Chapter 9 - Solutions

Question 1

What molar solubility is makes solutes soluble?

Answer 1

Above 0.1M in solution

Question 2

Seven solubility rules

Answer 2

1. All salts containing NH4+ and alkali metal (group 1) cations
2. All salts with NO3- and acetate anions are water soluble
3. Halides (Cl-, Br-, I-) excluding fluorides are soluble exceptions when formed with Ag, Pb and Hg
4. all salts of SO4- are soluble, **except Ca, Sr, Ba, Pb
5. All metal oxides INSOLUBLE , **except when formed w alkali metals, NH4+, CaO, SrO, BaO
6. All OH are insoluble
   * *except if formed with alkali metals, NH4, Ca, Sr, Ba
7. Alll carbonates (CO3), PO4, S2- , SO3, are INSOLUBLE, except when w alkali metals and NH4

Question 3

Are salts of group 1 metals and nitrate salts soluble or insoluble?

Answer 3

SOLUBLE!!!!

Question 4

Percent composition by mass

Answer 4

(Mass solute/mass solution) x 100%

Question 5

Mole fraction

Answer 5

Xa = moles of a / total moles

Question 6

Molality

Answer 6

m = moles of solute / kg of solvent

Question 7

Normality

Answer 7

(N) equivalents of interest PER LITER OF SOLUTION

Question 8

What is the first step for any mcat solution equilibrium or solution stoich question ?

Answer 8

write the BALANCED EQUATION!!

Question 9

What is the solubility product constant

Answer 9

Ksp = [A^n+]^m[B^m

Question 10

What is the ion product?

Answer 10

Essentially the same as Ksp (same equation) but rather than using the concentrations at eq you use the current concentrations

Question 11

What if IP > Ksp?

Answer 11

Supersaturated…precipitation will occur

Question 12

IP < Ksp

Answer 12

Solute will continue to dissolve

Question 13

IP = Ksp

Answer 13

Solution is at equilibrium

Question 14

Molar solubility

Answer 14

Molarilty of a solution at equilibrium

**ksp doesn’t change!! (Only temp can change it)

Question 15

COMMON ION EFFECT

Answer 15

Molar solubility is reduced