1. Solution--a homogeneous mixture of two or more substances
Solute----the component in a solution which exists in the smaller quantity
Solvent--the component in a solution which exists in the greater quantity
Solubility--the maximum amount of a solute which can dissolve in a given amount of solvent at a given temperature
Immiscible-- describes two or more liquids that will not mix together to form a single homogeneous substance
Miscible-- describes two or more liquids that can be mixed together
Miscibility-- the tendency or capacity of two or more liquids to form a homogeneous solution, that is, to dissolve in each other
Saturated-- a chemical solution that is saturated has as much of a solid substance as possible mixed in it as part of the liquid
Unsaturated—a solvent is unsaturated with a solute if it can dissolve more of the solute
2. Ionization is a reaction which involves the breaking up of a neutral molecule into ions. However, dissociation is a reaction involving separating previously-existing ions in an ionic acid.
3. a) A solution needs moving charged particles to conduct electricity. In the solution the charge is carried by ions moving through the solution. For a solution to conduct, it requires moving ions.
b) All metals (all phase)
Acid or base (liquid/aqueous/molten)
Ionic compound (molten/ aqueous)
Organic acids (aqueous only)
4. a) ionic solid---a solid whose crystal structure is made up of ions
Example: NaCl - sodium chloride & LiBr - lithium bromide
Molecular solid---a solid whose crystal structure is made of neutral molecules
Example: sugar & solid carbon dioxide
b) Ionic solids conduct electricity in solutions because ionic solids can result moving ions in the solutions. However, when we put molecular solids in solutions, there are no ions.
5. a) metal: i) , ii)
acid: vii) ,xiii) , xiv)
base: xii),
organic acid: xiii) , xiv)
Ionic compound: x), xi),
alcohol: vii)
others: iii), v), iv), vi), ix), xv)

b) i), ii), vii) ix) x). xi). xiv)
6. London force and dipole-dipole force.
7. London forces are weak attractive forces which arise as a result of temporary dipolar attractions between neighboring atoms. London forces are always present, even in species which have covalent or ionic bonding.
Dipole-dipole force is a bonding force which exists as a result of an electrostatic attraction between molecules having permanent dipoles. Dipole-dipole force exists between polar molecules.
8. Dipole is a partial charge separation existing when one end of a molecule (or bond) has a slight excess of positive charge and the other end of the molecule has a slight excess of negative charge.
Example:
9. HCl & CH3Cl
10. O, N, F
11. BeF2, CH4, CH3CH2COCH2CH3
12. BeF2, CH4, CH3CH2COCH2CH3
13. HF
14. Polar solvents have dipoles which attract other dipoles, so polar solutes are attracted by polar solvents. Those attractions are due to electrostatic force. That’s why polar solutes tend to dissolve in the polar solvents and form homogeneous mixture.
15. Non-polar species do not possess positive and negative ends, so there is no attraction to polar or ionic species as a result of attractions between ions. Non-polar solvents are only attracted to solute particles by London force which is caused by electrostatic force.

17.
18.
19.
16.
(There is no No.20)
21. for Kw

23.
22.
24. a) False
b) False
c) False
d) True
25. d, b, f, g, a, c, e

26.