mL () 1000 L . 1060 () gmol - Loyola University Chicago - g ml to g liter

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• (1) Gram liter to g ml
• (2) Liters to grams calculator
• (3) Convert g ml to liters
• (4) Milliliters to liters

"A" students work
SOLUTIONS
(without solutions manual) solvent
~10 problems/night.
solute
Dr. Alanah Fitch
Flanner Hall 402
508-3119
afitch@luc.edu
Office Hours Th & F 2-3:30 pm
Define some measurement scales and units G3: Science Is referential
Module #13 molessolute
Solution Properties 1. Molarity M =
Lsolution
Defining types of concentrations 2. mole fraction nA A
For mixtures nA + nB .
3. molality molality = m = molessolute
kg solvent
Method for Conversion from Molarity to molality Example Density of an aqueous solution of ammonium sulfate is 1.06g/mL and the
molarity is 0.886. What is the molality? ( NH4 )2
SO4
1. Assume 1 L volume
2. Calculate moles of solute 1. Assume 1 L volume Atoms amu total
molessolute 2. Calculate moles of solute
Lsolution (1L) = molessolute molessolute 2 N 14.01 28.02
Lsolution (1L) = molessolute = 0.886 8( H) 8(1.008) 8.064
S 32.07 32.07
4(O) 4(16.00) 64
3. Calculate g of solution from d, V 3. Calculate g of solution from d, V total 133.098
103 mL
d solution L (1Lsolution ) = gsolution
g 1000mL
1.06 mL L ( Lsolution ) = 1060gsolution
4. Calculate g of solute from M
M (1Lsolution ) gsolute 4. Calculate g of solute from M
molsolute = gsolute mol
5. Subtract to get g of solvent 0.886 L (1Lsolution ) 133.098gsolute
molsolute = 117.9248gsolute
5. Subtract to get g of solvent
gsolution - gsolute = gsolvent 1060gsolution - 117.9248gsolute = 942.1gsoluent
6. Calculate g solute/g solvent
molality = m = molessolute 6. Calculate g solute/g solvent
kgsolvent
molality = m = molessolute = 0.886molessolute = 0.941
kgsolvent 0.9421kgsolvent
1
Method for Conversion from molality to Molarity Example Density of an aqueous solution of KOH is 1.43g/mL and the molality is
1. Assume 1 kg solvent 14.2. What is the molarity?
2. Calculate moles of solute 1. Assume 1 kg solvent
molessolute 2. Calculate moles of solute
kgsolvent 1kgsolvent = molessolute
14.2molesKOH
3. Calculate g of solute from MM 1kgwater [1kgwater] = 14.2molesKOH
(molessolute ) gsolute
molessolute = gsolute 3. Calculate g of solute from MM
4. Sum masses to get total mass of solution [14.2molesKOH] 39.10 + 16.00 + 1.08gKOH
moleKOH = 797.756gKOH
1000gsolvent + gsolute = gsolution 4. Sum masses to get total mass of solution
5. Calculate V of solution from density gsolution = gH2O + gKOH = 1000g + 797.756g = 1797.756gsolution
(gsolution ) mLsolution L
gsolution 103 mL = ( Lsolution ) 5. Calculate V of solution from density
6. Calculate moles/V (1797.756gsolution ) 1mLKOHsolution
M=
1.43gKOHsolution = 1,257.17mL
molessolute
Lsolution 6. Calculate moles/V
moles =
14.2moles,KOH = 11.296
M = Lsolution 1.257 LKOHsolution
Methods of measurement are related but not equivalent "A" students work
16 50 (without solutions manual)
Density
14 Molality 45 ~10 problems/night.
Weight %
40
12
35
10 30
Dr. Alanah Fitch
Flanner Hall 402
8 25 508-3119
afitch@luc.edu
6 20
15 Office Hours Th & F 2-3:30 pm
4
10
25
Module #13
Solution Properties
00
0 2 4 6 8 10 12 14 16
Molarity Water/Salt Solutions 1
2
Molaity or (densityx10)
weight percent
SOLUTIONS A mixture is usually plotted as variation in mole fractions
Any two components A and B
nnnAAA +++ nnnBBB == nnBB ++ nnBB = 1
AAA +++ BBB === nnnAAA +++ nnnBBB ... nnnAAA +++ nnnBBB ... nnAA ++ nnBB ..
nB B nA A
Mixed in any mole fraction nA + nB .
nA + nB.
1
0.8
0.6
0.4
0.2
0
B A 0 0.2 0.4 0.6 0.8 1
Solvent is usually Solute is usually Pure B moles of A Pure A
Considered the "dissolver" Considered the "dissolved"
mixture
Solvation Diagrammed as an Example of Hess's Law
kJ
2- H = - 91.2 mol
2+ + SO4,aq
SOLUTIONS MgSO4,s H2O Mgaq
solvent Any two components A and B
solute
Mixed in any mole fraction
-1284.9kJ
mole
-1376.1kJ
mole
water
kJ
2- H = - 91.2 mol
2+ + SO4,aq
MgSO4,s H2O Mgaq
3
mole fraction


How to convert from ML to liter?Common conversions from mL to liters:100 mL = 0.1 L250 mL = 0.25 L500 mL = 0.5 L750 mL = 0.75 L1000 mL = 1 L1250 mL = 1.25 L1500 mL = 1.5 L1750 mL = 1.75 L2000 mL = 2 L

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