unit 10: solutions name: _______________________ solution definitions s olution: a homogeneous mixture -- -- e.g., alloy: a so

Unit 10: Solutions Name: _______________________
Solution Definitions
s olution: a homogeneous mixture
--
-- e.g.,
alloy: a solid solution of metals
-- e.g.,
solvent: the substance that dissolves the solute
soluble: “will dissolve in”
miscible: refers to two liquids that mix evenly in all proportions
-- e.g.,
F actors Affecting the Rate of Dissolution
1. temperature

2. particle size

3. mixing
4. nature of solvent or solute
C lasses of Solutions
aqueous solution:

amalgam:
e.g.,
tincture:
e.g.,

organic solution:
e.g.,
Non-Solution Definitions
insoluble: “will NOT dissolve in”
e.g.,
immiscible: refers to two liquids that will NOT form a solution
e.g.,
suspension: appears uniform while being stirred, but settles over time
e.g.,
Molecular Polarity
nonpolar molecules: -- e– are shared equally
-- tend to be symmetric
e.g.,
polar molecules: -- e– NOT shared equally
e.g.,
“Like dissolves like.”
Using Solubility Principles
C hemicals used by body obey solubility principles.
-- water-soluble vitamins: e.g.,
-- fat-soluble vitamins: e.g.,
Dry cleaning employs ___________ liquids.
-- ________ liquids damage wool, silk
-- also, dry clean for stubborn stains (ink, rust, grease)
-- tetrachloroethylene was in
longtime use
emulsifying agent (emulsifier): --
--
e.g., soap detergent lecithin eggs

soap vs. detergent
-- --
--
Hard water contains minerals w/ions like Ca2+, Mg2+, and Fe3+ that
replace Na+ at polar end of soap molecule. Soap is changed
into an insoluble precipitate (i.e., soap scum).
micelle: a liquid droplet covered w/soap or detergent molecules

Solubility
unsaturated: sol’n could hold more
solute;
saturated: sol’n has “just right” amt.
of solute;
supersaturated: sol’n has “too much” solute
dissolved in it;
Solids dissolved in liquids Gases dissolved in liquids


As To , solubility ___ As To , solubility ___
Solubilities of Selected Solutes in Water

EX. Using an available solubility curve, classify as unsaturated,
saturated, or
supersaturated.
per
100 g
H2O
80 g NaNO3 @ 30oC
45 g KCl @ 60oC
30 g KClO3 @ 30oC
70 g Pb(NO3)2 @ 60oC
Per 500 g H2O, 100 g KNO3 @ 40oC
EX. Describe each situation below.

( A) Per 100 g H2O, 100 g NaNO3 @ 50oC.

( B) Cool sol’n (A) very slowly to 10oC.

( C) Quench sol’n (A) in an ice bath to 10oC.
Glassware – Precision and Cost beaker vs. volumetric flask
1000 mL + 5% 1000 mL + 0.30 mL

When filled to 1000 mL line,
how much liquid is present?

Concentration…a measure of solute-to-solvent ratio
concentrated dilute
Selected
units of
concentration
A. mass % = mass of solute x 100
mass of sol’n
B. parts per million (ppm) = mass of solute x 106
mass of sol’n
 also, ppb and ppt
-- commonly used for minerals or contaminants in water supplies

C. molarity (M) = moles of solute
L of sol’n
-- used most often in this class
EX. How many mol solute are req’d to make 1.35 L of 2.50 M sol’n?
What mass sodium hydroxide is this?
What mass magnesium phosphate is this?
EX. Find molarity if 58.6 g barium hydroxide are in 5.65 L sol’n.
EX. You have 10.8 g potassium nitrate. How many mL of sol’n will make
this a 0.14 M
sol’n?
M olarity and Stoichiometry
EX. __Pb(NO3)2(aq) + __KI (aq)  __PbI2(s) + __KNO3(aq)
What volume of 4.0 M KI sol’n is req’d to yield 89 g PbI2?
Strategy: (1)
(2)
EX. How many mL of a 0.500 M CuSO4 sol’n will react w/excess Al to
produce 11.0 g Cu?
Dilutions of Solutions  Acids (and sometimes bases) are purchased in
concentrated form (“concentrate”) and are easily diluted to any
desired concentration.
**Safety Tip:
Dilution Equation:
EX. Conc. H3PO4 is 14.8 M. What volume of concentrate is req’d to make
25.00 L of
0.500 M H3PO4?
How would you mix the above sol’n?
1. Measure out ________ L of conc. H3PO4.
2. In separate container, obtain ~20 L of cold H2O.
3. In fume hood, slowly pour H3PO4 into cold H2O.
4. Add enough H2O until 25.00 L of sol’n is obtained.
EX. You have 75 mL of conc. HF (28.9 M); you need 15.0 L of 0.100 M
HF. Do you have
enough to do the experiment?
Dissociation occurs when neutral combinations of particles
separate into ions while in aqueous solution.
sodium chloride NaCl 
sodium hydroxide NaOH 
hydrochloric acid HCl 
sulfuric acid H2SO4 
acetic acid CH3COOH 
In general, ________ yield hydrogen (H+) ions
in aqueous solution; ________ yield hydroxide (OH–) ions.

Strong electrolytes exhibit nearly 100% dissociation.
NaCl Na+ + Cl–
NOT in water:
in aq. sol’n:
Weak electrolytes exhibit little dissociation.
CH3COOH CH3COO– + H+
NOT in water:
in aq. sol’n:
electrolytes: solutes that dissociate in sol’n
-- conduct elec. current because of free-moving ions
-- e.g.,
-- are crucial for many cellular processes
-- obtained in a healthy diet
--
nonelectrolytes: solutes that DO NOT dissociate
--
-- e.g.,
Colligative Properties 

Compared to solvent’s… a sol’n w/that solvent has a…
…normal freezing point (NFP)
…normal boiling point (NBP)
Applications of Colligative Properties (NOTE: Data are fictitious.)
EX. salting roads in winter
FP
BP
water
water + a little salt
water + more salt
EX. antifreeze (AF) (a.k.a., “coolant”)
FP
BP
water
water + a little AF
50% water + 50% AF
EX. law enforcement
white powder
starts
melting at…
finishes
melting at…
penalty, if
convicted
A
B
C
10

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