Review Chapter 8 & 9:
General, Organic, & Biological Chemistry
Janice Gorzynski Smith
Chapter 8 & 9 Concepts
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Identify the solvent and solute in a solution
Like dissolves like, predict which molecules will form solutions
Predict the effect of temperature or pressure on a solution
Perform concentration calculations & conversions
Perform dilution calculations
Predict relative changes in colligative properties between multiple
solutions
Understand osmotic pressure & how your kidney’s work.
Identify an acid/base reaction, the acid, base, conjugate acid/base
Caculate Ka, Kb
Use Kw to determine concentration of H3O+ or OHDiscuss how water acts as both an acid and a base
Perform titration calculations
Communicate how a buffer prevents large pH changes
2
CH 8 Equations & Conversions
Molarity = moles of solute (mol)
V of solution (L)
M1V1
=
M2V2
CH 9 Equations & Conversions
[H3O+][ A −]
[HA]
Ka =
-
Kb
=
Kw
=
[OH ][BH+]
[ B]
[H3O+][OH−] = 1.0 x 10−14
pH = -log[H3O+]
•Acidic solution:
pH < 7  [H3O+] > 1 x 10−7
•Neutral solution:
pH = 7  [H3O+] = 1 x 10−7
•Basic solution:
pH > 7  [H3O+] < 1 x 10−7
Solutions, Solubility, & Concentration
1. The solute is the substance present in a lesser amount.
2. The solvent is the substance present in a larger amount.
Solubility is the amount of solute that dissolves in a given
amount of solvent. REMEMBER: LIKE DISSOLVES LIKE.
 In aqueous or liquid phase solutions solubility increases with
increasing temperature
 Gases dissolved in liquids increase solubility with decreasing
temperature and increasing pressure
Communicate how much of a solute is dissolved in a solvent using
concentration:
 % w/v
Dilution: Adding more solvent to the initial solution.
 % v/v
The number of moles solute DOES NOT CHANGE.
 % mass / mass
M1V1
=
M2V2
 ppm
initial values
final values
 Molarity
Colligative Properties
Colligative properties are properties of a solution that depend on the
concentration of the solute but not its identity.
 One mole of any nonvolatile solute raises the boiling point
of 1 kg of H2O the same amount, 0.51 oC.
 One mole of any nonvolatile solute lowers the freezing point
of 1 kg of H2O by the same amount,1.86 oC.
Reverse Osmosis
Apply pressure to
reverse osmosis.
This is how our
kidneys filter blood
Acids / Bases
•A Brønsted–Lowry acid is a proton (H+) donor.
Strong:
•A Brønsted–Lowry base is a proton (H+) acceptor.
Weak:
gain of H+
H A
acid
+
A − +
H B+
conjugate conjugate
acid
base
B
base
loss of H+
−
H
O
Conjugate
base
Kw
remove H+
=
H
[H3O+][OH−]
O
H
H2O as a base
H2O as an acid
+
H
add H+
H
O
H
conjugate acid
Acid / Base Equilibrium & pH
H3O+(aq) + A
HA(g) + H2O(l)
acid dissociation
constant
Ka =
[H3O+][ A −]
[HA]
pH = -log[H3O+]
-
=
Low pH (0 ~ 7)
[H3O+] high
Acidic Conditions
OH- (aq) + BH+ (aq)
B (g) + H2O(l)
Base dissociation K
b
constant
− (aq)
[OH ][BH+]
[ B]
High pH (7 ~ 14)
[H3O+] low
Basic Conditions
Common Acid / Base Reactions
Neutralization reaction: An acid-base reaction that produces a salt and water.
H+(aq) + OH− (aq)
H—OH(l)
A bicarbonate base, HCO3−, reacts with one H+ to form carbonic acid, H2CO3.
H+(aq) + HCO3−(aq)
H2CO3(aq)
H2O(l) + CO2(g)
A carbonate base, CO32–, reacts with two H+ to form carbonic acid, H2CO3.
2 H+(aq) + CO32–(aq)
H2CO3(aq)
H2O(l) + CO2(g)
Titration
AH + B  A- + BH+
Acid + Base  Conjugate Base + Conjugate Acid
mole–mole
conversion
factor
Moles of
base
M (mol/L)
conversion
factor
[1]
Volume of
base
[2]
Moles of
acid
[3]
Volume of
acid
M (mol/L)
conversion
factor
Buffers
pH of buffer = -log[H3O+] where
[H3O+]
=
Ka
x
[HA]
[ A −]