Compare and Contrast Make a table that compares the

Explain Use the properties of seawater to describe the characteristics of mixtures.

Distinguish between suspensions and colloids.

Identify the various types of solutions. Describe the characteristics of each type of solution.

Explain Use the Tyndall effect to explain why it is more difficult to drive through fog using high beams than using low beams.

Describe different types of colloids.

Explain Why do dispersed colloid particles stay dispersed?

Summarize What causes Brownian motion?

Compare and Contrast Make a table that compares the properties of suspensions, colloids, and solutions.

What is the percent by mass of NaHC O 3 in a solution containing 20.0 g of NaHC O 3 dissolved in 600.0 mL of H 2O?

You have 1500.0 g of a bleach solution. The percent by mass of the solute sodium hypochlorite (NaOCl) is 3.62%. How many grams of NaOCl are in the solution?

In Question 10, how many grams of solvent are in the solution?

Challenge The percent by mass of calcium chloride in a solution is found to be 2.65%. If 50.0 g of calcium chloride is used, what is the mass of the solution?

What is the percent by volume of ethanol in a solution that contains 35 mL of ethanol dissolved in 155 mL of water?

What is the percent by volume of isopropyl alcohol in a solution that contains 24 mL of isopropyl alcohol in 1.1 L of water?

Challenge If 18 mL of methanol is used to make an aqueous solution that is 15% methanol by volume, how many milliliters of solution is produced?

What is the molarity of an aqueous solution containing 40.0 g of glucose ( C 6H 12O 6) in 1.5 L of solution?

Calculate the molarity of 1.60 L of a solution containing 1.55 g of dissolved KBr.

What is the molarity of a bleach solution containing 9.5 g of NaOCl per liter of bleach?

Challenge How much calcium hydroxide (Ca(OH ) 2), in grams, is needed to produce 1.5 L of a 0.25M solution?

How many grams of CaC l 2 would be dissolved in 1.0 L of a 0.10M solution of CaC l 2?

How many grams of CaC l 2 should be dissolved in 500.0 mL of water to make a 0.20M solution of CaC l 2?

How much NaOH are in 250 mL of a 3.0M NaOH solution?

Challenge What volume of ethanol ( C 2H 3OH) is in 100.0 mL of 0.15M solution? The density of ethanol is 0.7893 g/mL.

What volume of a 3.00M KI stock solution would you use to make 0.300 L of a 1.25M KI solution?

How many milliliters of a 5.0M H 2S O 4 stock solution would you need to prepare 100.0 mL of 0.25M H 2S O 4?

Challenge If 0.5 L of 5M stock solution of HCl is diluted to make 2 L of solution, how much HCl, in grams, was in the solution?

What is the molality of a solution containing 10.0 g of N a 2S O 4 dissolved in 1000.0 g of water?

Challenge How much (Ba (OH ) 2), in grams, is needed to make a 1.00m aqueous solution?

What is the mole fraction of NaOH in an aqueous solution that contains 22.8% NaOH by mass?

Challenge If the mole fraction of sulfuric acid ( H 2S O 4) in an aqueous solution is 0.325, how much water, in grams, is in 100 mL of the solution?

Compare and contrast five quantitative ways to describe the composition of solutions

Explain the similarities and differences between a 1M solution of NaOH and a 1m solution of NaOH.

Calculate A can of chicken broth contains 450 mg of sodium chloride in 240.0 g of broth. What is the percent by mass of sodium chloride in the broth?

Solve How much ammonium chloride (N H 4 Cl), in grams, is needed to produce 2.5 L of a 0.5M aqueous solution?

Outline the laboratory procedure for preparing a specific volume of a dilute solution from a concentrated stock solution.

If 0.55 g of a gas dissolves in 1.0 L of water at 20.0 kPa of pressure, how much will dissolve at 110.0 kPa of pressure?

A gas has a solubility of 0.66 g/L at 10.0 atm of pressure. What is the pressure on a 1.0-L sample that contains 1.5 g of gas?

Challenge The solubility of a gas at 7 atm of pressure is 0.52 g/L. How many grams of the gas would be dissolved per 1 L if the pressure was raised to 10 atm?

Describe factors that affect the formation of solutions.

Define solubility.

Describe how intermolecular forces affect solvation

Explain on a particle basis why the vapor pressure of a solution is lower than a pure solvent.

Sumarize If a seed crystal was added to a supersaturated solution, how would you characterize the resulting solution?

Make and Use Graphs Use the information in Table 14.3 to graph the solubilities of aluminum sulfate, lithium sulfate, and potassium chloride at 0C, 20C, 60C, and 100C. Which substances solubility is most affected by increasing temperature?

What are the boiling point and freezing point of a 0.625m aqueous solution of any nonvolatile, nonelectrolyte solute?

What are the boiling point and freezing point of a 0.40m solution of sucrose in ethanol?

Challenge A 0.045m solution (consisting of a nonvolatile, nonelectrolyte solute) is experimentally found to have a freezing point depression of 0.08C. What is the freezing point depression constant ( K f). Which is most likely to be the solvent: water, ethanol, or chloroform?

Explain the nature of colligative properties

Describe four colligative properties of solutions

Explain why a solution has a lower boiling point than that of the pure solvent.

Solve An aqueous solution of calcium chloride (CaC l 2 ) boils at 101.3C. How many kilograms of calcium chloride were dissolved in 1000.0 g of the solvent?

Calculate the boiling point elevation of a solution containing 50.0 g of glucose ( C 6 H 12 O 6 ) dissolved in 500.0 g of water. Calculate the freezing point depression for the same solution.

Investigate A lab technician determines the boiling point elevation of an aqueous solution of a nonvolatile, nonelectrolyte to be 1.12C. What is the solutions molality?

Explain what is meant by the statement not all mixtures are solutions.

What is the difference between a solute and a solvent?

What is a suspension, and how does it differ from a colloid?

How can the Tyndall effect be used to distinguish between a colloid and a solution? Why?

Name a colloid formed from a gas dispersed in a liquid.

Salad dressing What type of heterogenous mixture is shown in Figure 14.24? What characteristic is most useful in classifying the mixture?

What causes the Brownian motion observed in liquid colloids?

Aerosol sprays are categorized as colloids. Identify the phases of an aerosol spray.

What is the difference between percent by mass and percent by volume?

What is the difference between molarity and molality?

What factors must be considered when creating a dilute solution from a stock solution?

How do 0.5M and 2.0M aqueous solutions of NaCl differ?

Under what conditions might a chemist describe a solution in terms of molality? Why?

According to lab procedure, you stir 25.0 g of MgC l 2 into 550 mL of water. What is the percent by mass of MgC l 2 in the solution?

How many grams of LiCl are in 275 g of a 15% aqueous solution of LiCl?

You need to make a large quantity of a 5% solution of HCl but have only 25 mL HCl. What volume of 5% solution can be made from this volume of HCl?

Calculate the percent by volume of a solution created by adding 75 mL of acetic acid to 725 mL of water.

Calculate the molarity of a solution that contain 15.7 g of CaC O 3 dissolved in 275 mL of water.

What is the volume of a 3.00M solution made with 122 g of LiF?

How many moles of BaS would be used to make 1.5 1 0 3 mL of a 10.0M solution?

How much CaC l 2 , in grams, is needed to make 2.0 L of a 3.5M solution?

Stock solutions of HCl with various molarities are frequently prepared. Complete Table 14.7 by calculating the volume of concentrated, or 12M, hydrochloric acid that should be used to make 1.0 L of HCl solution with each molarity listed. Table 14.7 HCl Solutions Molarity of HCl Desired Volume of 12M HCl Stock Solution Needed (mL) 0.5 1.0 1.5 2.0 5.0

How much of 5.0M nitric acid (HN O 3 ), in milliliters, is needed to make 225 mL of 1.0M HN O 3 ?

Experiment In the lab, you dilute 55 mL of a 4.0M solution to make 250 mL of solution. Calculate the molarity of the new solution.

How many milliliters of 3.0M phosphoric acid ( H 3 P O 4 ) can be made from 95 mL of a 5.0M H 3 P O 4 solution?

If you dilute 20.0 mL of a 3.5M solution to make 100.0 mL of solution, what is the molarity of the dilute solution?

What is the molality of a solution that contain 75.3 g of KCl dissolved in 95.0 g of water?

How many grams of N a 2 C O 3 must be dissolved into 155 g of water to create a solution with a molality of 8.20 mol/kg?

What is the molality of a solution containing 30.0 g of naphthalene ( C 10 H 8 ) dissolved in 500.0 g of toluene?

What are the molality and mole fraction of solute in a 35.5 percent by mass aqueous solution of formic acid (HCOOH)?

What is the mole fraction of H 2 S O 4 in a solution containing the percentage of sulfuric acid and water shown in Figure 14.25?

Calculate the mole fraction of MgC l 2 in a solution created by dissolving 132.1 g of MgC l 2 in 175 mL of water.

Describe the process of solvation.

What are three ways to increase the rate of solvation?

Explain the difference between saturated and unsaturated solutions.

At a pressure of 1.5 atm, the solubility of a gas is 0.54 g/L. Calculate the solubility when the pressure is doubled.

At 4.5 atm of pressure, the solubility of a gas is 9.5 g/L. How much gas, in grams, will dissolve in 1 L if the pressure is reduced by 3.5 atm?

Using Figure 14.26, compare the solubility of potassium bromide (KBr) and potassium nitrate (KN O 3 ) at 80C.

The solubility of a gas at 37.0 kPa is 1.80 g/L. At what pressure will the solubility reach 9.00 g/L?

Use Henrys law to complete Table 14.8. Table 14.8 Solubility and Pressure Solubility (g/L) Pressure (kPa) 2.9 ? 3.7 32 ? 39

Soft Drinks The partial pressure of C O 2 inside a bottle of soft drink is 4.0 atm at 25C. The solubility of C O 2 is 0.12 mol/L. When the bottle is opened, the partial pressure drops to 3.0 1 0 -4 atm. What is the solubility of C O 2 in the open drink? Express your answer in grams per liter.

Define the term colligative property

Use the terms dilute and concentrated to compare the solution on both sides of a membrane.

Identify each variable in the following formula: T b = K bm

Define the term osmotic pressure, and explain why it is considered a colligative property.

Calculate the freezing point of a solution of 12.1 g of naphthalene ( C 10 H 8 ) dissolved in 0.175 kg of benzene ( C 6 H 6 ). Refer to Table 14.6 needed data.

In the lab, you dissolve 179 g of MgC l 2 into 1.00 L of water. Use Table 14.6 to find the freezing point of the solution.

Cooking A cook prepares a solution for boiling by adding 12.5 g of NaCl to a pot holding 0.750 L of water. At what temperature should the solution in the pot boil? Use Table 14.5 for needed data.

The boiling point of ethanol ( C 2 H 5 OH) changes from 78.5C to 85.2C when an amount of naphthalene ( C 10 H 8 ) is added to 1.00 kg of ethanol. How much naphthalene, in grams, is required to cause this change? Refer to Table 14.5 for needed data.

Ice Cream A rock salt (NaCl), ice, and water mixture is used to cool milk and cream to make homemade ice cream. How many grams of rock salt must be added to water to lower the freezing point by 10.0C?

Apply your knowledge of polarity and solubility to predict whether solvation is possible in each situation shown in Table 14.9. Explain your answers. Table 14.9 Is solvation possible? Solute Solvent solid Mg Cl 2 liquid H 2 O liquid N H 3 liquid C 6 H 6 gaseous H 2 liquid H 2 O liquid I 2 liquid Br 2

Household Paint Some types of paint are colloids composed of pigment particles dispersed in oil. Based on what you know about colloids, recommend an appropriate location for storing cans of leftover household paint. Justify your recommendation

Which solute has the greatest effect on the boiling point of 1.00 kg of water: 50.0 g of strontium chloride (SrC l 2 ) or 150.0 g of carbon tetrachloride (CC l 4 )? Justify your answer

Study Table 14.4. Analyze solubility and temperature data to determine the general trend followed by the gases (N H 3 , C O 2 , O 2 ) in the chart. Compare this trend to the trend followed by most of the solids in the chart. Identify the solids listed that do not follow the general trend followed by most of the solids in the chart.

An air sample yields the percent composition shown in Figure 14.27. Calculate the mole fraction for each gas present in the sample.

If you prepared a saturated aqueous solution of potassium chloride at 25C and then heated it to 50C, would you describe the solution as unsaturated, saturated, or supersaturated? Explain.

How many grams of calcium nitrate (Ca(N O 3 ) 2 ) would you need to prepare 3.00 L of a 0.500M solution?

What would be the molality of the solution described in the previous problem?

Develop a plan for making 1000 mL of a 5% by volume solution of hydrochloric acid in water. Your plan should describe the amounts of solute and solvent necessary, as well as the steps involved in making the solution

Compare and Infer Study the phase diagram in Figure 14.21 on page 501. Compare the dotted lines surrounding T f and T b , and describe the differences you observe. How might these lines be positioned differently for solutions of electrolytes and nonelectrolytes? Why?

Extrapolate The solubility of argon in water at various pressures is shown in Figure 14.28. Extrapolate the data to 15 atm. Use Henrys law to verify the solubility determined by your extrapolation

Infer Dehydration occurs when more fluid is lost from the body than is taken in. Scuba divers are advised to hydrate their bodies before diving. Use your knowledge of the relationship between pressure and gas solubility to explain the importance of hydration prior to a dive.

Graph Table 14.10 shows solubility data that was collected in an experiment. Plot a graph of the molarity of KI versus temperature. What is the solubility of KI at 55C? Table 14.10 Solubility of KI Temperature (C) Grams of KI per 100.0 g Solution 20 144 40 162 60 176 80 192 100 206

Design an Experiment You are given a sample of a solid solute and three aqueous solutions containing that solute. How would you determine which solution is saturated, unsaturated, and supersaturated?

Compare Which of the following solutions has the highest concentration? Rank the solutions from the greatest to the smallest boiling point depression. Explain your answer. a. 0.10 mol NaBr in 100.0 mL solution b. 2.1 mol KOH in 1.00 L solution c. 1.2 mol KMn O 4 in 3.00 L solution

Interpret the solubility data in Table 14.11 using the concept of Henrys law. Table 14.11 Measurements of Solubility of a Gas Measurement Solubility 1 0.225 2 0.45 3 0.9 4 1.8 5 3.6

You have a solution containing 135.2 g of dissolved KBr in 2.3 L of water. What volume of this solution, in mL, would you use to make 1.5 L of a 0.1M KBr solution? What is the boiling point of this new solution?

The radius of an argon atom is 94 pm. Assuming the atom is spherical, what is the volume of an argon atom in cubic nanometers ? V = 4/3 r 3 (Chapter 3)

Identify which molecule is polar. (Chapter 8) a. Si H 4 c. H 2 S b. N O 2 d. NC l 3

Name the following compounds. (Chapter 7) a. NaBr b. Pb(C H 3 COO ) 2 c. (N H 4 ) 2 C O 3

A 12.0-g sample of an element contains 5.94 1 0 22 atoms. What is the unknown element? (Chapter 10)

Pure bismuth can be produced by the reaction of bismuth oxide with carbon at high temperatures. 2B i 2 O 3 + 3C 4Bi + 3C O 2 How many moles of B i 2 O 3 reacted to produce 12.6 mol of C O 2 ? (Chapter 11)

Homogenized Milk The first homogenized milk was sold in the United States around 1919. Today, almost all milk sold in this country is homogenized in the form of a colloidal emulsion. Research the homogenization process. Write a brief article describing the process. The article should include a flowchart or diagram of the process, as well as a discussion of the reputed benefits and drawbacks associated with drinking homogenized milk.

Are dissolved oxygen values most closely related to latitude or longitude? Why do you think this is true?

At what latitude are average dissolved oxygen values the lowest?

Describe the general trend defined by the data. Relate the trend to the relationship between gas solubility and temperature.