Define molality

What is a solution? List some examples.

What is an aqueous solution?

In a solution, what is the solvent? What is the solute? List some examples.

Explain what like dissolves like means.

What is solubility?

Describe what happens when additional solute is added to: (a) a saturated solution (b) an unsaturated solution (c) a supersaturated solution

Explain the difference between a strong electrolyte solution and a nonelectrolyte solution. What kinds of solutes form strong electrolyte solutions?

How does gas solubility depend on temperature?

Explain recrystallization.

How is rock candy made?

When you heat water on a stove, bubbles form on the bottom of the pot before the water boils. What are these bubbles? Why do they form?

Explain why warm soda pop goes flat faster than cold soda pop.

How does gas solubility depend on pressure? How does this relationship explain why a can of soda pop fizzes when opened.

What is the difference between a dilute solution and a concentrated solution?

Define the concentration units mass percent and molarity.

What is a stock solution?

How does the presence of a nonvolatile solute affect the boiling point and melting point of a solution relative to the boiling point and melting point of the pure solvent?

What are colligative properties?

Define molality

What is osmosis?

Two shipwreck survivors were rescued from a life raft. One had drunk seawater while the other had not. The one who had drunk the seawater was more severely dehydrated than the one who did not. Explain.

Why are intravenous fluids always isoosmotic saline solutions? What would happen if pure water were administered intravenously?

Determine whether or not each mixture is a solution. (a) sand and water mixture (b) oil and water mixture (c) salt and water mixture (d) sterling silver cup

Determine whether or not each mixture is a solution. (a) air (b) carbon dioxide and water mixture (c) a blueberry muffin (d) a brass buckle

Identify the solute and solvent in each solution. (a) salt water (b) sugar water (c) soda water

Identify the solute and solvent in each solution. (a) 80-proof vodka (40% ethyl alcohol) (b) oxygenated water (c) antifreeze (ethylene glycol and water)

Pick an appropriate solvent from Table 13.2 to dissolve: (a) motor oil (nonpolar) (b) sugar (polar) (c) lard (nonpolar) (d) potassium chloride (ionic)

Pick an appropriate solvent from Table 13.2 to dissolve: (a) glucose (polar) (b) salt (ionic) (c) vegetable oil (nonpolar) (d) sodium nitrate (ionic)

What are the dissolved particles in a solution containing an ionic solute? What is the name for this kind of solution?

What are the dissolved particles in a solution containing a molecular solute? What is the name for this kind of solution?

A solution contains 35 g of NaCl per 100 g of water at 25 C. Is the solution unsaturated, saturated, or supersaturated? (See Figure 13.4.)

A solution contains 28 g of KNO3 per 100 g of water at 25 C. Is the solution unsaturated, saturated, or supersaturated? (See Figure 13.4.)

A KNO3 solution containing 45 g of KNO3 per 100 g of water is cooled from 40 C to 0 C. What happens during cooling? (See Figure 13.4.)

A KCl solution containing 42 g of KCl per 100 g of water is cooled from 60 C to 0 C. What happens during cooling? (See Figure 13.4.)

Refer to Figure 13.4 to determine whether each of the given amounts of solid will completely dissolve in the given amount of water at the indicated temperature. (a) 30.0 g KClO3 in 85.0 g of water at 35 C (b) 65.0 g NaNO3 in 125 g of water at 15 C (c) 32.0 g KCl in 70.0 g of water at 82 C

Refer to Figure 13.4 to determine whether each of the given amounts of solid will completely dissolve in the given amount of water at the indicated temperature. (a) 45.0 g CaCl2 in 105 g of water at 5 C (b) 15.0 g KClO3 in 115 g of water at 25 C (c) 50.0 g Pb(NO3)2 in 95.0 g of water at 10 C

Some laboratory procedures involving oxygensensitive reactants or products call for using preboiled (and then cooled) water. Explain why this is so.

A person preparing a fish tank uses preboiled (and then cooled) water to fill it. When the fish is put into the tank, it dies. Explain.

Scuba divers breathing air at increased pressure can suffer from nitrogen narcosisa condition resembling drunkennesswhen the partial pressure of nitrogen exceeds about 4 atm. What property of gas/water solutions causes this to happen? How could the diver reverse this effect?

Scuba divers breathing air at increased pressure can suffer from oxygen toxicitytoo much oxygen in the bloodstreamwhen the partial pressure of oxygen exceeds about 1.4 atm. What happens to the amount of oxygen in a divers bloodstream when he or she breathes oxygen at elevated pressures? How can this be reversed?

Calculate the concentration of each solution in mass percent. (a) 41.2 g C12H22O11 in 498 g H2O (b) 178 mg C6H12O6 in 4.91 g H2O (c) 7.55 g NaCl in 155 g H2O

Calculate the concentration of each solution in mass percent. (a) 132 g KCl in 598 g H2O (b) 22.3 mg KNO3 in 2.84 g H2O (c) 8.72 g C2H6O in 76.1 g H2O

A soft drink contains 42 g of sugar in 311 g of H2O. What is the concentration of sugar in the soft drink in mass percent?

A soft drink contains 32 mg of sodium in 309 g of H2O. What is the concentration of sodium in the soft drink in mass percent?

Complete the table: Mass Solute Mass Solvent Mass Solution Mass Percent 15.5 g 238.1 g ______ ______ 22.8 g ______ ______ 12.0% ______ 183.3 g 212.1 g ______ ______ 315.2 g ______ 15.3%

Complete the table: Mass Solute Mass Solvent Mass Solution Mass Percent 2.55 g 25.0 g ______ ______ ______ 45.8 g ______ 3.8% 1.38 g ______ 27.2 g ______ 23.7 g ______ ______ 5.8%

Ocean water contains 3.5% NaCl by mass. How much salt can be obtained from 254 g of seawater?

A saline solution contains 1.1% NaCl by mass. How much NaCl is present in 96.3 g of this solution?

Determine the amount of sucrose in each solution. (a) 48 g of a solution containing 3.7% sucrose by mass (b) 103 mg of a solution containing 10.2% sucrose by mass (c) 3.2 kg of a solution containing 14.3% sucrose by mass

Determine the amount of potassium chloride in each solution. (a) 19.7 g of a solution containing 1.08% KCl by mass (b) 23.2 kg of a solution containing 18.7% KCl by mass (c) 38 mg of a solution containing 12% KCl by mass

Determine the mass (in g) of each NaCl solution that contains 1.5 g of NaCl. (a) 0.058% NaCl by mass (b) 1.46% NaCl by mass (c) 8.44% NaCl by mass

Determine the mass (in g) of each sucrose solution that contains 12 g of sucrose. (a) 4.1% sucrose by mass (b) 3.2% sucrose by mass (c) 12.5% sucrose by mass

AgNO3 solutions are often used to plate silver onto other metals. What is the maximum amount of silver in grams that can be plated out of 4.8 L of an AgNO3 solution containing 3.4% Ag by mass? (Assume that the density of the solution is 1.01 g/mL.)

A dioxin-contaminated water source contains 0.085% dioxin by mass. How much dioxin is present in 2.5 L of this water? (Assume that the density of the solution is 1.01 g/mL.)

Ocean water contains 3.5% NaCl by mass. What mass of ocean water in grams contains 45.8 g of NaCl?

A hard water sample contains 0.0085% Ca by mass (in the form of ions). What mass of water in grams contains 1.2 g of Ca? (1.2 g of Ca is the recommended daily allowance of calcium for 19- to 24-year-olds.)

Lead is a toxic metal that affects the central nervous system. A Pb-contaminated water sample contains 0.0011% Pb by mass. What volume of the water in milliliters contains 115 mg of Pb? (Assume that the density of the solution is 1.0 g/mL.)

Benzene is a carcinogenic (cancer-causing) compound. A benzene-contaminated water sample contains 0.000037% benzene by mass. What volume of the water in liters contains 175 mg of benzene? (Assume that the density of the solution is 1.0 g/mL.)

Calculate the molarity of each solution. (a) 0.127 mol of sucrose in 655 mL of solution (b) 0.205 mol of KNO3 in 0.875 L of solution (c) 1.1 mol of KCl in 2.7 L of solution

Calculate the molarity of each solution. (a) 1.54 mol of LiCl in 22.2 L of solution (b) 0.101 mol of LiNO3 in 6.4 L of solution (c) 0.0323 mol of glucose in 76.2 mL of solution

Calculate the molarity of each solution. (a) 22.6 g of C12H22O11 in 0.442 L of solution (b) 42.6 g of NaCl in 1.58 L of solution (c) 315 mg of C6H12O6 in 58.2 mL of solution

Calculate the molarity of each solution. (a) 33.2 g of KCl in 0.895 L of solution (b) 61.3 g of C2H6O in 3.4 L of solution (c) 38.2 mg of KI in 112 mL of solution

A 205-mL sample of ocean water contains 6.8 g of NaCl. What is the molarity of the solution with respect to NaCl?

A 355-mL can of soda pop contains 41 g of sucrose (C12H22O11). What is the molarity of the solution with respect to sucrose?

How many moles of NaCl are contained in each solution? (a) 1.5 L of a 1.2 M NaCl solution (b) 0.448 L of a 0.85 M NaCl solution (c) 144 mL of a 1.65 M NaCl solution

How many moles of sucrose are contained in each solution? (a) 3.4 L of a 0.100 M sucrose solution (b) 0.952 L of a 1.88 M sucrose solution (c) 21.5 mL of a 0.528 M sucrose solution

What volume of each solution contains 0.15 mol of KCl? (a) 0.255 M KCl (b) 1.8 M KCl (c) 0.995 M KCl

What volume of each solution contains 0.325 mol of NaI? (a) 0.152 M NaI (b) 0.982 M NaI (c) 1.76 M NaI

Complete the table: Solute Solute Mass Mol Solute Volume Solution Molarity KNO3 22.5 g ______ 125.0 mL ______ NaHCO3 ______ ______ 250.0 mL 0.100 M C12H22O11 55.38 g ______ ______ 0.150 M

Complete the table: Solute Solute Mass Mol Solute Volume Solution Molarity MgSO4 0.588 g ______ 25.0 mL ______ NaOH ______ ______ 100.0 mL 1.75 M CH3OH 12.5 g ______ ______ 0.500 M

Calculate the mass of NaCl in a 35-mL sample of a 1.3 M NaCl solution.

Calculate the mass of glucose (C6H12O6) in a 105-mL sample of a 1.02 M glucose solution.

A chemist wants to make 2.5 L of a 0.100 M KCl solution. How much KCl in grams should the chemist use?

A laboratory procedure calls for making 500.0 mL of a 1.4 M KNO3 solution. How much KNO3 in grams is needed?

How many liters of a 0.500 M sucrose (C12H22O11) solution contain 1.5 kg of sucrose?

What volume of a 0.35 M Mg(NO3)2 solution contains 87 g of Mg(NO3)2?

Determine the concentration of in each aqueous solution. (Assume complete dissociation of each compound.) (a) 0.15 M NaCl (b) 0.15 M CuCl2 (c) 0.15 M AlCl3

Determine the concentration of in each aqueous solution. (Assume complete dissociation of each compound.) (a) 0.10 M KNO3 (b) 0.10 M Ca(NO3)2 (c) 0.10 M Cr(NO3)3

Determine the concentration of the cation and anion in each aqueous solution. (Assume complete dissociation of each compound.) (a) 0.12 M Na2SO4 (b) 0.25 M K2CO3 (c) 0.11 M RbBr

Determine the concentration of the cation and anion in each aqueous solution. (Assume complete dissociation of each compound.) (a) 0.20 M SrSO4 (b) 0.15 M Cr2(SO4)3 (c) 0.12 M SrI2

A 122-mL sample of a 1.2 M sucrose solution is diluted to 500.0 mL. What is the molarity of the diluted solution?

A 3.5-L sample of a 5.8 M NaCl solution is diluted to 55 L. What is the molarity of the diluted solution?

Describe how you would make 2.5 L of a 0.100 M KCl solution from a 5.5 M stock KCl solution.

Describe how you would make 500.0 mL of a 0.200 M NaOH solution from a 15.0 M stock NaOH solution.

To what volume should you dilute 25 mL of a 12 M stock HCl solution to obtain a 0.500 M HCl solution?

To what volume should you dilute 75 mL of a 10.0 M H2SO4 solution to obtain a 1.75 M H2SO4 solution?

How much of a 12.0 M HNO3 solution should you use to make 850.0 mL of a 0.250 M HNO3 solution?

How much of a 5.0 M sucrose solution should you use to make 85.0 mL of a 0.040 M solution?

Determine the volume of 0.150 M NaOH solution required to neutralize each sample of hydrochloric acid. The neutralization reaction is: (a) 25 mL of a 0.150 M HCl solution (b) 55 mL of a 0.055 M HCl solution (c) 175 mL of a 0.885 M HCl solution NaOH1aq2 + HCl1aq2 H2O1l2 + NaCl1aq2

Determine the volume of 0.225 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is: (a) 45 mL of 0.225 M H2SO4 (b) 185 mL of 0.125 M H2SO4 (c) 75 mL of 0.100 M H2SO4 K2SO41aq2 + 2 H2O1l2 H2SO41aq2 + 2 KOH1aq2

Consider the reaction: What volume of 0.225 M K3PO4 solution is necessary to completely react with 134 mL of 0.0112 M NiCl2? Ni31PO4221s2 + 6 KCl1aq2 2 K3PO41aq2 + 3 NiCl21aq2

Consider the reaction: What volume of 0.225 M K2S solution is required to completely react with 175 mL of 0.115 M Co(NO3)2? K2S1aq2 + Co1NO3221aq2 2 KNO31aq2 + CoS1s2

A 10.0-mL sample of an unknown H3PO4 solution requires 112 mL of 0.100 M KOH to completely react with the H3PO4. What was the concentration of the unknown H3PO4 solution? H3PO41aq2 + 3 KOH1aq2 3 H2O1l2 + K3PO41aq2

A 25.0-mL sample of an unknown HClO4 solution requires 45.3 mL of 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is: HClO41aq2 + NaOH1aq2 H2O1l2 + NaClO41aq2

What is the minimum amount of 6.0 M H2SO4 necessary to produce 15.0 g of H2(g) according to the reaction: 2 Al1s2 + 3 H2SO41aq2 Al21SO4231aq2 + 3 H21g2

What is the molarity of ZnCl2(aq) that forms when 15.0 g of zinc completely reacts with CuCl2(aq) according to the following reaction? (Assume a final volume of 175 mL.) Zn1s2 + CuCl21aq2 ZnCl2 + Cu1s2

Calculate the molality of each solution. (a) 0.25 mol solute; 0.250 kg solvent (b) 0.882 mol solute; 0.225 kg solvent (c) 0.012 mol solute; 23.1 g solvent

Calculate the molality of each solution. (a) 0.455 mol solute; 1.97 kg solvent (b) 0.559 mol solute; 1.44 kg solvent (c) 0.119 mol solute; 488 g solvent

Calculate the molality of a solution containing 12.5 g of ethylene glycol (C2H6O2) dissolved in 135 g of water.

Calculate the molality of a solution containing 257 g glucose (C6H12O6) dissolved in 1.62 L of water. (Assume a density of 1.00 g/mL for water.)

Calculate the freezing point of a water solution at each concentration. (a) 0.85 m (b) 1.45 m (c) 4.8 m (d) 2.35 m

Calculate the freezing point of a water solution at each concentration. (a) 0.100 m (b) 0.469 m (c) 1.44 m (d) 5.89 m

Calculate the boiling point of a water solution at each concentration. (a) 0.118 m (b) 1.94 m (c) 3.88 m (d) 2.16 m

Calculate the boiling point of a water solution at each concentration. (a) 0.225 m (b) 2.58 m (c) 4.33 m (d) 6.77 m

A glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g of water. Calculate the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)

An ethylene glycol solution contains 21.2 g of ethylene glycol (C2H6O2) in 85.4 mL of water. Calculate the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)

An NaCl solution is made using 133 g of NaCl and diluting to a total solution volume of 1.00 L. Calculate the molarity and mass percent of the solution. (Assume a density of 1.08 g/mL for the solution.)

A KNO3 solution is made using 88.4 g of KNO3 and diluting to a total solution volume of 1.50 L. Calculate the molarity and mass percent of the solution. (Assume a density of 1.05 g/mL for the solution.)

A 125-mL sample of an 8.5 M NaCl solution is diluted to 2.5 L. What volume of the diluted solution contains 10.8 g of NaCl?

A 45.8-mL sample of a 5.8 M KNO3 solution is diluted to 1.00 L. What volume of the diluted solution contains 15.0 g of KNO3?

To what final volume should you dilute 50.0 mL of a 5.00 M KI solution so that 25.0 mL of the diluted solution contains 3.25 g of KI?

To what volume should you dilute 125 mL of an 8.00 M CuCl2 solution so that 50.0 mL of the diluted solution contains 5.9 g CuCl2?

What is the molarity of an aqueous solution that is 5.88% NaCl by mass? (Assume a density of 1.02 g/mL for the solution.)

What is the molarity of an aqueous solution that is 6.75% glucose (C6H12O6) by mass? (Assume a density of 1.03 g/mL for the solution.)

Consider the reaction: What minimum volume of 4.0 M H2SO4 is required to produce 15.0 L of H2 at STP? 2 Al1s2 + 3 H2SO41aq2 Al21SO4231aq2 + 3 H21g2

Consider the reaction: What minimum amount of 1.85 M HCl is necessary to produce 28.5 L of H2 at STP? Mg1s2 + 2 HCl1aq2 MgCl21aq2 + H21g2

How much of a 1.25 M sodium chloride solution in milliliters is required to completely precipitate all of the silver in 25.0 mL of a 0.45 M silver nitrate solution?

How much of a 1.50 M sodium sulfate solution in milliliters is required to completely precipitate all of the barium in 150.0 mL of a 0.250 M barium nitrate solution?

Nitric acid is usually purchased in concentrated form with a 70.3% HNO3 concentration by mass and a density of 1.41 g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5 L of 0.500 M HNO3?

Hydrochloric acid is usually purchased in concentrated form with a 37.0% HCl concentration by mass and a density of 1.20 g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5 L of 0.500 M HCl?

An ethylene glycol solution is made using 58.5 g of ethylene glycol (C2H6O2) and diluting to a total volume of 500.0 mL. Calculate the freezing point and boiling point of the solution. (Assume a density of 1.09 g/mL for the solution.)

A sucrose solution is made using 144 g of sucrose (C12H22O11) and diluting to a total volume of 1.00 L. Calculate the freezing point and boiling point of the solution. (Assume a density of 1.06 g/mL for the final solution.)

A 250.0-mL sample of a 5.00 M glucose (C6H12O6) solution is diluted to 1.40 L. What are the freezing and boiling points of the final solution? (Assume a density of 1.06 g/mL for the final solution.)

A 135-mL sample of a 10.0 M ethylene glycol (C2H6O2) solution is diluted to 1.50 L. What are the freezing and boiling points of the final solution? (Assume a density of 1.05 g/mL for the final solution.)

An aqueous solution containing 17.5 g of an unknown molecular (nonelectrolyte) compound in 100.0 g of water has a freezing point of . Calculate the molar mass of the unknown compound.

An aqueous solution containing 35.9 g of an unknown molecular (nonelectrolyte) compound in 150.0 g of water has a freezing point of . Calculate the molar mass of the unknown compound.

What is the boiling point of an aqueous solution that freezes at ?

What is the freezing point of an aqueous solution that boils at 102.1 C?

A 125-g sample contains only glucose (C6H12O6) and sucrose (C12H22O11). When the sample is added to 0.500 kg of pure water, the resulting solution has a freezing point of . What were the masses of glucose and sucrose in the original sample?

A 13.03-g sample contains only ethylene glycol (C2H6O2) and propylene glycol (C3H8O2). When the sample is added to 100.0 g of pure water, the resulting solution has a freezing point of . What was the percent composition of ethylene glycol and propylene glycol in the original sample?

Consider the molecular views of osmosis cells. For each cell, determine the direction of water flow.

What is wrong with this molecular view of a sodium chloride solution? What would make the picture correct?

The Safe Drinking Water Act (SDWA) sets a limit for mercurya toxin to the central nervous systemat 0.002 mg/L. Water suppliers must periodically test their water to ensure that mercury levels do not exceed 0.002 mg/L. Suppose water became contaminated with mercury at twice the legal limit (0.004 mg/L). How much of this water would have to be consumed to ingest 0.100 g of mercury?

Water softeners often replace calcium ions in hard water with sodium ions. Since sodium compounds are soluble, the presence of sodium ions in water does not result in the white, scaly residues caused by calcium ions. However, calcium is more beneficial to human health than sodium. Calcium is a necessary part of the human diet, while high levels of sodium intake are linked to increases in blood pressure. The Food and Drug Administration (FDA) recommends that adults ingest less than 2.4 g of sodium per day. How many liters of softened water, containing a sodium concentration of 0.050% sodium by mass, have to be consumed to exceed the FDA recommendation? (Assume a density of 1.0 g/mL for water.)