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chemistry
physical chemistry

Questions and Answers of Physical Chemistry

A solution contains 0.115 mol H2O and an unknown number of moles of sodium chloride. The vapor pressure of the solution at 30 oC is 25.7 torr. The vapor pressure of pure water at this temperature is
Two beakers are placed in a sealed box at 25 oC. One beaker contains 30.0 mL of a 0.050 M aqueous solution of a non-volatile nonelectrolyte. The other beaker contains 30.0 mL of a 0.035 M aqueous
A car owner who knows no chemistry has to put antifreeze in his car's radiator. The instructions recommend a mixture of 30% ethylene glycol and 70% water. Thinking he will improve his protection he
Calculate the freezing point of a 0.100 m aqueous solution of K2SO4, (a) Ignoring interionic attractions, and (b) Taking interionic into consideration by using the van't Hoff factor (Table 13.4)?
Carbon disulfide (CS2) boils at 46.30 oC and has a density of 1.261 g/mL.
A lithium salt used in lubricating grease has the formula LiCnH2n+1O2. The salt is soluble in water to the extent of 0.036 g per 100 g of water at 25 oC. The osmotic pressure of this solution is
Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at 25 oC, and their solubilities
At ordinary body temperature (37 oC) the solubility of N2 in water in contact with air at ordinary atmospheric pressure (1.0 atm) is 0.015 g/L. Air is approximately 78 mol % N2. Calculate the number
Consider of following values for enthalpy of vaporization (kJ/mol) of several organic substances:(a) Use variations in the intermolecular forces operating in these organic substances to account for
A textbook on chemical thermodynamics states, "The heat of solution represents the difference between the lattice energy of the crystalline solid and the solvation energy of the gaseous ions." (a)
Suppose you had a balloon made of some highly flexible semipermeable membrane. The balloon is filled completely with a 0.2 M solution of some solute and is submerged in a 0.1 M solution of the same
(a) A sample of hydrogen gas is generated in a closed container by reacting 2.050 g of zinc metal with 15.0 mL of 1.00 M sulfuric acid. Write the balanced equation for the reaction, and calculate the
The following table presents the solubilities of several gases in water at 25 oC under a total pressure of gas and water vapor of 1 atm.
A small cube of lithium (density = 0.535 g/cm3) measuring 1.0 mm on edge is added to 0.500 L of water. The following reaction occurs: 2 Li(s) + 2 H2O(l) → LiOH(aq) + H2(g)
At 35 oC the vapor pressure of acetone, (CH3)2CO, is 360 torr, and that of chloroform, CHCl3, is 300 torr. Acetone and chloroform can form very weak hydrogen bonds between one another as follows:
The molecule n-octylglucoside, shown here, is widely used in biochemical research as a nonionic detergent for "solubilizing" large hydrophobic protein molecules. What characteristics of this molecule
In general, the attractive intermolecular forces between solvent and solute particles must be comparable or greater than solute-solute interactions for significant solubility to occur. Explain this
(a) Considering the energetics of solute-solute, solvent- solvent, and solute-solvent interactions, explain why NaCl dissolves in water but not in benzene (C6H6). (b)What factors cause a cation to be
Indicate the type of solute-solvent interaction (Section 11.2) that should be most important in each of the following solutions: (a) CCl4 in benzene (C6H6), (b) Methanol (CH3OH) in water, (c) KBr in
Indicate the principal type of solute-solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute-solvent interaction: (a) KCl in water, (b) CH2Cl2
An ionic compound has a very negative in water. Would you expect it to be very soluble or nearly insoluble in water? Explain in terms of the enthalpy and entropy changes that accompany the process?
When ammonium chloride dissolves in water, the solution becomes colder. (a) Is the solution process exothermic or endothermic? (b) Why does the solution form?
(a) In Equation 13.1 which of the enthalpy terms for dissolving an ionic solid would correspond to the lattice energy? (b) Which energy term in this equation is always exothermic?
The schematic diagram of the solution process as the net sum of three steps in Figure 13.4 does not show the relative magnitudes of the three components because these will vary from case to case. For
When two nonpolar organic liquids such as hexane (C6H14) and heptane (C7H16) are mixed, the enthalpy change that occurs is generally quite small. (a) Use the enthalpy diagram in Figure 13.4 to
The enthalpy of solution of KBr in water is about + 198 kJ/Mol. Nevertheless, the solubility of KBr in water is relatively high. Why does the solution process occur even though it is endothermic?
The solubility of Cr(NO3)3 ( 9 H2O in water is 208 g per 100 g of water at 15oC. A solution of Cr(NO3)3 ( 9 H2O in water at is formed by dissolving 324 g in 100 g water. When this solution is slowly
The solubility of MnSO4 ( H2O in water at 20oC is 70 g per 100 mL of water.
By referring to Figure 13.18, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40oC will lead to a saturated solution: (a) NaNO3, (b) KCl, (c)
By referring to Figure 13.18, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 oC:(a) KClO3,(b) Pb(NO3)2,(c) Ce2(SO4)3.
Water and glycerol, CH2(OH)CH(OH)CH2OH, are miscible in all proportions. What does this mean? How do the OH groups of the alcohol molecule contribute to this miscibility?
Oil and water are immiscible. What does this mean? Explain in terms of the structural features of their respective molecules and the forces between them?
Common laboratory solvents include acetone (CH3COCH3), methanol (CH3OH), toluene (C6H5CH3), and water. Which of these is the best solvent for nonpolar solutes? Explain.
How does the lattice energy of an ionic solid affect its solubility in water?
Would you expect alanine (an amino acid) to be more soluble in water or in hexane? Explain.
(a) Would you expect stearic acid, CH3(CH2)16COOH, to be more soluble in water or in carbon tetrachloride? Explain.(b) Which would you expect to be more soluble in water, cyclohexane or dioxane?
Ibuprofen, widely used as a pain reliever, has a limited solubility in water, less than 1 mg/mL. Which feature of the molecule contributes to its low solubility in water, and which feature
Which of the following in each pair is likely to be more soluble in hexane, C6H14: (a) CCl4 or CaCl2; (b) Benzene (C6H6) or glycerol, CH2(OH)CH(OH)CH2OH; (c) Octanoic acid, CH3CH2CH2CH2CH2CH2CH2COOH,
Which of the following in each pair is likely to be more soluble in water: (a) Cyclohexane (C6H12) or glucose (C6H12O6) (Figure 13.12); (b) Propionic acid (CH3CH2COOH) or sodium propionate
(a) Explain why carbonated beverages must be stored in sealed containers. (b) Once the beverage has been opened, why does it maintain more carbonation when refrigerated than at room temperature?
Explain why pressure substantially affects the solubility of O2 in water but has little effect on the solubility of NaCl in water?
The Henry's law constant for helium gas in water in 30 oC is 3.7 × 10-4 M/atm and the constant for N2 at 30 oC is 6.0 × 10-4 M/atm. If the two gases are each present at 1.5 atm pressure, calculate
The partial pressure of O2 in air at sea level is 0.21 atm. Using the data in Table 13.1, together with Henry's law, calculate the molar concentration of O2 in the surface water of a mountain lake
(a) Calculate the mass percentage of Na2SO4 in a solution containing 10.6 g Na2SO4 in 483 g water.(b) An ore contains 2.86 g of silver per ton of ore. What is the concentration of silver in ppm?
A quantity of the blue solid on the left in Figure 13.7 is placed in an oven and heated for a time. It slowly turns from blue to the white of the solid on the right. What has occurred?
(a) What is the mass percentage of iodine (I2) in a solution containing 0.035 mol I2 in 125 g of CCl4?(b) Seawater contains per 0.0079 g Sr2+ kilogram of water. What is the concentration of Sr2+
A solution is made containing 14.6 g of CH3OH in 184 g H2O. Calculate(a) The mole fraction of CH3OH,(b) The mass percent of CH3OH, (c) The molality of CH3OH.
A solution is made containing 20.8 g phenol (C6H5OH) in 425 g ethanol (C2H5OH). Calculate(a) The mole fraction of phenol,(b) The mass percent of phenol,(c) The molality of phenol?
Calculate the molarity of the following aqueous solutions:(a) 0.540 g Mg(NO3)2 in 250.0 mL of solution,(b) 22.4 g LiCIO4 ( 3 H2O in 125 mL of solution,(c) 25.0 mL of 3.50 M HNO3 diluted to 0.250 L.
What is the molarity of each of the following solutions:(a) 15.0 g Al2(SO4)3 in 0.250 mL solution,(b) 5.25 g in 175 mL of solution,(c) 35.0 mL of 9.00 M H2SO4 diluted to 0.500 L?
Calculate the molality of each of the following solutions:(a) 8.66 g benzene (C6H6) dissolved in 23.6 g carbon tetrachloride (CCl4),(b) 4.80 g NaCl dissolved in 0.350 L of water?
(a) What is the molality of a solution formed by dissolving 1.12 mol of KCl in 16.0 mol of water?(b) How many grams of sulfur (S8) must be dissolved in 100.0 g naphthalene (C10H8) to make a 0.12 m
A sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution has a density of 1.329 g/cm3. Calculate (a) The mass percentage, (b) The mole fraction, (c) The molality, (d) The molarity
Ascorbic acid (vitamin C, C6H8O6) is a water-soluble vitamin.
The density of acetonitrile (CH3CN) is 0.786 g/mL and the density of methanol (CH3OH) is 0.791 g/mL. A solution is made by dissolving 22.5 mL CH3OH in 98.7 mL CH3CN. (a) What is the mole fraction of
Which of the following is the best representation of a saturated solution? Explain your reasoning.
The density of toluene (C7H8) is 0.876, and the density of thiophene (C4H4S) is 1.065 g/mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. (a) Calculate the mole
Calculate the number of moles of solute present in each of the following aqueous solutions: (a) 600 mL of 0.250 M SrBr2, (b) 86.4 g of 0.180 m KCl, (c) 124.0 g of a solution that is 6.45% glucose
Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 M HNO3(aq), (b) 50.0 mg of an aqueous solution that is 1.50 m NaCl, (c) 75.0 g of an aqueous
Describe how you would prepare each of the following aqueous solutions, starting with solid KBr: (a) 0.75 L of 1.5 × 10-2 M KBr, (b) 125 g of 0.180 m KBr, (c) 1.85 L of a solution that is by mass
Describe how you would prepare each of the following aqueous solutions: (a) 1.50 L of 0.110 M (NH4)2SO4 solution, starting with solid (NH4)2SO4; (b) 225 g of a solution that is 0.65 m in Na2CO3,
Commercial aqueous nitric acid has a density of 1.42 g/mL and is 16 M. Calculate the percent HNO3 by mass in the solution?
Commercial concentrated aqueous ammonia is 28% NH3 by mass and has a density of 0.90 g/mL. What is the molarity of this solution?
Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of red brass consisting of 80.0% Cu and 20.0% Zn by mass has a density of 8750 kg/m3. (a) What is the
Caffeine (C8H10N4O2) is a stimulant found in coffee and tea. If a solution of caffeine in chloroform (CHCl3) as a solvent has a concentration of 0.0500 m, calculate (a) The percent caffeine by
During a typical breathing cycle, the CO2 concentration in the expired air rises to a peak of 4.6% by volume. Calculate the partial pressure of the CO2 at this point, assuming 1 atm pressure. What is
The solubility of Xe in water at 1 atm pressure and 20 oC is approximately 5 × 10-3. Compare this with the solubilities of Ar and Kr in water (Table 13.1) and explain what properties of the rare gas
Breathing air that contains 4.0% by volume CO2 over time causes rapid breathing, throbbing headache, and nausea, among other symptoms. What is the concentration of CO2 in such air in terms of (a) Mol
How does increasing the concentration of a nonvolatile solute in water affect the following properties: (a) Vapor pressure, (b) Freezing point, (c) Boiling point; (d) Osmotic pressure?
Consider two solutions, one formed by adding 10 g of glucose (C6H12O6) to 1 L of water and the other formed by adding 10 g of sucrose (C12H22O11) to 1 L of water. Are the vapor pressures over the two
(a) What is an ideal solution? (b) The vapor pressure of pure water at is 60 oC is 149 torr. The vapor pressure of water over a solution at 60 oC containing equal numbers of moles of water and
(a) Calculate the vapor pressure of water above a solution prepared by adding 22.5 g of lactose (C12H22O11) to 200.0 g of water at 338 K. (Vapor-pressure data for water are given in Appendix B.) (b)
(a) Calculate the vapor pressure of water above a solution prepared by dissolving 28.5 g of glycerin (C3H8O3) in 125 g of water at 343 K. (The vapor pressure of water is given in Appendix B.) (b)
At 63.5 oC the vapor pressure of H2O is 175 torr, and that of ethanol (C2H5OH) is 400 torr. A solution is made by mixing equal masses of H2O and C2H5OH. (a) What is the mole fraction of ethanol in
At 20 oC the vapor pressure of benzene (C6H6) is 75 torr, and that of toluene (C7H8) is 22 torr. Assume that benzene and toluene form an ideal solution. (a) What is the composition in mole fractions
(a) Why does a 0.10 m aqueous solution of NaCl have a higher boiling point than a 0.10 m aqueous solution of C6H12O6? (b) Calculate the boiling point of each solution. (c) The experimental boiling
The structures of vitamins E and B6 are shown below. Predict which is largely water soluble and which is largely fat soluble. Explain.
Arrange the following aqueous solutions, each by mass in solute, in order of increasing boiling point: glucose (C6H12O6), sucrose (C12H22O11), sodium nitrate (NaNO3)?
List the following aqueous solutions in order of increasing boiling point: 0.120 m glucose, 0.050 m LiBr, 0.050 m Zn(NO3)2?
List the following aqueous solutions in order of decreasing freezing point: 0.040 m glycerin (C3H8O3), 0.020 m KBr, 0.030 m phenol (C6H5OH)?
Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (a) 0.22 m glycerol (C3H8O3) in ethanol, (b) 0.240 mol of naphthalene (C10H8) in 2.45 mol of
Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (a) 0.25 m glucose in ethanol; (b) 20.0 g of decane, C10H22, in 50.0 g CHCl3; (c) 3.50 g NaOH
How many grams of ethylene glycol (C2H6O2) must added to 1.00 kg of water to produce a solution that freezes at - 5.00 oC?
What is the freezing point of an aqueous solution that boils at 105.0 oC?
What is the osmotic pressure formed by dissolving 44.2 mg of aspirin (C9H8O4) in 0.358 L of water at 25 oC?
Seawater contains 3.4 g of salts for every liter of solution. Assuming that the solute consists entirely of NaCl (over 90% is), calculate the osmotic pressure of seawater at 20 oC?
Adrenaline is the hormone that triggers the release of extra glucose molecules in times of stress or emergency. A solution of 0.64 g of adrenaline in 36.0 g of CCl4 elevates the boiling point by 0.49
If you wanted to prepare a solution of CO in water at in which the CO concentration was 2.5 mM, what pressure of CO would you need to use? (See Figure 13.19.)
Lauryl alcohol is obtained from coconut oil and is used to make detergents. A solution of 5.00 g of lauryl alcohol in 0.100 kg of benzene freezes at 4.1 oC. What is the approximate molar mass of
Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210 mL of solution has an osmotic pressure of 0.953 torr at 25 oC. What is the molar mass of
A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 L of solution. The resulting solution has an osmotic pressure
The osmotic pressure of a 0.010 M aqueous solution of CaCl2 is found to be 0.674 atm at 25 oC. (a) Calculate the van't Hoff factor, i, for the solution. (b) How would you expect the value of i to
Based on the data given in Table 13.4, which solution would give the larger freezing-point lowering, a 0.030 m solution of NaCl or a 0.020 m solution of K2SO4? How do you explain the departure from
(a) Why is there no colloid in which both the dispersed substance and the dispersing substance are gases?
(a) Many proteins that remain homogeneously distributed in water have molecular masses in the range of 30,000 amu and larger. In what sense is it appropriate to consider such suspensions to be
Indicate whether each of the following is a hydrophilic or a hydrophobic colloid: (a) Butterfat in homogenized milk, (b) Hemoglobin in blood, (c) Vegetable oil in a salad dressing, (d) Colloidal gold
Explain how each of the following factors helps determine the stability or instability of a colloidal dispersion: (a) Particulate mass, (b) Hydrophobic character, (c) Charges on colloidal particles?
Colloidal dispersions of proteins, such as a gelatin, can often be caused to separate into two layers by addition of a solution of an electrolyte. Given that protein molecules may carry electrical
The figure shows two identical volumetric flasks containing the same solution at two temperatures. (a) Does the molarity of the solution change with the change in temperature? Explain. (b) Does the
Explain how (a) A soap such as sodium stearate stabilizes a colloidal dispersion of oil droplets in water; (b) Milk curdles upon addition of an acid?

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