SCH 3U Workbook Answer Key - Unit 3 by Michael Papadimitriou

Francis Libermann Catholic High School Science Department

Grade 11 University Chemistry SCH 3U1 â&#x20AC;&#x201C; Course Workbook Unit 3 Answer Keys

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Types of Solutions – Homework Questions KNOWLEDGE

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Knowledge 1. Name the two basic components of a solution. solute and solvent 2. Give examples of each type of solution. (a) solid solution (b) liquid solution (c) gaseous solution (at room temperature) (a) steel, bronze, brass (b) methanol in water, vinegar (c) air 3. Explain the term “homogeneous mixture.” Only one phase can be seen in a solution, but it can be separated by physical means such as evaporation. 4. Give examples of each type of mixture. (a) homogeneous mixture (b) mechanical mixture (heterogeneous mixture) (a) apple juice (homogeneous) (b) soil (heterogeneous) 5. Distinguish between the following terms: soluble, miscible, and immiscible. Soluble indicates that a certain amount of solute will dissolve in a given amount of solvent. Miscible refers to two liquids that will mix together in any amount. Immiscible refers to liquids that will not dissolve in each other. 6. Distinguish between an alloy and an amalgam. Give one example of each. An alloy is a mixture of two or more metals that have been melted and mixed together in some proportion and then allowed to solidify. Bronze, brass, and white gold are examples. An amalgam is an alloy of a lesser amount of liquid mercury in a greater amount of silver solvent. Dentists have used this combination to fill cavities. Today plastic solutes are dissolved in silver to perform the same function. 7. What type of solute dissolves in a polar solvent, such as water? Give an example. Ionic solids dissolve best in polar solvents such as water. Examples are KBr and NaCl. 8. Two different clear, colourless liquids were gently heated in an evaporating dish. Liquid A left no residue, while liquid B left a white residue. Which liquid was a solution, and which was a pure substance? Explain your answer. Liquid A was the pure substance as it left no residue showing that it is composed of only one substance; liquid B was a solution containing solutes that did not evaporate but were left behind as a residue.

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – Limiting reactants – Science Department

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Thinking 9. Potassium bromate, KBrO3, is sometimes added to bread dough to make it easier to work with. Suppose that you are given an aqueous solution of potassium bromate. How can you determine if the solution is saturated or unsaturated? If a crystal of potassium bromate is added to the solution, it will dissolve if the solution is unsaturated and if it is saturated, and will not dissolve if the solution is saturated. 10. You are given three liquids. One is a pure substance, and the second is a solution of two miscible liquids. The third is a solution composed of a solid solute dissolved in a liquid solvent. Describe the procedure you would follow to distinguish between the three solutions. If you boil the pure substance, nothing will remain. If you boil the miscible liquids, one liquid will evaporate, while the other will remain. If you boil the solution, only a solid will remain.

Communication 11. How do the properties of a homogeneous mixture differ from the properties of a heterogeneous mixture, or mechanical mixture? Use diagrams to explain. Homogeneous mixture is one phase and heterogeneous is two or more phases

Application 12. In 1989, the oil tanker Exxon Valdez struck a reef in Prince William Sound, Alaska. The accident released 40 million litres of crude oil. The oil eventually covered 26 000 km2 of water. a.) Explain why very little of the spilt oil dissolved in the water. b.) How do you think most of the oil from a tanker accident is dispersed over time? Why would this have been a slow process in Prince William Sound? a.) Oil is nonpolar substance that does not dissolve in seawater, a polar solvent. b.) Wave action dispersed the oil. Prince William Sound has less wave action than the open sea, and the lesser wave action slowed the progress of the oil. 13. Food colouring is often added to foods such as candies, ice cream, and icing. Are food colouring dyes more likely to be polar or non-polar molecules? Explain your answer. Food colouring would be a nonpolar molecule since it is added to foods like candies, ice cream and icing which all have high fat content. Fat molecules are nonpolar and will be able to dissolve the food colouring as a result.

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit â&#x20AC;&#x201C; Limiting reactants â&#x20AC;&#x201C; Science Department

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Factors that Affect Solubility & Dissolving – Homework Questions KNOWLEDGE

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Knowledge 1. Describe the particle attractions that occur as sodium chloride dissolves in water. _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ 2. When water vaporizes, which type of attraction, intramolecular or intermolecular, is broken? Explain. _______________________________________________________________________________ _______________________________________________________________________________ 3. Describe the effect of increasing temperature on the solubility of: a.) a typical solid in water __________________________________________________________ b.) a gas in water _________________________________________________________________ 4. Sugar is more soluble in water than salt. Why does a salt solution (brine) conduct electricity, while a sugar solution does not? _______________________________________________________________________________ _______________________________________________________________________________ 5. Dissolving a certain solute in water releases heat. Dissolving a different solute in water absorbs heat. Explain why. _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – Factors Affecting Solubility & Dissolving – Science Department

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Thinking 6. The graph below shows the solubility of various substances plotted against the temperature of the solution. a.) Which substance decreases in solubility as the temperature increases? _____________________________________ b.) Which substance is least soluble at room temperature? Which substance is most soluble at room temperature? _____________________________________ c.) The solubility of which substance is least affected by a change in temperature? _____________________________________ d.) At what temperature is the solubility of potassium chlorate equal to 40 g/100 g of water? _____________________________________ e.) 20 mL of a saturated solution of potassium nitrate at 50°C is cooled to 20°C. Approximately what mass of solid will precipitate from the solution? Why is it not possible to use the graph to interpolate an accurate value? _______________________________________________________________________________ _______________________________________________________________________________

Application 7. Would you expect to find more mineral deposits near a thermal spring or near a cool mountain spring? Explain. _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – Factors Affecting Solubility & Dissolving – Science Department

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The Concentration of Solutions – Practice Questions KNOWLEDGE

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Knowledge 1. What is the concentration in percent (m/v) of each solution? a.) 14.2 g of potassium chloride, KCl (used as a salt substitute), dissolved in 450.0 mL of solution

b.) 31.5 g of calcium nitrate, Ca(NO3)2 (used to make explosives), dissolved in 1.80 L of solution

c.) 1.72 g of potassium permanganate, KMnO4 (used to bleach stone-washed blue jeans), dissolved in 60.0 mL of solution

2. A solution of hydrochloric acid was formed by dissolving 1.52 g of hydrogen chloride gas in enough water to make 24.1 mL of solution. What is the concentration in percent (m/v) of the solution?

3. At 25°C, a saturated solution of carbon dioxide gas in water has a concentration of 0.145% (m/v). What mass of carbon dioxide is present in 250 mL of the solution?

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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4. Ringer’s solution contains three dissolved salts in the same proportions as they are found in blood. The salts and their concentrations (m/v) are as follows: 0.86% NaCl, 0.030% KCl, and 0.033% CaCl2. Suppose that a patient needs to receive 350 mL of Ringer’s solution by an intravenous drip. What mass of each salt does the pharmacist need to make the solution?

5. Calculate the mass/mass percent of solute for each solution. a.) 17 g of sulfuric acid in 65 g of solution

b.) 18.37 g of sodium chloride dissolved in 92.2 g of water. Hint: Remember that a solution consists of both solute and solvent.

c.) 12.9 g of carbon tetrachloride dissolved in 72.5 g of benzene

6. If 55 g of potassium hydroxide is dissolved in 100.0 g of water, what is the concentration of the solution expressed as mass/mass percent?

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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7. Steel is an alloy of iron and about 1.7% carbon. It also contains small amounts of other materials, such as manganese and phosphorus. What mass of carbon is needed to make a 5.0 kg sample of steel?

8. Stainless steel is a variety of steel that resists corrosion. Your cutlery at home may be made of this material. Stainless steel must contain at least 10.5% chromium. What mass of chromium is needed to make a stainless steel fork with a mass of 60.5 g?

9. 18-carat white gold is an alloy. It contains 75% gold, 12.5% silver, and 12.5% copper. A piece of jewelry, made of 18-carat white gold, has a mass of 20.0 g. How much pure gold does it contain?

10. 60.0 mL of ethanol is diluted with water to a final volume of 400.0 mL. What is the percent by volume of ethanol in the solution?

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit â&#x20AC;&#x201C; The Concentration of Solutions â&#x20AC;&#x201C; Science Department

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11. Milk fat is present in milk. Whole milk usually contains about 5.0% milk fat by volume. If you drink a glass of milk with a volume of 250 mL, what volume of milk fat have you consumed?

12. The average adult human body contains about 5.0 L of blood. Of this volume, only about 0.72% consists of leukocytes (white blood cells). These essential blood cells fight infection in the body. What volume of pure leukocyte cells is present in the body of a small child, with only 2.5 L of blood?

13. Symptoms of mercury poisoning become apparent after a person has accumulated more than 20.0 mg of mercury in the body. a.) Express this amount as parts per million for a 60.0 kg person.

b.) Express this amount as parts per billion.

c.) Express this amount as a (m/m) percent.

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit â&#x20AC;&#x201C; The Concentration of Solutions â&#x20AC;&#x201C; Science Department

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14. The use of the pesticide DDT has been banned in Canada since 1969 because of its damaging effect on wildlife. In 1967, the concentration of DDT in an average lake trout, taken from Lake Simcoe in Ontario, was 16 ppm. Today it is less than 1 ppm. What mass of DDT would have been present in a 2.5 kg trout with DDT present at 16 ppm?

15. The concentration of chlorine in a swimming pool is generally kept in the range of 1.4 to 4.0 mg/L. The water in a certain pool has 3.0 mg/L of chlorine. Express this value as parts per million. (Hint: 1 L of water has a mass of 1000 g.)

16. What is the molar concentration of each solution? a.) 0.50 mol of NaCl dissolved in 0.30 L of solution

b.) 0.289 mol of iron (III) chloride, FeCl3, dissolved in 120 mL of solution

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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c.) 0.0877 mol of copper (II) sulfate, CuSO4, dissolved in 70.0 mL of solution

d.) 4.63 g of sugar, C12H22O11, dissolved in 16.8 mL of solution

e.) 1.2 g of NaNO3 dissolved in 80.0 mL of solution

17. What mass of solute is present in each aqueous solution? a.) 1.00 L of 0.045 mol/L calcium hydroxide, Ca(OH)2, solution

b.) 500.0 mL of 0.100 mol/L silver nitrate, AgNO3 , solution

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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c.) 2.5 L of 1.00 mol/L potassium chromate, K2CrO4, solution

d.) 40.0 mL of 6.0 mol/L sulfuric acid, H2SO4, solution

e.) 4.24 L of 0.775 mol/L ammonium nitrate, NH4NO3, solution.

18. A student dissolves 30.46 g of silver nitrate, AgNO3, in water to make 500.0 mL of solution. What is the molar concentration of the solution?

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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19. What volume of 0.25 mol/L solution can be made using 14 g of sodium hydroxide, NaOH?

20. A 100.0 mL bottle of skin lotion contains a number of solutes. One of these solutes is zinc oxide, ZnO. The concentration of zinc oxide in the skin lotion is 0.915 mol/L. What mass of zinc oxide is present in the bottle?

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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9. 18-carat white gold is an alloy. It contains 75% gold, 12.5% silver, and 12.5% copper. A piece of jewelry, made of 18-carat white gold, has a mass of 20.0 g. How much pure gold does it contain?

10. 60.0 mL of ethanol is diluted with water to a final volume of 400.0 mL. What is the percent by volume of ethanol in the solution?

11. Milk fat is present in milk. Whole milk usually contains about 5.0% milk fat by volume. If you drink a glass of milk with a volume of 250 mL, what volume of milk fat have you consumed?

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit â&#x20AC;&#x201C; The Concentration of Solutions â&#x20AC;&#x201C; Science Department

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13. Symptoms of mercury poisoning become apparent after a person has accumulated more than 20.0 mg of mercury in the body. a.) Express this amount as parts per million for a 60.0 kg person.

b.) Express this amount as parts per billion.

c.) Express this amount as a (m/m) percent.

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit â&#x20AC;&#x201C; The Concentration of Solutions â&#x20AC;&#x201C; Science Department

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16. What is the molar concentration of each solution? a.) 0.50 mol of NaCl dissolved in 0.30 L of solution

b.) 0.289 mol of iron (III) chloride, FeCl3, dissolved in 120 mL of solution

c.) 0.0877 mol of copper (II) sulfate, CuSO4, dissolved in 70.0 mL of solution

d.) 4.63 g of sugar, C12H22O11, dissolved in 16.8 mL of solution

e.) 1.2 g of NaNO3 dissolved in 80.0 mL of solution

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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17. What mass of solute is present in each aqueous solution? a.) 1.00 L of 0.045 mol/L calcium hydroxide, Ca(OH)2, solution

b.) 500.0 mL of 0.100 mol/L silver nitrate, AgNO3 , solution

c.) 2.5 L of 1.00 mol/L potassium chromate, K2CrO4, solution

d.) 40.0 mL of 6.0 mol/L sulfuric acid, H2SO4, solution

e.) 4.24 L of 0.775 mol/L ammonium nitrate, NH4NO3, solution.

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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18. A student dissolves 30.46 g of silver nitrate, AgNO3, in water to make 500.0 mL of solution. What is the molar concentration of the solution?

19. What volume of 0.25 mol/L solution can be made using 14 g of sodium hydroxide, NaOH?

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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Solutions and their Concentrations – Chapter Review KNOWLEDGE

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Knowledge 1. 1. Identify at least two solutions in your home that are a.) beverages _________________________ b.) found in the bathroom or medicine cabinet ____________________________ c.) solids _________________________ 2. How is a solution different from a pure compound? Give specific examples. _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ 3. Mixing 2 mL of linseed oil and 4 mL of turpentine makes a binder for oil paint. What term is used to describe liquids that dissolve in each other? Which liquid is the solvent? _________________________________________________________________________________ _________________________________________________________________________________ 4. How does the bonding in water molecules account for the fact that water is an exellent solvent? _________________________________________________________________________________ _________________________________________________________________________________ 5. Why does an aqueous solution of an electrolyte conduct electricity, but an aqueous solution of a nonelectrolyte does not? _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ 6. Use the concept of forces between particles to explain why oil and water are immiscible. _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ KNOWLEDGE

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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7. Explain the expression “like dissolves like” in terms of intermolecular forces. _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ 8. What factors affect the rate of dissolving of a solid in a liquid? _________________________________________________________________________________ _________________________________________________________________________________ 9. Which of the following substances would you expect to be soluble in water? Briefly explain each answer. a.) potassium chloride, KCl _________________________________________________________________________________ b.) carbon tetrachloride, CCl4 _________________________________________________________________________________ c.) sodium sulfate, Na2SO4 _________________________________________________________________________________ d.) butane, C4H10 _________________________________________________________________________________ 10. Benzene, C6H6, is a liquid at room temperature. It is sometimes used as a solvent. Which of the following compounds is more soluble in benzene: naphthalene, C10H8, or sodium fluoride, NaF? Would you expect ethanol, CH3CH2OH, to be soluble in benzene? Explain your answers. _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________

Thinking 11. Boric acid solution is used as an eyewash. What mass of boric acid is present in 250 g of solution that is 2.25% (m/m) acid in water?

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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12. 10.0% (m/m) sodium hydroxide solution, NaOH(aq), is used to break down wood fibre to make paper. a.) What mass of solute is needed to make 250 mL of 10.0% (m/m) solution?

b.) What mass of solvent is needed?

c.) What is the molar concentration of the solution?

13. What volume of pure ethanol is needed to make 800.0 mL of a solution of ethanol in water that is 12% (v/v)?

14. Some municipalities add sodium fluoride, NaF, to drinking water to help protect the teeth of children. The concentration of sodium fluoride is maintained at 2.9×10–5 mol/L. What mass (in mg) of sodium fluoride is dissolved in 1 L of water? Express this concentration in ppm.

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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15. A saturated solution of sodium acetate, NaCH3COO, can be prepared by dissolving 4.65 g in 10.0 mL of water at 20.0°C. What is the molar concentration of the solution?

16. What is the molar concentration of each of the following solutions? a.) 7.25 g of silver nitrate, AgNO3, dissolved in 100.0 mL of solution

b.) 80.0 g of glucose, C6H12O6, dissolved in 70.0 mL of solution

17. Calculate the mass of solute that is needed to prepare each solution below. a.) 250 mL of 0.250 mol/L calcium acetate, Ca(CH3COO)2

b.) 1.8 L of 0.35 mol/L ammonium sulfate, (NH4)2SO4

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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18. Calculate the molar concentration of each solution formed after dilution. a.) 20.0 mL of 6.0 mol/L hydrochloric acid, HCl(aq), diluted to 70.0 mL

b.) 300.0 mL of 12.0 mol/L ammonia, NH3(aq), diluted to 2.50 L

19. Calculate the molar concentration of each solution. Assume that the volumes can be added. a.) 85.0 mL of 1.50 mol/L ammonium chloride, NH4Cl(aq), added to 250 mL of water

b.) a 1:3 dilution of 1.0 mol/L calcium phosphate (that is, one part stock solution mixed with three parts water)

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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20. A standard solution of 0.250 mol/L calcium ion is prepared by dissolving solid calcium carbonate in an acid. What mass of calcium carbonate is needed to prepare 1.00 L of the solution?

21. Suppose that your teacher gives you three test tubes. Each test tube contains a clear, colourless liquid. One liquid is an aqueous solution of an electrolyte. Another liquid is an aqueous solution of a nonelectrolyte. The third liquid is distilled water. Outline the procedure for an experiment to identify which liquid is which. _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ 22. Fertilizers for home gardeners may be sold as aqueous solutions. Suppose that you want to begin a company that sells an aqueous solution of potassium nitrate, KNO3, fertilizer. You need a solubility curve (a graph of solubility versus temperature) to help you decide what concentration to use for your solution. Describe an experiment that you might perform to develop a solubility curve for potassium nitrate. State which variables are controlled, which are varied, and which must be measured. _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit â&#x20AC;&#x201C; The Concentration of Solutions â&#x20AC;&#x201C; Science Department

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23. Potassium alum, KAl(SO4)212H2O , is used to stop bleeding from small cuts. The solubility of potassium alum, at various temperatures, is given in the following table.

a.) Plot a graph of solubility against temperature. b.) From your graph, interpolate the solubility of potassium alum at 67°C. _________________________________________________________________________________ c.) By extrapolation, estimate the solubility of potassium alum at 82°C. _________________________________________________________________________________ d.) Look at your graph. At what temperature will 120 g of potassium alum form a saturated solution in 100 g of water? _________________________________________________________________________________ 24. What minimum temperature is required to dissolve 24 g of potassium nitrate in 40.0 g of water?

25. A teacher wants to dilute 200 mL of 12 mol/L hydrochloric acid to make a 1 mol/L solution. What safety precautions should the teacher take? _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ KNOWLEDGE

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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Communication 26. Suppose that you make a pot of hot tea. Later, you put a glass of the tea in the refrigerator to save it for a cool drink. When you take it out of the refrigerator some hours later, you notice that it is cloudy. How could you explain this to a younger brother or sister? _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ 27. Define each concentration term: a.) percent (m/v) __________________________________________________________________ b.) percent (m/m) __________________________________________________________________ c.) percent (v/v) ___________________________________________________________________ d.) parts per million, ppm ___________________________________________________________ e.) parts per billion, ppb ____________________________________________________________ 28. The concentration of iron in the water that is supplied to a town is 0.25 mg/L. Express this in ppm and ppb.

29. Ammonia is a gas at room temperature and pressure, but it can be liquefied easily. Liquid ammonia is probably present on some planets. Scientists speculate that it might be a good solvent. Explain why, based on the structure of the ammonia molecule shown above. _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ 30. At 20°C, the solubility of oxygen in water is more than twice that of nitrogen. A student analyzed the concentration of dissolved gases in an unpolluted pond. She found that the concentration of nitrogen gas was greater than the concentration of oxygen. Prepare an explanation for the student to give to her class. _________________________________________________________________________________ _________________________________________________________________________________

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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31. What is the concentration of pure water?

Application 32. A bright red mineral called cinnabar has the chemical formula HgS. It can be used to make an artist’s pigment, but it is a very insoluble compound. A saturated solution at 25°C has a concentration of 2×10 – 27 mol/L. In the past, why was heavy metal poisoning common in painters? Why did painters invariably waste more cinnabar than they used? _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ 33. Vitamin A is a compound that is soluble in fats but not in water. It is found in certain foods, including yellow fruit and green vegetables. In parts of central Africa, children frequently show signs of vitamin A deficiency, although their diet contains a good supply of the necessary fruits and vegetables. Why? _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________ _________________________________________________________________________________

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – The Concentration of Solutions – Science Department

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Precipitate Reaction Predictions – Worksheet KNOWLEDGE

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Using the general solubility guidelines from your text write YES if a precipitate forms and NO if a precipitate does not form.

Set A !

Ba(NO3)2

BaCl2

Na2CrO4

NaNO3

K2CrO4

KCl

Ba(NO3)2

BaCl2

Na2CrO4

NaNO3

K2CrO4

KCl

Na2SO4

MgCl2

Al2(SO4)3

Ba(NO3)2

Sr(NO3)2

AlCl3

! !

Set B ! Na2SO4 MgCl2

Al2(SO4)3

Ba(NO3)2

Sr(NO3)2

AlCl3

! !

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – Precipitate Reaction Predictions – Science Department

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Making Predictions on Solubility – Chapter Questions KNOWLEDGE

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Knowledge 1. a.) Name the two factors that affect the solubility of an ionic compound in water. __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ b.) Briefly explain how each factor affects solubility. __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ 2. Which would you expect to be less soluble: sodium fluoride, NaF (used in toothpaste), or sodium iodide, NaI (added to table salt to prevent iodine deficiency in the diet)? Explain your answer. __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ 3. Which of the following compounds are soluble in water? a.) calcium sulfide, CaS (used in skin products)

b.) iron(II) sulfate, FeSO4 (used as a dietary supplement)

c.) magnesium chloride, MgCl2 (used as a disinfectant and a food tenderizer)

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – Making Predictions About Solubility – Science Department

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Application

4. Which of the following compounds are insoluble in water? For each compound, relate its solubility to the use described. a.) barium sulfate, BaSO4 (can be used to obtain images of the stomach and intestines because it is opaque to X-rays)

b.) aluminum hydroxide, Al(OH)3 (found in some antacid tablets)

c.) zinc carbonate, ZnCO3 (used in suntan lotions)

Communication 5. Calcium nitrate is used in fireworks. Silver nitrate turns dark when exposed to sunlight. When freshly made, both solutions are clear and colourless. Imagine that someone has prepared both solutions but has not labelled them. You do not want to wait for the silver nitrate solution to turn dark in order to identify the solutions. Name a chemical that can be used to precipitate a silver compound with the silver nitrate solution, but will produce no precipitate with the calcium nitrate solution. State the reason for your choice. __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ 6. Suppose that you discover four dropper bottles containing clear, colourless liquids in your school laboratory. The following four labels lie nearby: • barium, Ba2+

• chloride, Cl–1

• silver, Ag+

• sulfate, SO4–2

Unfortunately the labels have not been attached to the bottles. You decide to number the bottles 1, 2, 3, and 4. Then you mix the solutions in pairs. Three combinations give white precipitates: bottles 1 and 2, 1 and 4, and 2 and 3. Which ion does each bottle contain? __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ KNOWLEDGE

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – Making Predictions About Solubility – Science Department

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Reaction in Aqueous Solutions – Understanding Concepts 1. Communication: Briefly compare the relationships among a chemical formula, a total ionic equation, and a net ionic equation. Use sentences or a graphic organizer. _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ 2. Knowledge: Write a net ionic equation for each double displacement reaction in aqueous solution. a.) tin (II) chloride with potassium phosphate

b.) nickel (II) chloride with sodium carbonate

c.) chromium (III) sulfate with ammonium sulfide

3. Knowledge: For each reaction in question 2, identify the spectator ions.

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FRANCIS LIBERMANN CATHOLIC HIGH SCHOOL Chemistry Unit – Reactions in Aqueous Solutions – Science Department

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Section Review

4. Knowledge: Would you expect a qualitative analysis of a solution to give you the amount of each

Briefly compare the relationships chemical formula, a total ion present? Explain whyamong or whya not. ionic equation, and a net ionic equation. Use sentences or a graphic organizer.

K/U Write a net ionic equation for each double displacement reaction in aqueous solution.

(a) tin(II) chloride with potassium 5. Thinking: A solutionphosphate of limewater,

Ca(OH)2(aq), is basic. It is used to test for the presence of carbon acidic and turns limewater milky. Use a chemical equation to explain what happens during the test. What type of reaction occurs?

dioxide. Carbon dioxide is weakly (b) nickel(II) chloride with sodium carbonate

K/U

For each reaction in question 2, identify the spectator ions.

Identifying Ions in Aqueous Solution

Would you expect a qualitative analysis of a solution to give you the amount of each ion present? Explain why or why not. K/U

Suppose that you have a sample of water. You want to kn ions are dissolved in it. Today technological devices, such spectrometer, make this investigative work fairly simple. devices, however, chemists relied on wet chemical techni experimental tests, such as submitting a sample to a serie displacement reactions. Chemists still use wet chemical t With each reaction, insoluble compounds precipitate out (See Figure 9.6.) This enables the chemist to determine, e identity of one or several ions in the solution. This ion-id process is an example of qualitative analysis. Chemists use a range of techniques for qualitative ana ple, the colour of an aqueous solution can help to identify that it contains. Examine Table 9.3. However, the intensit varies with its concentration in the solution. Also keep in ions are colourless in aqueous solution. For example, the ments from Groups 1 (IA) and 2 (IIA), as well as aluminu most anions, are colourless. So there are limits to the infe make if you rely on solution colour alone. Another qualitative analysis technique is a flame test. ionic compound is placed in a flame. Table 9.4 lists the fl associated with several ions. Notice that all the ions are m flame test is only useful for identifying metallic ions in aq Qualitative analysis challenges a chemist’s creative im chemical understanding. Discover this for yourself in Inv

Knowledge: 6. of the2(aq) name formula of the that forms when aqueous solutions of Ca(OH) A solution limewater,State , is and basic. It is used toprecipitate test for copper (II) sulfate and sodium carbonate are mixed. Write the net ionic equation for the reaction. the presence of carbon dioxide. Carbon dioxide is weakly acidic and Identify the spectator ions. turns limewater milky. Use a chemical equation to explain what happens during the test. What type of reaction occurs? I

State the name and formula of the precipitate that forms when aqueous solutions of copper(II) sulfate and sodium carbonate are mixed. Write the net ionic equation for the reaction. Identify the spectator ions.

I All the solutions in this photograph have the same concentration: 0.1 mol/L. Use Table 9.3 to infer which ion causes the colour in each Thinking: solution. How confidence do you in have your inferences? 7. much All the solutions this in photograph have theWhat same concentration: 0.1 mol/L. Use table below to infer which ion causes the colour in each solution. How much confidence do you have in your could you do to increase your confidence?

K/U

inferences? What could you do to increase your confidence?

Table 9.3 The Colour of Some Common Ions in Aqueous Solution

Anions

Cations

Ions

Symbol

Table 9.4 The Flame Colour of Sele

Colour

Ion

chromium (II) copper(II)

Cr2+ Cu2+

blue

chromium(III) copper(I) iron(II) nickel(II)

Cr3+ Cu+ Fe2+ Ni2+

green

iron(III)

Fe3+

pale yellow

Symbol

lithium

Li+

sodium

Na+

potassium

K+

cesium

Cs+

calcium

Ca2+

strontium

Sr2+

barium

Ba2+

cobalt(II) manganese(II)

Co Mn2+

pink

chromate

CrO2! 4

yellow

copper

Cu2+

dichromate

Cr2O2! 7

orange

boron

B2+

permanganate

MnO!4

purple

lead

Pb2+

add precipitating solution

This illustration shows the basic idea behind a Chapter 9 Aqueous qualitative analysis for identifying ions in an aqueous solution. At each stage, the resulting precipitate is removed.

mixture of ions

Figure 9.6

Solutions • MHR

remaining ions

347 precipitate 1

344 MHR • Unit 3 Solutions and Solubility

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Solution Terminology – Worksheet KNOWLEDGE

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Choose the correct term for each blank space from the list shown below.

 Conductor

 Double displacement

 Net ionic equation

 Ionic equation

 Metallic

 Soluble

 Stronger

 Less soluble

 Precipitate

 Salt

 Spectator

 Insoluble

1. The experimental evidence that NaCl in aqueous solution is a(n) ________________________ tells us that this salt is an electrolyte. 2. Fe3+(aq) + 3Cl- (aq) + 3Na+ (aq) + 3OH-(aq)  Fe(OH)3(s) + 3Na+(aq) + 3Cl- (aq) is an example of a(n) ________________________ . 3. In the preceding question, the ions, which do not participate in the reaction are called ________________________ ions. 4. Since potassium chloride is a(n) ________________________ , it exists in water solution almost completely as ions. 5. Flame tests can be used to identify many ________________________ ions in solution. 6. Spectator ions are not included in a(n) ________________________ . 7. ________________________ generally means that more than 1g of solute will dissolve in 100 mL of water at room temperature. 8. The bond between small ions is ________________________ than the bond between large ions with the same charge. 9. Fluoride ions are ________________________ than chlorides, bromides and iodides because the fluoride ion is smaller. 10. The appearance of a ________________________ indicates that an insoluble compound is present. 11. ________________________ means that the solubility is less than 0.1 g per 100 mL water. 12. ________________________ reactions can be recognized by the formation of a precipitate, gas or water.

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Stoichiometry in Solutions Chemistry – Practice Questions KNOWLEDGE

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Thinking 1. Equal volumes of 0.120 mol/L potassium nitrate and 0.160 mol/L iron (III) nitrate are mixed together. What is the concentration of nitrate ions in the mixture?

2. Suppose that you want to remove the barium ions from 120.0 mL of 0.0500 mol/L aqueous barium nitrate solution. What is the minimum mass of sodium carbonate that you should add?

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3. An excess of aluminum foil is added to a certain volume of 0.675 mol/L aqueous copper (II) sulfate solution. The mass of solid copper that precipitates is measured and found to be 4.88 g. What was the volume of the copper (II) sulfate solution?

4. To generate hydrogen gas, a student adds 5.77 g of mossy zinc to 80.1 mL of 4.00 mol/L hydrochloric acid in an Erlenmeyer flask. When the reaction is over, what is the concentration of aqueous zinc chloride in the flask?

5. Copper can be recovered from scrap metal by adding sulfuric acid. Soluble copper sulfate is formed. The copper sulfate then reacts with metallic iron in a single displacement reaction. To simulate this reaction, a student places 1.942 g of iron wool in a beaker that contains 136.3 mL of 0.07500 mol/L aqueous copper (II) sulfate. What mass of copper is formed?

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6. Your stomach secretes hydrochloric acid to help you digest the food you have eaten. If too much HCl is secreted, however, you may need to take an antacid to neutralize the excess. One antacid product contains the compound magnesium hydroxide, Mg(OH)2. a.) Predict the reaction that takes place when magnesium hydroxide reacts with hydrochloric acid.

b.) Imagine that you are a chemical analyst testing the effectiveness of antacids. If 0.10 mol/L HCl(aq) serves as your model for stomach acid, how many litres will react with an antacid that contains 0.10 g of magnesium hydroxide?

7. Even though lead is toxic, many lead compounds are still used as paint pigments (colourings). What volume of 1.50 mol/L lead (II) acetate contains 0.400 mol Pb2+ ions.

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Acid–Base Theories – Practice Problems KNOWLEDGE

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Thinking – Suppose that you have four unknown solutions,

labelled A, B, C, and D. You use a conductivity apparatus to test their conductivity, and obtain the results shown below. Use these results to answer the questions that follow.

a.) Which of these solutions has a high concentration of dissolved ions? What is your evidence?

b.) Which of these solutions has a low concentration of dissolved ions? What is your evidence?

c.) Which of the four unknowns are probably aqueous solutions of acids or bases?

d.) Based on these tests alone, can you distinguish the acidic solution(s) from the basic solutions(s)? Why or why not?

e.) Suggest one way that you could distinguish the acidic solution(s) from the basic solution(s).

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Knowledge 2.

a.) What is the conjugate acid of a base?

b.) What is the conjugate base of an acid?

c.) Use an example to illustrate your answers to parts (a) and (b) above.

3. Write the formula for the conjugate acid of the following: a.) the hydroxide ion, OH– b.) the carbonate ion, CO3–2

4. Write the formula for the conjugate base of the following: a.) nitric acid, HNO3 b.) the hydrogen sulfate ion, HSO4–

5. Which of the following compounds is an acid according to the Arrhenius theory? a.) H2O

b) Ca(OH)2

c.) H3PO3

d.) HF

6. Which of the following compounds is a base according to the Arrhenius theory? a.) KOH

b.) Ba(OH)2

c.) HClO

d.) H3PO4

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Communication – Hydrofluoric acid dissociates in water to form fluoride ions. a.) Write a balanced chemical equation for this reaction.

b.) Identify the conjugate acid-base pairs.

c.) Explain how you know whether or not you have correctly identified the conjugate acid-base pairs.

Thinking – Identify the conjugate acid-base pairs in the following reactions: a.) H2PO4–(aq) + CO3–2(aq)  HPO4–2(aq) + HCO3–(aq)

b.) HCOOH(aq) + CN–(aq)  HCOO–(aq) + HCN(aq)

c.) H2PO4–(aq) + OH–(aq)  HPO4–2(aq) + H2O( ) l

9. Hydrogen cyanide is a poisonous gas at room temperature. When this gas dissolved in water, the following reaction occurs: HCN(aq) + H2O( )  H3O+(aq) + CN–(aq) !

Identify the conjugate acid-base pairs.

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10. Sodium acetate is a good electrolyte. In water, the acetate ion reacts as follows: CH3COO–(aq) + H2O( )  CH3COOH(aq) + OH–(aq) l

Identify the conjugate acid-base pairs.

11. Write equations to show how the hydrogen sulfide ion, HS–, can react with water. First show the ion acting as an acid. Then show the ion acting as a base.

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Strong and Weak Acids & Bases – Understanding Concepts 1. Knowledge: Distinguish, in terms of degree of dissociation, between a strong acid and a weak acid, and a strong base and a weak base. _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ 2. Knowledge: Give one example of the following: a.) a weak acid ___________________

c.) a strong base _____________________

b.) a strong acid __________________

d.) a weak base _____________________

3. Knowledge: Formic acid, HCOOH, is responsible for the painful bites of fire ants. Is formic acid strong or weak? Explain.

4. Knowledge: KMnO4 is an intense purple-coloured solid that can be made into a solution to kill bacteria. What is the name of this compound? Give the name and the formula of the acid that forms when KMnO4 combines with water.

5. Knowledge: State the name or the formula for the acid that forms from each of the following anions: a.) hydrogen sulfate __________________

c.) HS– __________________

b.) F– __________________

d.) hypophosphite __________________

6. Knowledge: Explain the meaning of pH, both in terms of hydrogen ions and hydronium ions.

7. Knowledge: Arrange the following foods in order of increasing acidity: beets, pH = 5.0; camembert cheese, pH = 7.4; egg white, pH = 8.0; sauerkraut, pH = 3.5; yogurt, pH = 4.5.

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8. Thinking: Calculate the pH of each body fluid, given the concentration of hydronium ions. a.) tears, [H3O+] = 4.0x10–8 mol/L

b.) stomach acid, [H3O+] = 4.0x10–2 mol/L

9. Thinking: Calculate the pH of the solution that is formed by diluting 50.0 mL of 0.025 mol/L hydrochloric acid to a final volume of 1.0 L

10. Communication: What is [H3O+] in a solution with pH = 0? Why do chemists not usually use pH to describe [H3O+] when the pH value would be a negative number?

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Acid – Base Reactions – Understanding Concepts 1. Knowledge: Write a generalized word equation to describe what happens during a neutralization reaction.

2. Knowledge: Write a balanced chemical equation for each neutralization reaction. a.) KOH with HNO3

b.) HBr with Ca(OH)2

c.) H3PO4 with NaOH

d.) Mg(OH)2 (the active ingredient in milk of magnesia, an antacid) with HCl (the acid in your stomach)

3. Knowledge: Distinguish between the equivalence point and the end-point in a titration. Why might they be different? How would this affect the result of a titration? _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ _______________________________________________________________________________ 4. Thinking: A 25.0 mL sample of sulfuric acid is completely neutralized by adding 32.8 mL of 0.116 mol/L ammonia solution. Ammonium sulfate, (NH4)2SO4, and water are formed. What is the concentration of the sulfuric acid?

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I A 25.0 mL sample of sulfuric acid is complet adding 32.8 mL of 0.116 mol/L ammonia solutio (NH4)2SO4 , and water are formed. What is the co sulfuric acid?

5. Thinking: The following data were collected during a titration. the concentration of the 5 I Calculate The following data were collected during a ti sodium hydroxide solution.

concentration of the sodium hydroxide solution. Titration Data Volume of HCl(aq)

10.00 mL

Final volume of NaOH(aq)

23.08 mL

Initial volume of NaOH(aq)

1.06 mL

Concentration of HCl(aq) 6

0.235 mol/L

I You should always put the two solutions for in clean, dry beakers. You do not need to dry the which you add the solutions, however, if it has b with distilled water. Explain the difference in th

6. Thinking: You should always put the two solutions for a titration experiment in clean, dry beakers. Suppose that a laboratory technician acciden You do not need to dry the Erlenmeyer flask to which you 7addC the solutions, however, if it has been of a strong acid on her hands, the sleeve thoroughly rinsed with distilled water. Explain the differencesolution in these procedures.

the laboratory bench. Explain how she would de

404 MHR • Unit 3 Solutions and Solubility

7. Communication: Suppose that a laboratory technician accidentally spills a dilute solution of a strong acid on her hands, the sleeve of her lab coat, and the laboratory bench. Explain how she would deal with this spill.

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