10.E: Solutions (Exercises)

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The following questions are related to the material covered in this chapter. For additional discussion on each topic, also check the links included in each heading.

9.1: Solutions

Concept Review Exercises

What causes a solution to form?
How does the phrase like dissolves like relate to solutions?

Answers

Solutions form because a solute and a solvent have similar intermolecular interactions.
It means that substances with similar intermolecular interactions will dissolve in each other.

Exercises

Define solution.
Give several examples of solutions.
What is the difference between a solvent and a solute?
Can a solution have more than one solute in it? Can you give an example?
Does a solution have to be a liquid? Give several examples to support your answer.
Give at least two examples of solutions found in the human body.
Which substances will probably be soluble in water, a very polar solvent?
1. sodium nitrate (NaNO₃)
2. hexane (C₆H₁₄)
3. isopropyl alcohol [(CH₃)₂CHOH]
4. benzene (C₆H₆)
Which substances will probably be soluble in toluene (C₆H₅CH₃), a nonpolar solvent?
1. sodium nitrate (NaNO₃)
2. hexane (C₆H₁₄)
3. isopropyl alcohol [(CH₃)₂CHOH]
4. benzene (C₆H₆)
The solubility of alcohols in water varies with the length of carbon chain. For example, ethanol (CH₃CH₂OH) is soluble in water in any ratio, while only 0.0008 mL of heptanol (CH₃CH₂CH₂CH₂CH₂CH₂CH₂OH) will dissolve in 100 mL of water. Propose an explanation for this behavior.
Dimethyl sulfoxide [(CH₃)₂SO] is a polar liquid. Based on the information in Exercise 9, which do you think will be more soluble in it—ethanol or heptanol?

Answers

a homogeneous mixture

2. vinegar, dextrose IV, saline IV, coffee, tea, wine

A solvent is the majority component of a solution; a solute is the minority component of a solution.

4. yes. Coke or Pepsi has sugar, caffeine and carbon dioxide as solutes.

A solution does not have to be liquid; air is a gaseous solution, while some alloys are solid solutions (answers will vary).

6. Urine, plasma

1. probably soluble
2. probably not soluble
3. probably soluble
4. probably not soluble

probably not soluble
probably soluble
probably not soluble
probably soluble

9. Small alcohol molecules have strong polar intermolecular interactions, so they dissolve in water. In large alcohol molecules, the nonpolar end overwhelms the polar end, so they do not dissolve very well in water.

10. Ethanol is a smaller molecule. It will be more soluble in water than heptanol.

9.2: Concentration

Concept Review Exercises

What are some of the units used to express concentration?
Distinguish between the terms solubility and concentration.

Answers

% m/m, % m/v, ppm, ppb, molarity, and Eq/L (answers will vary)
Solubility is typically a limit to how much solute can dissolve in a given amount of solvent. Concentration is the quantitative amount of solute dissolved at any concentration in a solvent.

Exercises

Define solubility. Do all solutes have the same solubility?
Explain why the terms dilute or concentrated are of limited usefulness in describing the concentration of solutions.
If the solubility of sodium chloride (NaCl) is 30.6 g/100 mL of H₂O at a given temperature, how many grams of NaCl can be dissolved in 250.0 mL of H₂O?
If the solubility of glucose (C₆H₁₂O₆) is 120.3 g/100 mL of H₂O at a given temperature, how many grams of C₆H₁₂O₆ can be dissolved in 75.0 mL of H₂O?
How many grams of sodium bicarbonate (NaHCO₃) can a 25.0°C saturated solution have if 150.0 mL of H₂O is used as the solvent?
If 75.0 g of potassium bromide (KBr) are dissolved in 125 mL of H₂O, is the solution saturated, unsaturated, or supersaturated?
Calculate the mass/mass percent of a saturated solution of NaCl. Use the data from Table 9.E.19.E.1 "Solubilities of Various Solutes in Water at 25°C (Except as Noted)", assume that masses of the solute and the solvent are additive, and use the density of H₂O (1.00 g/mL) as a conversion factor.
Calculate the mass/mass percent of a saturated solution of MgCO₃ Use the data from Table 9.E.19.E.1 "Solubilities of Various Solutes in Water at 25°C (Except as Noted)", assume that masses of the solute and the solvent are additive, and use the density of H₂O (1.00 g/mL) as a conversion factor.
Only 0.203 mL of C₆H₆ will dissolve in 100.000 mL of H₂O. Assuming that the volumes are additive, find the volume/volume percent of a saturated solution of benzene in water.
Only 35 mL of aniline (C₆H₅NH₂) will dissolve in 1,000 mL of H₂O. Assuming that the volumes are additive, find the volume/volume percent of a saturated solution of aniline in water.
A solution of ethyl alcohol (C₂H₅OH) in water has a concentration of 20.56% v/v. What volume of C₂H₅OH is present in 255 mL of solution?
What mass of KCl is present in 475 mL of a 1.09% m/v aqueous solution?
The average human body contains 5,830 g of blood. What mass of arsenic is present in the body if the amount in blood is 0.55 ppm?
The Occupational Safety and Health Administration has set a limit of 200 ppm as the maximum safe exposure level for carbon monoxide (CO). If an average breath has a mass of 1.286 g, what is the maximum mass of CO that can be inhaled at that maximum safe exposure level?
Which concentration is greater—15 ppm or 1,500 ppb?
Express the concentration 7,580 ppm in parts per billion.
What is the molarity of 0.500 L of a potassium chromate solution containing 0.0650 mol of K₂CrO₄?
What is the molarity of 4.50 L of a solution containing 0.206 mol of urea [(NH₂)₂CO]?
What is the molarity of a 2.66 L aqueous solution containing 56.9 g of NaBr?
If 3.08 g of Ca(OH)₂ is dissolved in enough water to make 0.875 L of solution, what is the molarity of the Ca(OH)₂?
What mass of HCl is present in 825 mL of a 1.25 M solution?
What mass of isopropyl alcohol (C₃H₈O) is dissolved in 2.050 L of a 4.45 M aqueous C₃H₈O solution?
What volume of 0.345 M NaCl solution is needed to obtain 10.0 g of NaCl?
How many milliliters of a 0.0015 M cocaine hydrochloride (C₁₇H₂₂ClNO₄) solution is needed to obtain 0.010 g of the solute?
Aqueous calcium chloride reacts with aqueous silver nitrate according to the following balanced chemical equation:

CaCl₂(aq) + 2AgNO₃(aq) → 2AgCl(s) + Ca(NO₃)₂(aq)

How many moles of AgCl(s) are made if 0.557 L of 0.235 M CaCl₂ react with excess AgNO₃? How many grams of AgCl are made?
Sodium bicarbonate (NaHCO₃) is used to react with acid spills. The reaction with sulfuric acid (H₂SO₄) is as follows:

2NaHCO₃(s) + H₂SO₄(aq) → Na₂SO₄(aq) + 2H₂O(ℓ) + 2CO₂(g)

If 27.6 mL of a 6.25 M H₂SO₄ solution were spilled, how many moles of NaHCO₃ would be needed to react with the acid? How many grams of NaHCO₃ is this?
The fermentation of glucose to make ethanol and carbon dioxide has the following overall chemical equation:

C₆H₁₂O₆(aq) → 2C₂H₅OH(aq) + 2CO₂(g)

If 1.00 L of a 0.567 M solution of C₆H₁₂O₆ were completely fermented, what would be the resulting concentration of the C₂H₅OH solution? How many moles of CO₂ would be formed? How many grams is this? If each mole of CO₂ had a volume of 24.5 L, what volume of CO₂ is produced?
Aqueous sodium bisulfite gives off sulfur dioxide gas when heated:

2NaHSO₃(aq) → Na₂SO₃(aq) + H₂O(ℓ) + SO₂(g)

If 567 mL of a 1.005 M NaHSO₃ solution were heated until all the NaHSO₃ had reacted, what would be the resulting concentration of the Na₂SO₃ solution? How many moles of SO₂ would be formed? How many grams of SO₂ would be formed? If each mole of SO₂ had a volume of 25.78 L, what volume of SO₂ would be produced?
What is the concentration of a 1.0 M solution of K⁺(aq) ions in equivalents/liter?
What is the concentration of a 1.0 M solution of SO₄²⁻(aq) ions in equivalents/liter?
A solution having initial concentration of 0.445 M and initial volume of 45.0 mL is diluted to 100.0 mL. What is its final concentration?
A 50.0 mL sample of saltwater that is 3.0% m/v is diluted to 950 mL. What is its final mass/volume percent?

Answers

Solubility is the amount of a solute that can dissolve in a given amount of solute, typically 100 mL. The solubility of solutes varies widely.

2. The term dilute means relatively less solute and the term concentrated implies relatively more solute. Both are of limited usefulness because these are not accurate.

3. 76.5 g

4. 90.2 g

5. 12.6 g

6. unsaturated

7. 26.5%

8. 2.15%

9. 0.203%

10. 3.4%

11. 52.4 mL

12. 5.18 g

13. 0.00321 g

14. 2.57 x 10^-4g

15. 15 ppm

16. 7,580,000 ppb

17. 0.130 M

18. 0.0458 M

19. 0.208 M

20. 0.0475 M

21. 37.6 g

22. 548 g

23. 0.496 L

24. 20 mL

25. 0.262 mol; 37.5 g

26. 0.345 mol; 29.0 g

27. 1.13 M C₂H₅OH; 1.13 mol of CO₂; 49.7 g of CO₂; 27.7 L of CO₂

28. 0.503 M Na₂SO₃; 0.285 mol SO₂; 18.3 g SO₂; 471 L SO₂

29. 1.0 Eq/L

30. 2.0 Eq/L

31. 0.200 M

32. 0.16 % m/v

9.3: The Dissolution Process

Concept Review Exercise

Explain how the solvation process describes the dissolution of a solute in a solvent.

Answer

Each particle of the solute is surrounded by particles of the solvent, carrying the solute from its original phase.

Exercises

Describe what happens when an ionic solute like Na₂SO₄ dissolves in a polar solvent.
Describe what happens when a molecular solute like sucrose (C₁₂H₂₂O₁₁) dissolves in a polar solvent.
Classify each substance as an electrolyte or a nonelectrolyte. Each substance dissolves in H₂O to some extent.
1. NH₄NO₃
2. CO₂
3. NH₂CONH₂
4. HCl
Classify each substance as an electrolyte or a nonelectrolyte. Each substance dissolves in H₂O to some extent.
1. CH₃CH₂CH₂OH
2. Ca(CH₃CO₂)₂
3. I₂
4. KOH
Will solutions of each solute conduct electricity when dissolved?
1. AgNO₃
2. CHCl₃
3. BaCl₂
4. Li₂O
Will solutions of each solute conduct electricity when dissolved?
1. CH₃COCH₃
2. N(CH₃)₃
3. CH₃CO₂C₂H₅
4. FeCl₂

Answers

Each ion of the ionic solute is surrounded by particles of solvent, carrying the ion from its associated crystal.

2. Each sucrose molecule is surrounded by solvent molecules (attracted to each other via intermolecular forces of attraction).

1. electrolyte
2. nonelectrolyte
3. nonelectrolyte
4. electrolyte

nonelectrolyte
electrolyte
nonelectrolyte
electrolyte

a. no

b. no

c. no

d. yes

9.4: Properties of Solutions

Concept Review Exercises

What are the colligative properties of solutions?
Explain how the following properties of solutions differ from those of the pure solvent: vapor pressure, boiling point, freezing point, and osmotic pressure.

Answers

Colligative properties are characteristics that a solution has that depend on the number, not the identity, of solute particles.
In solutions, the vapor pressure is lower, the boiling point is higher, the freezing point is lower, and the osmotic pressure is higher.

Exercises

In each pair of aqueous systems, which will have the lower vapor pressure?
1. pure water or 1.0 M NaCl
2. 1.0 M NaCl or 1.0 M C₆H₁₂O₆
3. 1.0 M CaCl2CaCl2 or 1.0 M (NH₄)₃PO₄
In each pair of aqueous systems, which will have the lower vapor pressure?
1. 0.50 M Ca(NO₃)₂ or 1.0 M KBr
2. 1.5 M C₁₂H₂₂O₁₁ or 0.75 M Ca(OH)₂
3. 0.10 M Cu(NO₃)₂ or pure water
In each pair of aqueous systems, which will have the higher boiling point?
1. pure water or a 1.0 M NaCl
2. 1.0 M NaCl or 1.0 M C₆H₁₂O₆
3. 1.0 M CaCl2CaCl2 or 1.0 M (NH₄)₃PO₄
In each pair of aqueous systems, which will have the higher boiling point?
1. 0.50 M Ca(NO₃)₂ or 1.0 M KBr
2. 1.5 M C₁₂H₂₂O₁₁ or 0.75 M Ca(OH)₂
3. 0.10 M Cu(NO₃)₂ or pure water
Estimate the boiling point of each aqueous solution. The boiling point of pure water is 100.0°C.
1. 0.50 M NaCl
2. 1.5 M Na₂SO₄
3. 2.0 M C₆H₁₂O₆
Estimate the freezing point of each aqueous solution. The freezing point of pure water is 0.0°C.
1. 0.50 M NaCl
2. 1.5 M Na₂SO₄
3. 2.0 M C₆H₁₂O₆
Explain why salt (NaCl) is spread on roads and sidewalks to inhibit ice formation in cold weather.
Salt (NaCl) and calcium chloride (CaCl2) are used widely in some areas to minimize the formation of ice on sidewalks and roads. One of these ionic compounds is better, mole for mole, at inhibiting ice formation. Which is that likely to be? Why?
What is the osmolarity of each aqueous solution?
1. 0.500 M NH₂CONH₂
2. 0.500 M NaBr
3. 0.500 M Ca(NO₃)₂
What is the osmolarity of each aqueous solution?
1. 0.150 M KCl
2. 0.450 M (CH₃)₂CHOH
3. 0.500 M Ca₃(PO₄)₂

11. A 1.0 M solution of an unknown soluble salt has an osmolarity of 3.0 osmol. What can you conclude about the salt?

12. A 1.5 M NaCl solution and a 0.75 M Al(NO₃)₃ solution exist on opposite sides of a semipermeable membrane. Determine the osmolarity of each solution and the direction of solvent flow, if any, across the membrane.

Answers

1. 1.0 M NaCl
2. 1.0 M NaCl
3. 1.0 M (NH₄)₃PO₄

1.0 M KBr
0.75 M Ca(OH)₂
0.10 M Cu(NO₃)₂

1.0 M NaCl
1.0 M NaCl
1.0 M (NH₄)₃PO₄

1.0 M KBr
0.75 M Ca(OH)₂
0.10 M Cu(NO₃)₂

100.5°C
102.3°C
101°C

-1.9°C
-8.6°C
-3.8°C

7. NaCl lowers the freezing point of water, so it needs to be colder for the water to freeze.

8. CaCl2 splits up into 3 ions while NaCl splits up into 2 ions only. CaCl2 will be more effective.

0.500 osmol
1.000 osmol
1.500 osmol

10.

0.300 osmol
0.450 osmol
2.50 osmol

11. It must separate into three ions when it dissolves.

12. Both NaCl and Al(NO₃)₃have 3.0 osmol. There will be no net difference in the solvent flow.

11.4: Dilutions and Concentrations

What is the difference between dilution and concentration?
What quantity remains constant when you dilute a solution?
A 1.88 M solution of NaCl has an initial volume of 34.5 mL. What is the final concentration of the solution if it is diluted to 134 mL?
A 0.664 M solution of NaCl has an initial volume of 2.55 L. What is the final concentration of the solution if it is diluted to 3.88 L?
If 1.00 mL of a 2.25 M H₂SO₄ solution needs to be diluted to 1.00 M, what will be its final volume?
If 12.00 L of a 6.00 M HNO₃ solution needs to be diluted to 0.750 M, what will be its final volume?
If 665 mL of a 0.875 M KBr solution are boiled gently to concentrate the solute to 1.45 M, what will be its final volume?
If 1.00 L of an LiOH solution is boiled down to 164 mL and its initial concentration is 0.00555 M, what is its final concentration?
How much water must be added to 75.0 mL of 0.332 M FeCl₃(aq) to reduce its concentration to 0.250 M?

How much water must be added to 1.55 L of 1.65 M Sc(NO₃)₃(aq) to reduce its concentration to 1.00 M?

Answers

Dilution is a decrease in a solution’s concentration, whereas concentration is an increase in a solution’s concentration.
0.484 M
2.25 mL
401 mL
24.6 mL

11.5: Concentrations as Conversion Factors

Using concentration as a conversion factor, how many moles of solute are in 3.44 L of 0.753 M CaCl₂?
Using concentration as a conversion factor, how many moles of solute are in 844 mL of 2.09 M MgSO₄?
Using concentration as a conversion factor, how many liters are needed to provide 0.822 mol of NaBr from a 0.665 M solution?
Using concentration as a conversion factor, how many liters are needed to provide 2.500 mol of (NH₂)₂CO from a 1.087 M solution?
What is the mass of solute in 24.5 mL of 0.755 M CoCl₂?
What is the mass of solute in 3.81 L of 0.0232 M Zn(NO₃)₂?
What volume of solution is needed to provide 9.04 g of NiF₂ from a 0.332 M solution?
What volume of solution is needed to provide 0.229 g of CH₂O from a 0.00560 M solution?
What volume of 3.44 M HCl will react with 5.33 mol of CaCO₃? 2HCl + CaCO₃ → CaCl₂ + H₂O + CO₂
What volume of 0.779 M NaCl will react with 40.8 mol of Pb(NO₃)₂? Pb(NO₃)₂ + 2NaCl → PbCl₂ + 2NaNO₃
What volume of 0.905 M H₂SO₄ will react with 26.7 mL of 0.554 M NaOH? H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O
What volume of 1.000 M Na₂CO₃ will react with 342 mL of 0.733 M H₃PO₄? 3Na₂CO₃ + 2H₃PO₄ → 2Na₃PO₄ + 3H₂O + 3CO₂
It takes 23.77 mL of 0.1505 M HCl to titrate with 15.00 mL of Ca(OH)₂. What is the concentration of Ca(OH)₂? You will need to write the balanced chemical equation first.
It takes 97.62 mL of 0.0546 M NaOH to titrate a 25.00 mL sample of H₂SO₄. What is the concentration of H₂SO₄? You will need to write the balanced chemical equation first.
It takes 4.667 mL of 0.0997 M HNO₃ to dissolve some solid Cu. What mass of Cu can be dissolved? Cu + 4HNO₃(aq) → Cu(NO₃)₂(aq) + 2NO₂ + 2H₂O
It takes 49.08 mL of 0.877 M NH₃ to dissolve some solid AgCl. What mass of AgCl can be dissolved? AgCl(s) + 4NH₃(aq) → Ag(NH₃)₄Cl(aq)
What mass of 3.00% H₂O₂ is needed to produce 66.3 g of O₂(g)? 2H₂O₂(aq) → 2H₂O(ℓ) + O₂(g)

A 0.75% solution of Na₂CO₃ is used to precipitate Ca²⁺ ions from solution. What mass of solution is needed to precipitate 40.7 L of solution with a concentration of 0.0225 M Ca²⁺(aq)?

Na₂CO₃(aq) + Ca²⁺(aq) → CaCO₃(s) + 2Na⁺(aq)

Answers

2.59 mol
1.24 L
2.40 g
0.282 L
3.10 L
8.17 mL
0.1192 M
7.39 mg
4.70 kg

11.6: Colligative Properties of Solutions

What are the three colligative properties that involve phase changes?
Which colligative property does not involve a phase change? Give an example of its importance.
If 45.0 g of C₆H₆ and 60.0 g of C₆H₅CH₃ are mixed together, what is the mole fraction of each component?
If 125 g of N₂ are mixed with 175 g of O₂, what is the mole fraction of each component?
If 36.5 g of NaCl are mixed with 63.5 g of H₂O, what is the mole fraction of each component?
An alloy of stainless steel is prepared from 75.4 g of Fe, 12.6 g of Cr, and 10.8 g of C. What is the mole fraction of each component?
A solution is made by mixing 12.0 g of C₁₀H₈ in 45.0 g of C₆H₆. If the vapor pressure of pure C₆H₆ is 76.5 torr at a particular temperature, what is the vapor pressure of the solution at the same temperature?
A solution is made by mixing 43.9 g of C₆H₁₂C₆ in 100.0 g of H₂O. If the vapor pressure of pure water is 26.5 torr at a particular temperature, what is the vapor pressure of the solution at the same temperature?
At 300°C, the vapor pressure of Hg is 32.97 torr. If 0.775 g of Au were dissolved into 3.77 g of Hg, what would be the vapor pressure of the solution?
At 300°C, the vapor pressure of Hg is 32.97 torr. What mass of Au would have to be dissolved in 5.00 g of Hg to lower its vapor pressure to 25.00 torr?
If 25.0 g of C₆H₁₂O₆ are dissolved in 100.0 g of H₂O, what is the boiling point of this solution?
If 123 g of C₁₀H₁₆O are dissolved in 355 g of C₆H₆, what is the boiling point of this solution?
If 1 mol of solid CBr₄ is mixed with 2 mol of CCl₄, what is the boiling point of this solution?
A solution of C₂H₂O₄ in CH₃COOH has a boiling point of 123.40°C. What is the molality of the solution?
If 123 g of C₁₀H₁₆O are dissolved in 355 g of C₆H₆, what is the freezing point of this solution?
If 25.0 g of C₆H₁₂O₆ are dissolved in 100.0 g of H₂O, what is the freezing point of this solution?
C₈H₁₇OH is a nonvolatile solid that dissolves in C₆H₁₂. If 7.22 g of C₈H₁₇OH is dissolved in 45.3 g of C₆H₁₂, what is the freezing point of this solution?
A solution of C₂H₂O₄ in CH₃COOH has a freezing point of 10.00°C. What is the molality of the solution?
If 25.0 g of C₆H₁₂O₆ are dissolved in H₂O to make 0.100 L of solution, what is the osmotic pressure of this solution at 25°C?
If 2.33 g of C₂₇H₄₆O are dissolved in liquid CS₂ to make 50.00 mL of solution, what is the osmotic pressure of this solution at 298 K?
At 298 K, what concentration of solution is needed to have an osmotic pressure of 1.00 atm?

The osmotic pressure of blood is about 7.65 atm at 37°C. What is the approximate concentration of dissolved solutes in blood? (There are many different solutes in blood, so the answer is indeed an approximation.)

Answers

boiling point elevation, freezing point depression, vapor pressure depression
mole fraction C₆H₆: 0.469; mole fraction C₆H₅CH₃: 0.531
mole fraction NaCl: 0.157; mole fraction H₂O: 0.843
65.8 torr
27.26 torr
100.71°C
92.9°C
−5.65°C
−18.3°C
33.9 atm
0.0409 M

Additional Exercises

One brand of ethyl alcohol (Everclear) is 95% ethyl alcohol, with the remaining 5% being water. What is the solvent and what is the solute of this solution?
Give an example of each type of solution from your own experience.
1. A solution composed of a gas solute in a liquid solvent.
2. A solution composed of a solid solute in a liquid solvent.
3. A solution composed of a liquid solute in a liquid solvent.
4. A solution composed of a solid solute in a solid solvent. (Hint: usually such solutions are made as liquids and then solidified.)
Differentiate between the terms saturated and concentrated.
Differentiate between the terms unsaturated and dilute.
What mass of FeCl₂ is present in 445 mL of 0.0812 M FeCl₂ solution?
What mass of SO₂ is present in 26.8 L of 1.22 M SO₂ solution?
What volume of 0.225 M Ca(OH)₂ solution is needed to deliver 100.0 g of Ca(OH)₂?
What volume of 12.0 M HCl solution is needed to obtain exactly 1.000 kg of HCl?
The World Health Organization recommends that the maximum fluoride ion concentration in drinking water is 1.0 ppm. Assuming water has the maximum concentration, if an average person drinks 1,920 mL of water per day, how many milligrams of fluoride ion are being ingested?
For sanitary reasons, water in pools should be chlorinated to a maximum level of 3.0 ppm. In a typical 5,000 gal pool that contains 21,200 kg of water, what mass of chlorine must be added to obtain this concentration?
Given its notoriety, you might think that uranium is very rare, but it is present at about 2–4 ppm of the earth's crust, which is more abundant than silver or mercury. If the earth's crust is estimated to have a mass of 8.50 × 10²⁰ kg, what range of mass is thought to be uranium in the crust?
Chromium is thought to be an ultratrace element, with about 8.9 ng present in a human body. If the average body mass is 75.0 kg, what is the concentration of chromium in the body in pptr?
What mass of 3.00% H₂O₂ solution is needed to produce 35.7 g of O₂(g) at 295 K at 1.05 atm pressure?
2H₂O₂(aq) → 2H₂O(ℓ) + O₂(g)
What volume of pool water is needed to generate 1.000 L of Cl₂(g) at standard temperature and pressure if the pool contains 4.0 ppm HOCl and the water is slightly acidic? The chemical reaction is as follows:
HOCl(aq) + HCl(aq) → H₂O(ℓ) + Cl₂(g)
Assume the pool water has a density of 1.00 g/mL.
A 0.500 m solution of MgCl₂ has a freezing point of −2.60°C. What is the true van 't Hoff factor of this ionic compound? Why is it less than the ideal value?
The osmotic pressure of a 0.050 M LiCl solution at 25.0°C is 2.26 atm. What is the true van 't Hoff factor of this ionic compound? Why is it less than the ideal value?
Order these solutions in order of increasing boiling point, assuming an ideal van 't Hoff factor for each: 0.10 m C₆H₁₂O₆, 0.06 m NaCl, 0.4 m Au(NO₃)₃, and 0.4 m Al₂(SO₄)₃.
Order these solutions in order of decreasing osmotic pressure, assuming an ideal van 't Hoff factor: 0.1 M HCl, 0.1 M CaCl₂, 0.05 M MgBr₂, and 0.07 M Ga(C₂H₃O₂)₃

Answers

solvent: ethyl alcohol; solute: water
Saturated means all the possible solute that can dissolve is dissolved, whereas concentrated implies that a lot of solute is dissolved.
4.58 g
6.00 L
1.92 mg
1.7 × 10¹⁵ to 3.4 × 10¹⁵ kg
2,530 g
2.80; it is less than 3 because not all ions behave as independent particles.
0.10 m C₆H₁₂O₆ < 0.06 m NaCl < 0.4 m Au(NO₃)₃ < 0.4 m Al₂(SO₄)₃