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

What is solubility?

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.)

What is a solution? List some examples.

Problem 2Q What is an aqueous solution?

Problem 3Q In a solution, what is the solvent? What is the solute? List some examples.

Problem 4Q Explain what “like dissolves like” means.

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) Table 13.2 Common Laboratory Solvents Common Polar Solvents Common Nonpolar Solvents water \(\mathrm {(H_2O)}\) hexane \(\mathrm {(C_6H_{14})}\) acetone \(\mathrm {(CH_3COCH_3)}\) diethyl ether \(\mathrm {(CH_3CH_2OCH_2CH_3)}\) methyl alcohol \(\mathrm {(CH_3OH)}\) toluene \(\mathrm {(C_7H_8)}\) Equation Transcription: Text Transcription: (H_2O) (CH_3COCH_3) (CH_3OH) (C_6H_{14}) (CH_3CH_2OCH_2CH_3) (C_7H_8)

Pick an appropriate solvent from Table 13.2 to dissolve: (a) glucose (polar) (b) salt (ionic) (c) vegetable oil (nonpolar) (d) sodium nitrate (ionic) Table 13.2 Common Laboratory Solvents Common Polar Solvents Common Nonpolar Solvents water \(\mathrm {(H_2O)}\) hexane \(\mathrm {(C_6H_{14})}\) acetone \(\mathrm {(CH_3COCH_3)}\) diethyl ether \(\mathrm {(CH_3CH_2OCH_2CH_3)}\) methyl alcohol \(\mathrm {(CH_3OH)}\) toluene \(\mathrm {(C_7H_8)}\) Equation Transcription: Text Transcription: (H_2O) (CH_3COCH_3) (CH_3OH) (C_6H_{14}) (CH_3CH_2OCH_2CH_3) (C_7H_8)

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 \(25^{\circ} \mathrm{C}\). Is the solution unsaturated, saturated, or supersaturated? (See Figure \(13.4\).) Figure \(13.4\) Solubility of some ionic solids as a function of temperature Equation Transcription: 25°C Text Transcription: 35 g 25 degree C 13.4

A solution contains \(28 g\) of KNO3 per \(100 g\) of water at \(25^{\circ} \mathrm{C}\). Is the solution unsaturated, saturated, or supersaturated? (See Figure \(13.4\).) Figure \(13.4\) Solubility of some ionic solids as a function of temperature Equation Transcription: KNO3 25°C Text Transcription: 28 g KNO_3 100 g 25 degree C 13.4

A KNO3 solution containing \(45 g\) of KNO3 per \(100 g\) of water is cooled from \(40^{\circ} \mathrm{C}\) to \(0^{\circ} \mathrm{C}\). What happens during cooling? (See Figure \(13.4\).) Figure \(13.4\) Solubility of some ionic solids as a function of temperature Equation Transcription: KNO3 40°C 0°C Text Transcription: 45 g KNO_3 100 g 40 degree C 0 degree C 13.4

A KCl solution containing \(42 g\) of KCl per \(100 g\) of water is cooled from \(60^{\circ} \mathrm{C}\) to \(0^{\circ} \mathrm{C}\). What happens during cooling? (See Figure \(13.4\).) Figure \(13.4\) Solubility of some ionic solids as a function of temperature Equation Transcription: 60°C 0°C Text Transcription: 42 g 100 g 60 degree C 0 degree C 13.4

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

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) \(30.0 \mathrm{g} \ \mathrm{KClO}_{3}\) in \(85.0 g\) of water at \(35^{\circ} \mathrm{C}\) (b) \(65.0 \mathrm{g} \ \mathrm{NaNO}_{3}\) in \(125 g\) of water at \(15^{\circ} \mathrm{C}\) (c) \(32.0 g KCl\) in \(70.0 g\) of water at \(82^{\circ} \mathrm{C}\) Figure \(13.4\) Solubility of some ionic solids as a function of temperature . Equation Transcription: 30.0 g KClO3 35°C 65.0 g NaNO3 15°C 32.0 g KCl 82°C Text Transcription 13.4 30.0 g KClO_3 85.0 g 35 degree C 65.0 g NaNO_3 125 g 15 degree C 32.0 g KCl 70.0 g 82 degree 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) \(45.0 \mathrm{g} \ \mathrm{CaCl}_{2}\) in \(105 g\) of water at \(5^{\circ} \mathrm{C}\) (b) \(15.0 \mathrm{g} \ \mathrm{KClO}_{3}\) in \(115 g\) of water at \(25^{\circ} \mathrm{C}\) (c) \(50.0 \mathrm{g} \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\) in \(95.0 g\) of water at \(10^{\circ} \mathrm{C}\) Figure \(13.4\) Solubility of some ionic solids as a function of temperature Equation Transcription: 45.0 g CaCl2 5°C 15.0 g KClO3 25°C 50.0 g Pb(NO3)2 10°C Text Transcription: 13.4 45.0 g CaCl_2 105 g 5°C 15.0 g KClO_3 115 g 25°C 50.0 g Pb(NO_3)_2 95.0 g

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.

Problem 39P Scuba divers breathing air at increased pressure can suffer from nitrogen narcosis—a condition resembling drunkenness—when 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 toxicity—too much oxygen in the bloodstream—when the partial pressure of oxygen exceeds about 1.4 atm. What happens to the amount of oxygen in a diver’s 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 \(\mathrm {C_{12}H_{22}O_{11}}\) in 498 g \(\mathrm {H_2O}\) (b) 178 mg \(\mathrm {C_6H_{12}O_6}\) in 4.91 g \(\mathrm {H_2O}\) (c) 7.55 g NaCl in 155 g \(\mathrm {H_2O}\) Equation Transcription: Text Transcription: C_{12}H_{22}O_{11} H_2O C_6H_{12}O_6

Calculate the concentration of each solution in mass percent. (a) 132 g KCl in 598 g \(\mathrm {H_2O}\) (b) 22.3 mg \(\mathrm {KNO_3}\) in 2.84 g \(\mathrm {H_2O}\) (c) 8.72 g \(\mathrm {C_2H_6O}\) in 76.1 g \(\mathrm {H_2O}\) Equation Transcription: Text Transcription: H_2O KNO_3 C_2H_6O

A soft drink contains 42 g of sugar in 311 g of \(\mathrm {H_2O}\). What is the concentration of sugar in the soft drink in mass percent? ________________ Equation Transcription: Text Transcription: H_2O

A soft drink contains 32 mg of sodium in 309 g of \(\mathrm {H_2O}\). What is the concentration of sodium in the soft drink in mass percent? Equation Transcription: Text Transcription: H_2O

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

\(\mathrm {AgNO_3}\) 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 \(\mathrm {AgNO_3}\) solution containing 3.4% Ag by mass? (Assume that the density of the solution is 1.01 g/mL.) Equation Transcription: Text Transcription: AgNO_3

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 \(\mathrm {Ca^{2+}}\) 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.) Equation Transcription: Text Transcription: Ca^{2+}

Problem 57P 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.)

Problem 58P 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 \(\mathrm {KNO_3}\) in 0.875 L of solution (c) 1.1 mol of KCl in 2.7 L of solution Equation Transcription: Text Transcription: KNO_3

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 \(\mathrm {C_{12}H_{22}O_{11}}\) in 0.442 L of solution (b) 42.6 g of NaCl in 1.58 L of solution (c) 315 mg of \(\mathrm {C_6H_{12}O_6}\) in 58.2 mL of solution Equation Transcription: Text Transcription: C_{12}H_{22}O_{11} C_6H_{12}O_6

Calculate the molarity of each solution. (a) 33.2 g of KCl in 0.895 L of solution (b) 61.3 g of \(\mathrm {C_2H_6O}\) in 3.4 L of solution (c) 38.2 mg of KI in 112 mL of solution Equation Transcription: Text Transcription: C_2H_6O

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 \(\mathrm {(C_{12}H_{22}O_{11})}\). What is the molarity of the solution with respect to sucrose? Equation Transcription: Text Transcription: (C_{12}H_{22}O_{11})

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 \(\mathrm {KNO_3}\) 22.5 g _____ 125.0 mL _____ \(\mathrm {NaHCO_3}\) _____ _____ 250.0 mL 0.100 M \(\mathrm {C_{12}H_{22}O_{11}}\) 55.38 g _____ _____ 0.150 M Equation Transcription: Text Transcription: KNO_3 NaHCO_3 C_{12}H_{22}O_{11}

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

Calculate the mass of glucose \(\mathrm {(C_6H_{12}O_6)}\) in a 105-mL sample of a 1.02 M glucose solution. Equation Transcription: Text Transcription: (C_6H_{12}O_6)

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 \(\mathrm {KNO_3}\) solution. How much \(\mathrm {KNO_3}\) in grams is needed? Equation Transcription: Text Transcription: KNO_3

Problem 75P How many liters of a 0.500 M sucrose (C12H22O11) solution contain 1.5 kg of sucrose?

Determine the concentration of \(\mathrm {Cl^-}\) in each aqueous solution. (Assume complete dissociation of each compound.) (a) 0.15 M NaCl (b) 0.15 M \(\mathrm {CuCl_2}\) (c) 0.15 M \(\mathrm {AlCl_3}\) Equation Transcription: Text Transcription: Cl^- CuCl_2 AlCl_3

Determine the concentration of \(\mathrm {NO_3^-}\) in each aqueous solution. (Assume complete dissociation of each compound.) (a) 0.10 M \(\mathrm {KNO_3}\) (b) 0.10 M \(\mathrm {Ca(NO_3)_2}\) (c) 0.10 M \(\mathrm {Cr(NO_3)_3}\) Equation Transcription: Text Transcription: NO_3^- KNO_3 Ca(NO_3)_2 Cr(NO_3)_3

Problem 76P What volume of a 0.35 M Mg(NO3)2 solution contains 87 g of Mg(NO3)2?

Problem 79P 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 (a) 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 \(\mathrm {SrSO_4}\) (b) 0.15 M \(\mathrm {Cr_2(SO_4)_3}\) (c) 0.12 M \(\mathrm {SrI_2}\) Equation Transcription: Text Transcription: SrSO_4 Cr_2(SO_4)_3 SrI_2

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.

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 \(\mathrm {H_2SO_4}\) solution to obtain a 1.75 M \(\mathrm {H_2SO_4}\) solution? Equation Transcription: Text Transcription: H_2SO_4

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

How much of a 12.0 M \(\mathrm {HNO_3}\) solution should you use to make 850.0 mL of a 0.250 M \(\mathrm {HNO_3}\) solution? Equation Transcription: Text Transcription: HNO_3

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: \(\mathrm {NaOH}(aq)+\mathrm {HCl}(aq) \longrightarrow \mathrm{H_2O}(l)+\mathrm{NaCl}(aq)\) (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 Equation Transcription: Text Transcription: NaOH(aq)+HCl(aq) rightarrow H_2O(l)+NaCl(aq)

Determine the volume of 0.225 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is: \(\mathrm {H_2SO_4}(aq)+2~\mathrm {KOH}(aq) \longrightarrow \mathrm{K_2SO_4}(aq)+2~\mathrm{H_2O}(l)\) (a) 45 mL of 0.225 M \(\mathrm {H_2SO_4}\) (b) 185 mL of 0.125 M \(\mathrm {H_2SO_4}\) (c) 75 mL of 0.100 M \(\mathrm {H_2SO_4}\) Equation Transcription: Text Transcription: H_2SO_4(aq)+2 KOH(aq) rightarrow K_2SO_4(aq)+2 H_2O(l) H_2SO_4

Consider the reaction: \(2~\mathrm{K_3PO_4}(aq)+3~\mathrm{NiCl_2}(aq) \longrightarrow \mathrm{Ni_3(PO_4)_2}(s)+6~\mathrm{KCl}(aq)\) What volume of 0.225 M \(\mathrm {K_3PO_4}\) solution is necessary to completely react with 134 mL of 0.0112 M \(\mathrm {NiCl_2}\)? Equation Transcription: Text Transcription: 2 K_3PO_4(aq)+3 NiCl2(aq) rightarrow Ni_3(PO_4)_2(s)+6 KCl(aq) K_3PO_4 NiCl_2

Problem 93P 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? H3PO4 (aq) + 3 KOH(aq) ? 3 H2O(l) + K3PO4(aq)

Consider the reaction: \(\mathrm{K}_{2} \mathrm{~S}(a q)+\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow 2 \mathrm{KNO}_{3}(a q)+\operatorname{CoS}(s)\) What volume of 0.225 M \(\mathrm{K}_{2} \mathrm{~S}\) solution is required to completely react with 175 mL of 0.115 M \(\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2} \)?

Problem 94P 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: HClO4(aq) + NaOH(aq) ? H2O(l) + NaClO4(aq)

What is the minimum amount of 6.0 M \(\mathrm {H_2SO_4}\) necessary to produce 15.0 g of \(\mathrm {H_2}(g)\) according to the reaction: \(2~\mathrm{Al}(s)+3~\mathrm{H_2SO_4}(aq) \longrightarrow \mathrm{Al_2(SO_4)_3}(aq)+3~ \mathrm{H_2}(g)\) Equation Transcription: Text Transcription: H_2SO_4 H_2(g) 2 Al(s)+3 H_2SO_4(aq) rightarrow Al_2(SO_4)_3(aq)+3 H_2(g)

What is the molarity of \(\mathrm {ZnCl_2}(aq)\) that forms when 15.0 g of zinc completely reacts with \(\mathrm {CuCl_2}(aq)\) according to the following reaction? (Assume a final volume of 175 mL.) \(\mathrm {Zn}(s)+\mathrm{CuCl_2}(aq) \longrightarrow \mathrm{ZnCl_2+Cu}(s)\) Equation Transcription: Text Transcription: ZnCl_2(aq) CuCl_2(aq) Zn(s)+CuCl_2(aq) rightarrow ZnCl_2+Cu(s)

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 \(\mathrm {(C_2H_6O_2)}\) dissolved in 135 g of water. Equation Transcription: Text Transcription: (C_2H_6O_2)

Calculate the molality of a solution containing 257 g glucose \(\mathrm {(C_6H_{12}O_6)}\) dissolved in 1.62 L of water. (Assume a density of 1.00 g/mL for water.) Equation Transcription: Text Transcription: (C_6H_{12}O_6)

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 \(\mathrm {(C_6H_{12}O_6)}\) 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.) Equation Transcription: Text Transcription: (C_6H_{12}O_6)

An ethylene glycol solution contains 21.2 g of ethylene glycol \(\mathrm {(C_2H_6O_2)}\) 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.) Equation Transcription: Text Transcription: (C_2H_6O_2)

Problem 107P 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.)

Problem 108P 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.)

Problem 109P 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?

Problem 110P 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?

Problem 112P 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 6.75% glucose \(\mathrm {(C_6H_{12}O_6)}\) by mass? (Assume a density of 1.03 g/ mL for the solution.) Equation Transcription: Text Transcription: (C_6H_{12}O_6)

Consider the reaction: \(2~\mathrm{Al}(s)+3~\mathrm{H_2SO_4}(aq) \longrightarrow \mathrm{Al_2(SO_4)_3}(aq)+3~\mathrm{H_2}(g)\) What minimum volume of 4.0 M \(\mathrm {H_2SO_4}\) is required to produce 15.0 L of \(\mathrm {H_2}\) at STP? Equation Transcription: Text Transcription: 2 Al(s)+3 H_2SO_4(aq) rightarrow Al_2(SO_4)_3(aq)+3 H_2(g) H_2SO_4 H_2

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?

Consider the reaction: \(\mathrm{Mg}(s)+2~\mathrm{HCl}(aq) \longrightarrow \mathrm{MgCl_2}(aq)+\mathrm{H_2}(g)\) What minimum amount of 1.85 M HCl is necessary to produce 28.5 L of \(\mathrm H_2\) at STP? Equation Transcription: Text Transcription: Mg(s)+2 HCl(aq) rightarrow MgCl_2(aq)+H_2(g) H_2

Nitric acid is usually purchased in concentrated form with a 70.3% \(\mathrm{HNO_3}\) 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 \(\mathrm{HNO_3}\)? Equation Transcription: Text Transcription: HNO_3

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 \(\mathrm{(C_2H_6O_2)}\) 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.) Equation Transcription: Text Transcription: (C_2H_6O_2)

A sucrose solution is made using 144 g of sucrose \(\mathrm{(C_{12}H_{22}O_{11})}\) 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.) Equation Transcription: Text Transcription: (C_{12}H_{22}O_{11})

A 250.0-mL sample of a 5.00 M glucose \(\mathrm{(C_6H_{12}O_6)}\) 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.) Equation Transcription: Text Transcription: (C_6H_{12}O_6)

An aqueous solution containing 17.5 g of an unknown molecular (nonelectrolyte) compound in 100.0 g of water has a freezing point of \(\mathrm{-1.8~^\circ C}\). Calculate the molar mass of the unknown compound. Equation Transcription: Text Transcription: -1.8^oC

A 135-mL sample of a 10.0 M ethylene glycol \(\mathrm{(C_2H_6O_2)}\) 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.) Equation Transcription: Text Transcription: (C_2H_6O_2)

An aqueous solution containing 35.9 g of an unknown molecular (nonelectrolyte) compound in 150.0 g of water has a freezing point of \(\mathrm{-1.3~^\circ C}\). Calculate the molar mass of the unknown compound.

What is the boiling point of an aqueous solution that freezes at \(\mathrm{-6.7~^\circ C}\)? Equation Transcription: Text Transcription: -6.7^oC

A 125-g sample contains only glucose \(\mathrm{(C_6H_{12}O_6)}\) and sucrose \(\mathrm{(C_{12}H_{22}O_{11})}\). When the sample is added to 0.500 kg of pure water, the resulting solution has a freezing point of \(\mathrm{-1.75~^\circ C}\). What were the masses of glucose and sucrose in the original sample? Equation Transcription: Text Transcription: (C_6H_{12}O_6) (C_{12}H_{22}O_{11}) -1.75 ^oC

What is the freezing point of an aqueous solution that boils at \(\mathrm{102.1~^\circ C}\)? Equation Transcription: Text Transcription: 102.1 ^oC

A 13.03-g sample contains only ethylene glycol \(\mathrm{(C_2H_6O_2)}\) and propylene glycol \(\mathrm{(C_3H_8O_2)}\). When the sample is added to 100.0 g of pure water, the resulting solution has a freezing point of \(\mathrm{-3.50~ ^\circ C}\). What was the percent composition of ethylene glycol and propylene glycol in the original sample? Equation Transcription: Text Transcription: (C_2H_6O_2) (C_3H_8O_2) -3.50 ^oC

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

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

The Safe Drinking Water Act (SDWA) sets a limit for mercury—a toxin to the central nervous system—at \(0.002 mg/L\). Water suppliers must periodically test their water to ensure that mercury levels do not exceed \(0.002 mg/L\). Suppose water is contaminated with mercury at twice the legal limit (0.004 mg/L). How much of this water would a person have to consume to ingest \(0.100 g\) of mercury? Drinking water must be tested for the presence of various pollutants, including mercury compounds that can damage the nervous system. Equation Transcription: Text Transcription: 0.002 mg/L 0.100 g