Chemistry Grade 11: Aqueous Solutions & Elements

Study Notes

Course: Seniors 26, Grade 11
Learning Objective (LO.1): Aqueous Solutions
Session: 1
Preparation: Solve test banks, complete assignments, study diligently, print and highlight handouts, add notes, and attend sessions.

Data: The table organizes elements based on atomic number, electron configuration, and properties.
Data: Standard atomic weight (or most stable mass number) noted for each element.
Data: First ionization energy in kJ/mol.
Data: Oxidation states (most common highlighted).
Information: Radioactive elements have masses in parentheses.
Classification: Alkali metals, alkaline earth metals, transition metals, lanthanides, actinides, nonmetals, reactive nonmetals, noble gases, metalloids, unknown properties, and post-transition metals.

Topic: Purification of Water Supply
Topic: Processes for converting seawater to potable water
Essential Question: How can pure, drinkable water be obtained?
Concepts:
- Solutions and aqueous solutions
- Solubilities of salts (temperature impact)
- Solubility curves
- ppm
- Molarity
- Molality
- Normality
- Mole fraction
- Mass percentage
- TDS
- Strength
- Titers
- DO
- Percentage of ions needed by the human body daily
Methods of Purification:
- Resins (including ion exchange)
- EDTA
- Electrodialysis
- Simple distillation
- Filtration
- Adsorption
- Sedimentation/alum
- Biological treatment
- Oxygenation
- Osmosis and reverse osmosis
- Dissolved oxygen
- Quantitative analysis
- Qualitative analysis

Q1: If a 1 M solution is reduced to half its volume, the concentration doubles.
Q2: Heating a 1 M solution (without evaporation) does not change the concentration.
Q3: Heating a 1 M solution until 2/3 evaporates increases the concentration to 3/2 M.
Q4: Cooling a 1 M solution until 1/3 freezes increases the concentration to 3/2 M.
Q5: Doubling the volume of a 1 M solution halves the concentration.
Concentration Factors Affected by Temperature: Molarity
Solution of 0.5 Moles of NaCl in 1 Liter: Semimolar solution
To Half the Molarity of a Solution: Double the volume of the solution.
Molarity of 600 g H2O: 55.5 M

Different methods to express concentration: Molarity, Molality, Mass%, Volume %, Strength, Titre, Normality, Mole fraction, ppm.
Problem 1 (Practice): Final concentration after dilution of car battery acid.
Problem 2 (Practice): Volume of sodium hydroxide solution required.
Problem 3 (Practice): Amount concentration of ethanoic acid (acetic acid).
Problem 4 (Practice): Amount concentration of iron(III) nitrate stock solution.
Problem 5 (Dilution): Procedure for preparing a 0.4 M solution from 1 M CuSO4, with calculation of water that needed to be added.
Problem 6 (Dilution): Final concentration of nitric acid solution after dilution.
Practice 2 (Preparation of Solution): Procedures for preparing 1M Sodium hydroxide and 0.1M KMnO4
Conceptual Problems (Q1-Q5): Understanding how solution volume affect concentration, effect of temperature. Molarity calculation from volumes and moles.
Solutions With Same Molarity: Calculating mass required for different solutions to have the same colligative molarity.

Total Ion Concentration: Arranging solutions in order of increasing total ion concentration.
Electrolytes : Classify and calculate concentration when adding electrolytes that produce same different ions
Different Solutes Added and Volumes: Calculating moles of solid CaCl2 needed to adjust concentration in a solution.