1. colligative property - a property of a solution that depends on the concentration of the solute particles; boiling point elevation, freezing point depression, and vapor pressure lowering are colligative properties.
2. colloidal dispersion - a heterogeneous system which is dispersed as particles in another substance
3. dynamic equilibrium - an equilibrium in which processes occur continuously, with no net change. when 2 or more process occur at the same rate so that no net change occurs.
4. electrolyte - a compound that conducts an electric current in aqueous solution or the molten state; all ionic compounds are electrolytes, but most covalent compounds are not
5. heterogeneous mixture -a mixture that is not uniform in composition; its components are readily distinguished
6. homogeneous mixture - a mixture that is completely uniform in composition; its components are not distinguishable
7. molar - containing one mole per liter
8. molarity -(M) the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1L of solution
9. moles - (mol) the amount of a substance that contains 6.02x10^23 representative particles of that substance; a gram formula mass of any substance
10. percent solution (w/w) - (mass of solute)/(weight of solution) x 100
11. percent solution (w/v) - ( mass of solute)/(volume of solution) x 100
12. percent solution (v/v) - (volume of solute)/(volume of solution) x 100
13. polyunsaturated - molecule having long carbon chains with many double bonds unsaturated by hydrogen atom
14. saturated solution - a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature sand pressure; in a saturated solution, the dissolved and undisclosed solute are in dynamic equilibrium
15. solubility - the amount of a substance that dissolves in a given quantity of solvent at specified conditions of temperature and pressure to produce a saturated solution
16. solute - dissolved particles in a solution
17. solution - a homogeneous mixture
18. solvent - the dissolving medium in a solution
19. supersaturated solution - a solution that contains more solute than it can theoretically hold at given temperature
20. suspension - a mixture from which some of the particles settle out slowly upon standing
21. unsaturated solution - a solution that contains less solute that a saturated solution at a given temperature and pressure
Acid & Bases
1. acid - a compound containing hydrogen that ionizes to yield hydrogen ions (H + ) in water
2. acidic - the hydrogen-ion concentration is greater than the hydroxide-ion concentration
3. alkaline - basic solution / group 2A of periodic table
4. amphoteric - a substance that can act both as an acid and a base (ex. water)
5. Arrhenius acid - dissolves in water, tends to increase amount of H+
6. Arrhenius base - dissolves in water, tends to increase the amount of OH-
7. base - a compound that ionizes to yield hydroxide ions (OH- ) in water
8. basic - the hydroxide - ion concentration is greater than the hydrogen - ion concentration
9. Bronsted-Lowry acid - species that donate proton (H+)
10. Bronsted-Lowry base - species that accept a proton (H+)
11. buffer -a solution in which he pH remains relatively constant when small amount of acid or base are added; it consists a solution of a week acid(base) and the salt of a weak acid (base)
12. conjugated acid - the particle formed when a base gains a hydrogen ion (ex. NH+4 is conjugated acid of base NH3.
13. conjugated acid-base pair - two substances that are related by the loss or gain of a single hydrogen ion. (ex. NH3 and the NH+4 are a conjugated acid-base pair.
14. conjugate base - the particle that remains when a acid has donated a hydrogen ion; (ex OH- is the conjugate base of the acid water)
15. diprotic acid -any acid that contains two ionizable protons (hydrogen ions); (ex. sulfuric acid (H2SO4) is a diprotic acid. )
16. electron pair acceptor - an acid to Lewis Concept
17. electron pair donor - a base to Lewis Concept
18. hydrogen ion acceptor -a base, according to the Bronsted-Lowery theory
19. hydrogen ion donor - an acid, according to the Bronsted-Lowery theory
20. hydronium ion -(H3O+) the positive ion formed when a water molecule gains a hydrogen ion; all hydrogen ions in aqueous solution are present as hydronium ions.
21. hydroxide ion - (OH-) the negative ion formed when a water molecule loses a hydrogen ion
22. indicator - a substance that shows the presence or concentration of a specific material or chemical
23. ionize - produce or become ions
24. Lewis acid - any substance that can accept a pair of electrons to form a covalent bond
25. Lewis base - any substances that can donate a pair of electrons to form a covalent bond
26. litmus - acid - base indicator
27. monoprotic acid - any acid that contains one ionizable proton (hydrogen ion)(ex. nitric acid(HNO3) is a monoprotic acid)
28. neutral - not acid or alkaline
29. neutralization - made something neither acid nor alkaline
30. pH - a number sued to denote the hydrogen-ion concentration, or acidity, of a solution; it is the negative logarithm of the hydrogen ion concentration of a solution
31. pOH -mearuses the basicity of a solution. it is the negative log of the concentration of the hydroxide ions.
32. phenolphthalein - C20H20O4 , a acid-base indicator, in making dyes
33. property -trait or attribute, characteristic quality
34. strong acid - an acid that is completely (or almost completely) ionized in aqueous solution
35. strong base - a base that completely dissociates into metal ions and hydroxide ions in aqueous solution
36. titration - a method of reacting a solution of unknown concentration (acid) with one known concentration (base), usually to determine the concentration of the unknown solution(acid)
37. triprotic acid -any acid that contains three ionizable protons (hydrogen ions)(ex. phosphoric acid (H3PO4) is a triprotic acid)
38. verify - check wheatear something is true, prove something
39. weak acid- a acid that is only slightly ionized in aqueous solution
40. weak base - a base that does not dissociate completely in aqueous solution
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