
D) hydrated.
Q:
When a particular solid begins to dissolve in water, the temperature rises dramatically. For the dissolving of this solid in pure waterA) Hsoln is always negative and Ssoln may be negative or positive.B) Hsoln is always negative and Ssoln is always positive.C) Hsoln is always positive and Ssoln may be negative or positive.D) Hsoln is always positive and Ssoln is always positive.
Q:
Commercial cold packs often contain solid NH4NO3 and a pouch of water. The temperature of the pack drops as the NH4NO3 dissolves in water. Therefore, for the dissolving of NH4NO3 in water,A) Hsoln is negative and Ssoln may be negative or positive.B) Hsoln is negative and Ssoln is positive.C) Hsoln is positive and Ssoln may be negative or positive.D) Hsoln is positive and Ssoln is positive.
Q:
KBr does not dissolve well in nonpolar solvents because
A) solute-solute interactions are much larger than solvent-solvent or solute-solvent interactions.
B) solvent-solvent interactions are much larger than solute-solvent or solute-solute interactions.
C) solute-solvent interactions are much larger than solvent-solvent or solute-solute interactions.
D) solute-solvent interactions are similar to solvent-solvent and solute-solute interactions.
Q:
For which case would Hsoln be expected to be negative?A) if solute-solute interactions are much greater than solvent-solvent and solute-solvent interactionsB) if solvent-solvent interactions are much greater than solute-solvent and solute-solute interactionsC) if solute-solvent interactions are much greater than solvent-solvent and solute-solute interactionsD) if solute-solvent interactions are the same as solvent-solvent and solute-solute interactions
Q:
Iodine, I2(s), is more soluble in dichloromethane, CH2Cl2(l), than in water because
A) both iodine and dichloromethane have strong ion-dipole interactions.
B) the dipole-dipole forces in dichloromethane are much stronger than the dispersion forces in iodine.
C) the intermolecular forces are similar in both iodine and dichloromethane.
D) iodine is polar and dichloromethane has a large number of hydrogen bonds.
Q:
For a liquid solution made by dissolving a solid or a gas in a liquid, the
A) liquid is the solute.
B) liquid is the solvent.
C) solute is the component present in the greatest amount.
D) solvent is the component present in the greatest amount.
Q:
Which is not a solution?
A) brass
B) fog
C) hydrochloric acid
D) wine
Q:
The rubbing alcohol sold in drug stores often is composed of 70% isopropyl alcohol and 30% water. In this solution
A) isopropyl alcohol is the solvent.
B) water is the solvent.
C) both water and isopropyl alcohol are solvents.
D) neither water nor isopropyl alcohol is a solvent.
Q:
In most liquid solutions, the component present in the larger amount is called the
A) dispersed medium.
B) emulsifying agent.
C) solute.
D) solvent.
Q:
Stainless steel is an example of a ________ solution.
A) gas/solid
B) liquid/liquid
C) solid/liquid
D) solid/solid
Q:
Which of the following mixtures have components which can be separated by filtration?
A) colloids
B) solutions
C) suspensions
D) All of these
Q:
At 25 oC the vapor pressures of benzene and toluene are 96.0 mm Hg and 30.5 mm Hg, respectively. When a 1:1 molar mixture of benzene and toluene is fractionally distilled, the first fraction will have a mole fraction of benzene that is ________ (equal to, greater than, less than) 0.50.
Q:
At 300 K a 500.0 mL solution containing 0.4314 g of dextrose has an osmotic pressure of 89.6 mm Hg. What is the molar mass of dextrose?
Q:
The osmotic pressure of a 100-mL solution containing 1.0 g of sucrose, C12H22O11 will be ________ (equal to, greater than, less than) the osmotic pressure of a 100-mL solution containing 1.0 g of fructose, C6H12O6.
Q:
The osmotic pressure of a 0.10 M solution of sucrose, C12H22O11 will be ________ (equal to, greater than, less than) the osmotic pressure of a 0.10 M solution of fructose, C6H12O6.
Q:
A 1.0 m aqueous CaCl2 solution will have a ________ vapor pressure, ________ freezing point, and ________ boiling point than a 1.0 m aqueous solution of NaCl.
Q:
The boiling point of a solution containing a nonvolatile solute will be ________ than the boiling point of the pure solvent, whereas the boiling point of a solution of two volatile liquids will be ________ than the boiling point of the more volatile liquid and ________ than the boiling point of the less volatile liquid.
Q:
At 25C the vapor pressures of benzene and toluene are 96.0 mm Hg and 30.5 mm Hg, respectively. The vapor pressure of a solution that has a 0.50 mole fraction of toluene will have a vapor pressure ________ (equal to, greater than, less than) 30.5 mm Hg.
Q:
The vapor pressure of water at 25C is 23.8 mm Hg. The vapor pressure lowering, P, of an aqueous solution containing 0.500 mole fraction NaCl is ________ (equal to, greater than, less than) 11.9 mm Hg?
Q:
If dissociation of MgCl2 in water were 100%, the van"t Hoff factor would be ________; however, for real solutions the van"t Hoff factor for MgCl2 is ________ (greater than, less than) this value.
Q:
At 80.0C benzene has a vapor pressure of 96.0 mm Hg and toluene has a vapor pressure of 30.3 mm Hg. If a mixture of benzene and toluene has a vapor pressure of 54.6 mm Hg, what are the mole fractions of benzene and toluene?
Q:
At 80.0C heptane, C7H16, has a vapor pressure of 428 mm Hg and octane, C8H18, has a vapor pressure of 175 mm Hg. What is the vapor pressure of a solution that contains 20.0 g C7H16 and 11.4 g C8H18?
Q:
Freezing point depression, boiling point elevation, vapor pressure lowering, and osmotic pressure are examples of ________ properties, which depend on the amount but not the chemical identity of dissolved particles.
Q:
At 20C and 0.28 atm pressure Xenon has a solubility in water of 1.4 mmol/L. What is the Henry's Law-constant in mol/ Latm at 20C?
Q:
Dinitrogen monoxide is still used as a general anesthetic. The Henry's law constant for the solubility of N2O in water is 2.5 10-2 mol/Latm. What is the molar solubility of N2O in water if the partial pressure of N2O is 1500 m Hg?
Q:
The solubility of a gas in a liquid is greatest at ________ pressures and ________ temperatures.
Q:
Concentrations of fluoride in drinking water greater than 4.0 mg/L can cause mottled teeth in children. What is 4.0 mg/L expressed as molality?
Q:
Cocaine, C17H21NO4, in urine can be confirmed by mass spectroscopy at a concentration of 150 ng/mL. Assuming a urine density of 1.025 g/mL, what is this concentration expressed as molality?
Q:
The volume of 0.200 M H2SO4 that contains 5.00 mmol of H+ is ________ mL.
Q:
The number of moles of ions in 25 mL of 2.0 M Na2SO4 is ________ moles.
Q:
Molarity is defined as ________, whereas molality is defined as ________.
Q:
Amphetamines in urine can be confirmed by mass spectroscopy at a concentration of 500 ng/mL. Assuming a urine density of 1.025 g/mL, what is this concentration in parts per million?
Q:
A person is considered legally intoxicated with a blood alcohol level of 80 mg/dL. Assuming that blood plasma has a density of 1.025 g/mL, what is this concentration expressed in parts per million?
Q:
When KI is dissolved in water, the major forces overcome are ________ forces in the solute and ________ forces in the solvent, and the major forces created between solute and solvent particles are ________ forces.
Q:
According to the rule of thumb "like dissolves like." ionic solids like NaCl or polar substances like glucose are more soluble in ________ solvents, whereas nonpolar substances like I2 are more soluble in ________ solvents.
Q:
In a solution that is 55% ethyl alcohol and 45% water, the solute is ________ and the solvent is ________.
Q:
An aqueous solution has a normal boiling point of 10 3.0C. What is the freezing point of this solution? For water Kb = 0.51C /m and Kf = 1.86C /m.
A) -0. 82C
B) - 3.0C
C) -3.6C
D) - 11C
Q:
What is the freezing point of a solution of 7.15 g MgCl2 in 100 g of water? Kf for water is A) -0. 140C
B) - 1.40C
C) - 2.80C
D) - 4.18C
Q:
Calculate the freezing point of a solution of 40.0 g methyl salicylate, C7H6O2, dissolved in 800. g of benzene, C6H6. Kf for benzene is 5.10C /m and the freezing point is 5.50C for benzene.
A) - 2.09C
B) 2.09C
C) 3.41C
D) 7.59C
Q:
What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86C/m.
A) -0.93C
B) -1.9C
C) -2.8C
D) -6.5C
Q:
Which of the following solutions will have the lowest freezing point?
A) 0.010 m KBr
B) 0.010 m Na2CO3
C) 0.035 m CH3CH2OH
D) 0.015 m BaCl2
Q:
At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene = 0. 580.
A) 106 mm Hg
B) 121 mm Hg
C) 131 mm Hg
D) 242 mm Hg
Q:
A KCl solution is prepared by dissolving 20.0 g KCl in 250.0 g of water at 25C. What is the vapor pressure of the solution if the vapor pressure of water at 25C is 23.76 mm Hg?
A) 22.0 mm Hg
B) 22.9 mm Hg
C) 23.3 mm Hg
D) 24.6 mm Hg
Q:
A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. g of water at 25C. What is the vapor pressure of the solution if the vapor pressure of water at 25C is 23.76 mm Hg?
A) 0.198 mm Hg
B) 20.5 mm Hg
C) 23.6 mm Hg
D) 24.0 mm Hg
Q:
The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L atm) at 25C. What is the solubility of methyl bromide in water at 25C and at a partial pressure of 270. mm Hg?A) 0.0 565 mol/LB) 0.3 55 mol/LC) 0.4 48 mol/LD) 42.9 mol/L
Q:
In which case should CO2(g) be more soluble in water?
A) The total pressure is 5 atm and the partial pressure of CO2 is 0.5 atm.
B) The total pressure is 3 atm and the partial pressure of CO2 is 1 atm.
C) The total pressure is 1 atm and the partial pressure of CO2 is 0. 03 atm.
D) The total pressure is 1 atm and the partial pressure of CO2 is 0. 4 atm.
Q:
A solution of LiCl in water is 20.0 wt% LiCl. What is the mole fraction of LiCl?
A) 0. 0960
B) 0. 106
C) 0. 472
D) 4. 44
Q:
A solution of LiCl in water has XLiCl = 0.0 900. What is the molality?
A) 4.46 m LiCl
B) 5.00 m LiCl
C) 5.49 m LiCl
D) 9.89 m LiCl
Q:
What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose, C6H12O6, in 125.9 g of water?
A) 7.94 10-4 m
B) 0.143 m
C) 0.695 m
D) 0.794 m