1. Properties of water Solid phase ______ dense than liquid
High __________ heat
Heat retention
High latent heat of _______________
Evaporative cooling
Sweating
“______________ solvent”
Dissolves most molecules
All result from water’s chemical structure
less
specific
vaporization
Universal

2. Structure of water molecules
Bent
________ molecular shape
Characterized by _____ covalent bonding
Polar molecule: dipole – positive side and negative side
Oxygen = ____________ side
Hydrogen = ______________ side
____________ bonding between molecules
Accounts for many __________ properties
Ice floats due to the difference in ________
polar
negative
positive
Hydrogen
physical
density

6. The dissolving process
Solution - _______________ mixture of ions/molecules from two or more substances
Dissolving - the process of making a _____________
Components of a solution
Solvent - present in __________ amount
Solute - component ___________ in solvent
Aqueous solution - solid, liquid or gas dissolved in _______
homogeneous
solution
largest
dissolved
water

7. Solutions - further details…
Limits of solubility
____________ solutions – no more solute can be dissolved
Insoluble substances, no noticeable dissolving
Simple rule: “Like dissolves _______”
_______ substances dissolve each other
Polar substances can be dissolved by polar solvents
Nonpolar substances are dissolved by __________ solvents.
Fluids: gases and liquids
____________ fluids
Can mix in any proportions w/o separating
Immiscible fluids do not _______
Saturated
like
Similar
nonpolar
Miscible
mix

8. Liquid solvents and solids
“Like dissolves like”
Oil and grease are not __________ in water; but the salt is. Why?
Attraction between the ions of the salt crystal and the polar ends of the water molecules.
soluble

10. Concentration of solutions
Concentration - relative amounts of _________ and ___________
Relative terminology
“_____________” - large amount of solute
“_________” - small amount of solute
More precise to take measurements of concentration
Solute
Solvent
Concentrated
Dilute

11. Concentration Measurements
Concentration ratios
Parts per million (ppm); parts per billion (ppb)
By volume or weight
Percent by volume
Percent by weight
Salinity
Mass of salts dissolved in 1000 g of solution
Molarity (M)
Moles of solute in 1 liter of solution

13. Solubility Saturation Solute dissolving _______ limit
______________ between going in and out of solution
Solubility
____________________ of saturated solution
Depends on __________________
Gases: ____________ with temperature; ___________with pressure
limit
Equilibrium
Concentration
temperature
decreases
increases

15. Solubility Curve
Which salt shows the greatest increase in solubility from 0-60oC? _______
At 50oC, 70 g of KNO3 is dissolved in 100 g of water. Is the solution saturated, unsaturated or supersaturated? ___________________
Which salt is least soluble in water at 60oC? ___________________
Which is the most soluble salt at 20oC? ___________________
What is the solubility of KCl at 80oC? ___________________
What it the temperature at which KNO3 has a solubility of 90g/100g of water? ________________

16. Solubility Curve
Which salt is most soluble in water at 60oC? ___________________
Which salt shows the least increase in solubility from 0-60oC? _______
At 50oC, 40 g of KCl is dissolved in 100 g of water. Is the solution saturated, unsaturated or supersaturated? ___________________
Which is the least soluble salt at 20oC? ___________________
What is the solubility of KCl at 20oC? ___________________
What it the temperature at which KNO3 has a solubility of 20g/100g of water? ________________