solution: a homogeneous mixture solute: substance that gets dissolved solvent: substance that does...
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solution:
a homogeneous mixture
solute: substance that gets dissolved
solvent: substance that does the dissolving
tincture: sol’n in which alcohol is solvent
aqueous: water is solvent
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water is an excellent solvent because of its polarity
salt dissolving in water
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hydrochloric acid dissolving in water
δ+ HCl δ-δ+ HCl δ-
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“like dissolves like”
polar mixes w/ polar; nonpolar w/nonpolar
miscible: two liquids that mixex: water and alcohol
immiscible: liquids that don’t mix
ex: water and oil
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types of compounds that dissolve in water
I. Ionic (metal w/nonmetal) ex: NaCl, KI
II. Acids (H+ w/ anion) ex: HCl, H2SO4
III. polar covalent ex: NH3, H2O2
cmpds w/ -OH groups ex: sugars, alcohols
ethanol: glucose: C6H12O6C2H5OH
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compounds that don’t dissolve in water
nonpolar covalent cmpds
ex: hydrocarbons like C4H10
symmetrical molecules like CCl4
Conductivity of Solutions
Electrolyte:
cmpd that dissociates into ions; conducts electricity
must be ionic cmpd or an acid ex: CuSO4, HNO3
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nonelectrolyte: doesn’t dissociate; won’tconduct
covalent cmpds that are not acids
ex: sugar, C12H22O11
alcohols, C2H5OH
Sample problems: determine formula,classify as soluble or insoluble, electrolyte or non
acetic acid HC2H3O2 sol. elec.
calcium chloride CaCl2 sol. elec.
Hexane, C6H14 insol. nonelec
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silver nitrate
methanol
hydrochloric acid
butane
potassium iodide
AgNO3 sol, elec
CH3OH sol, nonelec
HCl sol, elec
KI sol, elec
C4H10 insol, nonelec
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saturated, unsaturated, supersaturated
saturated sol’n:
contains the maximum amt of dissolved solute;equilibrium btwn dissolved and undissolved solute
unsaturated sol’n:contains less than max. amt of solute
supersaturated sol’n
contains more than the normal amt of solute
crystallizes completely by adding a “seed”crystal of the solute.
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solubility: concentration of a saturatedsol’n
ex: solubility of NaCl at 25°C is 36g/100 mL
Effect of temperature on solubilitysolid solutes:solubility increases as temp increases
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Gases and solubility
Effect of temp decreasing temp (water)increases solubility of gas
Effect of pressure Increasing pressure(over the water) increasessolubility
cold, high pressure
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solubility curves
What is the solubilityof ammonium chlorideat 70°C ?
61 g/100 mLHow many gramsof potassium nitratewill dissolve in 100 mL water at 50°C?
83 g
How many gramsKNO3 will saturate250 mL water at 50°?
207.5 g
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100 mL of saturated potassiumchlorate sol’n is cooled from80°C to 30°C? How many gramsof solute will crystallize?
at 80°: 42 g
at 30°: 12 g
30 gHow many grams staydissolved? 12 g
a sol’n contains 20 g sodium chloride dissolved in 100 mLwater at 25°C; is it saturated,unsaturated, or supersaturated?
unsaturated
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Solution Concentration
dilute: contains little solute
concentrated: contains a lot of solute
ways to indicate concentration
percent: mass of solutetotal mass sol’n
100
ppm: parts per million ppb parts per billion
Molarity (M):moles solute
Liter of sol’n
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Calculating Molarity M= MOL L
What is the molarity of a sol’n made by dissolving0.25 mole of sucrose in enough water to make 100.0 mL of sol’n ?
M= 0.25 mol 0.1 L
2.5 M
What is the molarity of a sol’n that contains 30.0 grams of sodium hydroxide dissolved in 0.50 liter of sol’n?
30.0 g
g
mol1
40
0.75 mol
0.50 L1.5 M
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How many moles of HCl are contained in 5.0 litersof a 6.0 M HCl solution?
M= MOL L
6.0 M X mol
5.0 LX = 30 mol
How many grams of potassium sulfate are neededto dissolve in water to make 250 mL of a 2.0-molarsolution? K2SO4
2.0 MX mol
0.25 LX = 0.5 mol
0.5 mol
1 mol
174.3 g87 g
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Calculate the molarity of a solution that has 12.5 g ofglucose, C6H12O6, dissolved in 500 mL of solution.
12.5 g
g
mol1
1800.06944 mol
0.5 L0.14 M
How many moles and grams of potassium iodide would be needed to prepare 0.75 liter of a 0.15 Msolution?
0.15 M = x mol 0.75 L
X = 0.1125 mol
0.1125 mol
mol1
g16718.8 g
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Diluting a Solution M1V1 M2V2
concentrated diluted
If 100.0 mL of 6.0 M NaOH solution is diluted withwater to 800.0 mL, what is the molarity of the diluted solution?
(6.0 M) (100.0 mL) (800.0 mL)M2
800 mL800 mL
M2 = 0.75 M
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(12.0 M) V1 (1.0 L)(3.0 M)
12.0 M12.0 M
What volume of 12.0 M HCl solution is needed to make 1.0 liter of 3.0 M solution of HCl ?
25.0 mL of concentrated acetic acid (17 molar) arepipetted into a flask. Water is added to the 1.0 literMark. Calculate the molarity of the final solution.
V1 = 0.25 L
(17 M) (25.0 mL) (1000 mL)M2
1000 mL1000 mL
M2 = 0.43 M
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Colligative PropertiesProperties that depend on the concentrationof a solution
1. Lowering of vapor pressure
a solution has a lower V.P. than the puresolvent
pure water
water +a solute
the more concentrated the greaterthe effect
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2. Boiling Point Elevation
solutions have a higherB.P. than the pure solvent
more conc., higher the B.P.
100°C
B> 100°C
3. Freezing Point Depression
solutions have a lowerF.P. than the pure solvent
0°C
< 0°C
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Electrolytes vs. Nonelectrolytes
electrolytes dissociate into ions;
produces a higher concentration of dissolved solute particles
NaCl Na+ + Cl-
1 mol 2 moles ions
Nonelectrolytes don’t dissociate
C12H22O11 (s) C12H22O11 (aq)
1 mol 1 mol
Electrolytes have the greater
effect onC.P. ‘s
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examples:Which of these 1-molar solutions has thelowest freezing point?
AlCl3
KI
C12H22O11
Na2CO3
Al3+ + Cl-3
K+ + I-
C12H22O11
Na+ + CO3
2-2
4 ions
2 ions
1 molecule
3 ions
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Which of these 1-molal solutions has thehighest boiling point?
CuSO4 LiBr Mg(NO3)2 C6H12O6
2 2 3 1
Calculating Freezing & Boiling Point
ΔT = kf m ichange in F.P.
molality
freezing pt.constant
m = mol/kg solv.
ionization factor
ΔT = kb m i
kf = 1.86°C/mkb = 0.512°C/m
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Calculate the freezing & boiling point ofa 1.5-molal solution of sodium hydroxide.
F.P.
ΔT = kf m i
ΔT = (1.86 °C/m) (1.5 m) (2)
NaOH Na+ + OH-
ΔT = 5.58 °CF.P. = -5.6 °C
B.P.
ΔT = (0.512 °C/m) (1.5 m) (2)ΔT = 1.536 °C
B.P. = 101.5 °C
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Calculate the freezing and boiling point of a 2.0 maqueous solution of aluminum chloride.
AlCl3 Al+ + 3 Cl- ΔT = kf m i
ΔT = kbm i
ΔT = (1.86 °C/m) (2.0 m) (4)
ΔT = (0.512 °C/m) (2.0 m) (4)
ΔT = 14.88 °CF.P. = -15 °C
ΔT = 4.096 °C
B.P. = 104 °C