Chapter 9

Question 1

complex coordination ion

Answer 1

molecule with cation bonded to at least on electron pair donor

Question 2

coordinate covalent

Answer 2

electron pair donor (lewis base) and acceptor (acid) form stable lewis acid- base adducts

forms complex ions

Question 3

percent composition by mass

Answer 3

mass of solute/ mass of solution x100%

Question 4

mole fraction equation

Answer 4

Xa= moles A / total moles

Question 5

molarity

Answer 5

moles of solute/ liters solution

Question 6

molality

Answer 6

moles solute/ kg solvent

Question 7

normality

Answer 7

equiv. of interest/ liter

Question 8

dilution

Answer 8

MiVi= MfVf

molarity and volume

Question 9

solubility product constant

Answer 9

Ksp= [An+]^m [Bm-]^n

AT SATURATION

when AmBn -> mAn+ + nBM-

no pure solids or liquids

Question 10

ion product

Answer 10

shows if at saturation when compared to ksp

IP= [An+]^m [Bm-]^n

Question 11

comparing Ip and Ksp

Answer 11

Ip< Ksp= unsaturated, solute will continue to disolve

Ip> Ksp= supersaturated, precipitation will occur

Question 12

common ion effect

Answer 12

reduce solubility of a compound when constitute ion is in solution

Question 13

colligative properties

Answer 13

depends on concentration of dissolved particles

VP depression, BP elevation, FP depression and osmotic pressure

Question 14

Raoults Law

Answer 14

accounts for VP depression caused by solutes in solution

as concentration increases, VP decreases- because solution blocks evap

Question 15

Raoults Law equation

Answer 15

Pa= Xa Pa0

p= pressure of solvent and solute

Pa0= pure vapor pressure of solvent

Question 16

BP elevation equation

Answer 16

Delta Tb= iKbm

i= Hoff

m= molality

Question 17

Fp depression

Answer 17

delta tF= iKfm

Question 18

osmotic pressure

Answer 18

= iMRT

M= molarity