1. Aqueous Solutions & Reactions
CONCENTRATION
Aqueous Solutions & Reactions
Dr. Ron Rusay

2. Solutions http://chemconnections.org/crystals/
Homogeneous solutions are comprised of solute(s), the substance(s) dissolved, [The lesser amount of the component(s) in the mixture], and
solvent, the substance present in the largest amount.
Solutions with less solute dissolved than is physically possible are referred to as “unsaturated”. Those with a maximum amount of solute are “saturated”.
Occasionally there are extraordinary solutions that are “supersaturated” with more solute than normal.

3. Concentration and Temperature
Relative Solution
Concentrations:
Saturated
Unsaturated
Supersaturated

4. DHMO, dihydromonoxide: “The Universal” Solvent
The oil (nonpolar) and water (polar) mixture don’t mix and are immiscible. If liquids form a homogeneous mixture, they are miscible.
Generally, likes dissolve likes, i.e. polar-polar and nonpolar-nonpolar. Polar and nonpolar do not mix , eg. oil and water

5. Aqueous Reactions & Solutions
Many reactions are done in a homogeneous liquid or gas phase which generally improves reaction rates.
The prime medium for many inorganic reactions is water which serves as a solvent (the substance present in the larger amount), but does not react itself.
The substance(s) dissolved in the solvent is (are) the solute(s). Together they comprise a solution. The reactants would be the solutes.
Reaction solutions typically have less solute dissolved than is possible and are “unsaturated”.

6. Salt dissolving in a glass of water

7. Refer to the simulation for the following 6 questions
Aqueous Solutions
Questions
Refer to the simulation for the following 6 questions

8. Which action(s) will increase the concentration of the solution?
Add more Co(NO3)2
Evaporate water
Drain solution
(1) only
(1) and (2)
(2) and (3)
(1) and (3)
(1), (2), and (3)
Sim directions: Show students the various features available in the simulation -- use both faucets, add more solid from the salt shaker, evaporate some of the solution – initially without the concentration probe in solution. Comment on changes in solution colour, then use the concentration probe to show how concentration increases or decreases in response to these actions. Use Drink Mix for initial demonstrations as it gives students a real-world connection that they often find more intuitive for building an understanding of terms like dilute and concentrated, and for understanding what impacts concentration. Use sim observations to construct a definition of concentration before asking the following concept questions.
Correct answer: B
Representative results from pre-general chemistry: 85% correct (remaining students evenly distributed among other answers)
Follow-up discussion: Use the simulation to demonstrate each of the options given, and discuss as a class.
Note that setting up a specific starting solution is easiest if you create a slightly more concentrated solution and then dilute with water as needed (water faucets have higher precision control), and then drain any excess solution away.

9. Which action(s) will change the
Molarity (M) = Moles solute / Liter solution
Which action(s) will change the
number of moles of solute in the container?
Add water
Evaporate water
Drain solution
(1) only
(2) only
(3) only
(1) and (2)
(2) and (3)
Goal: Extend students observations of concentration (from the simulation) to the relationship between moles and concentration.
Correct answer: C
Representative results from pre-general chemistry: 62% correct (21% selected D)
Follow-up discussion: Summarize the observations, and ask the class the effect of each these actions on concentration, in parallel.

10. Molarity (M) = Moles solute / Liter solution
What will happen to the concentration and the number of moles when water is added?
Concentration Number of moles
Increase Decrease
Increase Increase
No change No change
Decrease Decrease
Decrease No change
Correct answer: E
Representative results from pre-general chemistry: 86-89% correct (remaining students evenly distributed between other answers)

11. How many moles of solute are in the beaker?
Molarity (M) = Moles solute / Liter solution
How many moles of solute are in the beaker?
Goal: Have students begin to think about concentration quantitatively
Correct answer: C
Representative results from pre-general chemistry: 63% correct (B and C are popular alternate answers)
Follow-up discussion: Ask students how many moles are in the beaker, and how they figured that out. Ask students to discuss with their peers, and offer the suggestion of thinking about how many moles would be in 1L of this same solution.
a moles b moles c moles
d moles e. None of these

12. Molarity (M1) x Volume (V1) = Molarity (M2) x Volume (V2)
You are given 200 mL of a M solution of KMnO4.
If you add water until total volume is 800 mL, what will be the final concentration of the solution?
a M
b M
c M
d M
e M
Goal: Introduce dilution (in this case of stock solutions) with simple numbers to promote proportional reasoning prior to calculation.
Correct answer: B
Follow-up discussion: Discuss whether a calculator is needed to solve this problem, and how students approached the question.

13. You start with 0.1 L of a 5.00 M solution of NiCl2, and you plan to dilute it (by adding water) to make a solution with a concentration of M. How far should you fill the beaker?
a mL
b mL
c mL
d mL
e. 1 L
A computation-based dilution problem
Correct answer: D
Representative results from pre-general chemistry: 81% correct (C is the next most popular answer at 10% student responses)

14. Solution Test Apparatus for Electrolytes

15. Conductivity

16. Electrolytes
Aqueous solutions can be categorized into 3 types: non-electrolytes, strong electrolytes or weak electrolytes based on their ability to conduct electricity.
A solution must have ions to conduct.
Pure Water does not conduct.
Aqueous solutions can be tested for conductivity which will determine the degree of ionization of the solutes.
It is possible to have full or partial ionization.

17. Electrolytes
Molarity (M) = Moles solute / Liter solution
Almost all ionic compounds and a few molecular compounds are strong electrolytes.
Several molecular compounds are weak conductors, most are non-conductors.
Conductivity is directly related to the amount of ionization, i.e. ions in solution. Table salt, sodium chloride, is completely ionized:
NaCl(s) + H2O(l) NaCl(aq) M Na +(aq) + Cl -(aq) 0.00M M M

18. You have prepared a 1.0 M solution of NaCl in the laboratory.
What is the concentration of chloride ions in the solution?
a M
b M
c M
d M
Multi-sim question: Sugar and salt solutions + Concentration
Goal: The following four questions extend students’ conception of concentration to ion concentrations.
Correct answer: B
Representative results from pre-general chemistry: 55% A and 37% B
Follow-up discussion: Review the nature of ionic compounds using the Sugar and Salt Solutions simulation (Micro tab) to demonstrate the ratio of sodium to chloride ions. Use the pause/play feature to count ions in the solid, and count the ions in solution, to show that the total number of ions is the same. Highlight the ion concentration shown on the graph. Ask students to discuss how many moles of sodium ions are in one mole of NaCl, and then relate this to concentration.

19. Electrolytes Concentrations:
Molarity (M) = Moles solute / Liter solution
Concentrations:
CaCl2 (s) + H2O(l) CaCl2(aq) M Ca 2+(aq) + 2 Cl -(aq) 0.00M M M

20. You have prepared a 1.0 M solution of CaCl2 in the laboratory.
What is the concentration of chloride ions in the solution?
a M
b M
c M
d M
Multi-sim question: Sugar and salt solutions + Concentration
Correct answer: D
Representative results from pre-general chemistry (on first poll): Votes roughly even split between A, B, and D
Follow-up discussion: Ask students what the component ions are in CaCl2, confirming that the anion is chloride, not Cl2. Use the Sugar and Salt Solutions simulation (Micro tab) to demonstrate the ratio of calcium to chloride ions. Use the pause/play feature to count ions in the solid, and count the ions in solution, to show that the total number of ions is the same. Highlight the ion concentrations shown on the graph, where chloride is roughly double that of calcium.
Representative results from pre-general chemistry (on second poll, following peer discussion): 83% correct

21. Electrolytes C12H22O11 (S) + H2O(l) C12H22O11 (aq)
Molarity (M) = Moles solute / Liter solution
Sugars like sucrose are non-ionic, molecular compounds that dissolve but produce no ions.
C12H22O11 (S) + H2O(l) C12H22O11 (aq)
Some molecular compounds like acetic acid ionize partially (dissociate) in water
HC2H3O2 (l) + H2O(l) H3O+(aq) M C2H3O2 -(aq)
M M

22. Aqueous Acids
Any compound that provides a proton can be considered an acid. Strong acids are sulfuric acid, nitric acid, perchloric acid, HI, HBr and HCl.

23. Electrolytes
How would the conductivity of acetic acid compare to hydrochloric acid?

24. Conductivity
Which of these solutions will have highest conductivity? A B C
0.1 M KCl(aq)
0.2 M HCl(aq)
0.3 M HC2H3O2(aq)
Multi-sim question: Sugar and salt solutions + Concentration
Correct answer: B
Representative results from pre-general chemistry: 91% correct
Follow-up discussion: Ask students about the concentration of each ion and discuss how conductivity is impacted by ion concentration

25. HCl Completely Ionized
Acetic Acid (HC2H3O2)
HCl Completely Ionized

26. Conductivity
Which of these solutions will have highest conductivity? A B C
0.1 M HCl(aq)
0.1 M CaCl2 (aq)
0.2 M HC2H3O2(aq)
Multi-sim question: Sugar and salt solutions + Concentration
Correct answer: B
Representative results from pre-general chemistry: 66% correct (with a roughly even split between the other two options)
Follow-up discussion: Ask students how they determined the higher conductivity solution – students have previously asked why this dissociates into 2 Cl- instead of 1 Cl22- since chlorine occurs naturally as Cl2. Other students responded to this query with ideas about ion charges and the absence of charge on molecular Cl2 gas.

27. Aqueous Bases NH3 (g) + H2O(l) NH3 (aq) NH4+(aq)+ OH-(aq)
Any compound that accepts a proton is a base.
The common bases are group IA & IIA metal hydroxide compounds. They are strong bases, dissociating completely in water.
An example of a weak base is ammonia.
NH3 (g) + H2O(l) NH3 (aq) NH4+(aq)+ OH-(aq)
Consider that aqueous ammonia is in equilibrium with ammonium hydroxide. The names have often been used interchangeably.

28. An Aqueous Solution of Sodium Hydroxide
NH3 in Water

30. QUESTION

31. ANSWER

32. Aqueous Reactions
There are several general types, but we will focus on two:
1) Acid-Base Reactions (Neutralization) generally produces a salt plus water
2) Oxidation-Reduction (Redox) there is a change in oxidation numbers between reactants and products
Precipitation: An insoluble salt forms from the addition of solutions.

33. Aqueous Reactions: Neutralization

34. QUESTION
An aqueous solution of H2SO4 is added to aqueous Ba(OH)2. A white cloudiness is observed and the reaction is monitored using a light conductivity tester. The reactants both produced strong light, which dimmed as they were added together and the reaction proceeded
Predict the correct statement(s).
I) Both H2SO4 and Ba(OH)2 are strong electrolytes.
II) This is a neutralization reaction.
III) This is a precipitation reaction.
IV) The light bulb will glow at the neutralization point.
A) II B) I and II
C) I, II and III D) I, II, III and IV

35. ANSWER
An aqueous solution of H2SO4 is added to aqueous Ba(OH)2. A white cloudiness is observed and the reaction is monitored using a light conductivity tester. The reactants both produced strong light, which dimmed as they were added together and the reaction proceeded
Predict the correct statement(s).
I) Both H2SO4 and Ba(OH)2 are strong electrolytes.
II) This is a neutralization reaction.
III) This is a precipitation reaction.
IV) The light bulb will glow at the neutralization point.
A) II B) I and II
C) I, II and III D) I, II, III and IV
Correct Answer: C
Question Number: 6

36. Aqueous Reactions: Acid-Base

37. QUESTION
If an antacid contains Al(OH)3 it will form AlCl3 upon neutralization of stomach acid. How many moles of Cl– ions are in mL of M AlCl3? M
0.010 M M
0.030 M
Molarity (M) = Moles solute / Liter solution

38. ANSWER
If an antacid contains Al(OH)3 it will form AlCl3 upon neutralization of stomach acid. How many moles of Cl– ions are in mL of M AlCl3? M
0.010 M M
0.030 M
AlCl3 dissociates into 3 moles of Cl–.
Molarity (M) = Moles solute / Liter solution

39. QUESTION

40. ANSWER

41. Oxidation-Reduction Oxidation is the loss of electrons.
Reduction is the gain of electrons.
The reactions occur together. One does not occur without the other.
The terms are used relative to the change in the oxidation state or oxidation number of the reactant(s).

42. Aqueous Reactions: Oxidation - Reduction
In the following reaction, identify what is being oxidized and what is being reduced?
What gains electrons and what looses?

44. QUESTION
In a redox reaction, oxidation and reduction must both occur. Which statement provides an accurate premise of redox chemistry?
The substance that is oxidized must be the oxidizing agent.
The substance that is oxidized must gain electrons.
The substance that is oxidized must have a higher oxidation number afterwards.
The substance that is oxidized must combine with oxygen.

45. ANSWER
In a redox reaction, oxidation and reduction must both occur. Which statement provides an accurate premise of redox chemistry?
The substance that is oxidized must be the oxidizing agent.
The substance that is oxidized must gain electrons.
The substance that is oxidized must have a higher oxidation number afterwards.
The substance that is oxidized must combine with oxygen.