Solution A homogeneous mixture of two or more substances.
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Transcript of Solution A homogeneous mixture of two or more substances.
Solution
A homogeneousA homogeneous
mixture of two ormixture of two or
more substances.more substances.
SolventSolvent - the substance present in the most amount.
SoluteSolute - the substance present in the least amount.
For Any Solution
SolventSolvent - there can be
only ONE
SoluteSolute - there can be
MORE than one
For Any Solution
SolventSolvent - the substance present in the most amount.
SoluteSolute - the substance present in the least amount.
What is the solventWhat is the solvent
in air?in air?
SolventSolvent - the substance present in the most amount.
SoluteSolute - the substance present in the least amount.
What are the solutesWhat are the solutes
in air?in air?
SolventSolvent - the substance present in the most amount.
SoluteSolute - the substance present in the least amount.
What is the solventWhat is the solvent
in stainless steel?in stainless steel?
SolventSolvent - the substance present in the most amount.
SoluteSolute - the substance present in the least amount.
What are the solutesWhat are the solutes
in stainless steel?in stainless steel?
SolventSolvent - Water
SoluteSolute - The substance dissolved in
water
Aqueous Solution
The amount of solute thatThe amount of solute that
can be dissolved in a givencan be dissolved in a given
amount of solvent, at aamount of solvent, at a
given temperature.given temperature.
Solubility
QuickTime™ and aTIFF (Uncompressed) decompressor
are needed to see this picture.
QuickTime™ and aTIFF (Uncompressed) decompressor
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QuickTime™ and aTIFF (Uncompressed) decompressor
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Is NaClIs NaClsolublesolublein Hin H22O?O?
A solution containing the A solution containing the
maximum amount of a solutemaximum amount of a solute
that is possible to dissolve in athat is possible to dissolve in a
given volume of solvent at agiven volume of solvent at a
given temperature.given temperature.
Saturated Solution
NaCl has a NaCl has a
solubility ofsolubility of
357 grams 357 grams
per liter of per liter of
"cold" H"cold" H22O.O.
Saturated Solution
++
How manyHow many
moles ofmoles of
NaCl areNaCl are
in thein the
solution?solution?
Saturated Solution
NaClNaClsolutionsolution
357 g NaCl 1 mole NaCl357 g NaCl 1 mole NaCl
Saturated Solution
NaClNaClsolutionsolution
58 g NaCl58 g NaCl
6.2 mole NaCl6.2 mole NaCl
==
How manyHow many
"particles" "particles"
of NaCl areof NaCl are
in thein the
solution?solution?
Saturated Solution
NaClNaClsolutionsolution
357 g NaCl 357 g NaCl
Saturated Solution
NaClNaClsolutionsolution
58 g NaCl58 g NaCl
3.7 X 103.7 X 102424 particles NaClparticles NaCl
==
6.02 X 106.02 X 102323 particles NaClparticles NaCl
A comparison of A comparison of
the amounts of the amounts of
solute and solventsolute and solvent
in a solution.in a solution.
Concentration
"Strong" and "Weak""Strong" and "Weak"
give SOME comparison,give SOME comparison,
but only a general idea.but only a general idea.
Concentration
"Dilute" and "Concentrated""Dilute" and "Concentrated"
still don't provide enoughstill don't provide enough
for quantitative calculations.for quantitative calculations.
Concentration
To do calculations, we mustTo do calculations, we must
know "how much" soluteknow "how much" solute
and "how much" solvent and "how much" solvent
are present.are present.
Concentration
M = M =
Molarity
moles solutemoles solute
dmdm33 solution solution
1 mole = formula mass (g)1 mole = formula mass (g)
1 liter = 1 cubic decimeter1 liter = 1 cubic decimeter
dmdm33
1 liter = 1000 milliliters
1 ml = 1 cm3
1. What is the molarity
of a liter of
solution containing
100 grams of
copper (II) chloride?
Molarity = moles
dm3
1 0 0 g C u C l 2
1 l i t e r
Molarity =moles
dm3
1 0 0 g C u C l 2
1 l i t e r
Molarity =
grams
moles
dm3
1 0 0 g C u C l 2
1 l i t e r
Molarity =
grams
mole
moles
dm3
1 0 0 g C u C l 2
1 l i t e r
Molarity =
grams
1 mole
moles
dm3
1 0 0 g C u C l 2 1 m o l e
1 l i t e r 1 3 4 g
Molarity =
Cu = 1 X 64 = 64Cl = 2 X 35 = 70
134
moles
dm3
1 0 0 g C u C l 2 1 m o l e 1 l i t e r
1 l i t e r 1 3 4 g 1 d m 3
Molarity =moles
dm3
1 0 0 g C u C l 2 1 m o l e 1 l i t e r
1 l i t e r 1 3 4 g 1 d m 3
Molarity =moles
dm3
Have we workedthe problem?
1 0 0 g C u C l 2 1 m o l e 1 l i t e r
1 l i t e r 1 3 4 g 1 d m 3
. 7 5 M C u C l 2
Molarity =moles
dm3
2. How much NaCl is
needed to prepare 250ml of 0.5M salt water
How is this problemdifferent from the first?
1. What is the molarity of a liter of
solution containing 100 grams of
copper (II) chloride?
2. How much NaCl is needed to prepare 250ml of 0.5M salt water?
The second GIVES M
The first ASKS for M
2.How much NaCl is needed to prepare 250 ml of 0.5 M salt water
250 ml 0.5 mole NaCl
dm3
Preparation
250 ml 0.5 mole NaCl
dm3
Preparation
What units will we havewhen the problem is worked?
250 ml 0.5 mole NaCl
dm3
Preparation
need grams
250 ml 0.5 mole NaCl
dm3
Preparation
need grams
250 ml 0.5 mole NaCl
dm3 1 mole NaCl
Preparation
need grams
250 ml 0.5 mole NaCl 58 g NaCl
dm3 1 mole NaCl
Preparation
need grams
250 ml 0.5 mole NaCl 58 g NaCl
dm3 1 mole NaCl
Preparation
Now What?need grams
250 ml 0.5 mole NaCl 58 g NaCl 1 dm3
dm3 1 mole NaCl 1000 ml
Preparation
need grams
250 ml 0.5 mole NaCl 58 g NaCl 1 dm3
dm3 1 mole NaCl 1000 ml
Preparation
7.3 grams NaCl
PracticeProblems
0.37 g CaCl2 1 mole 1000 ml
340 ml 110 g 1 dm3
0.01 M CaCl2
Practice Problem 1
50 cm3 0.2 mole Al(OH)3 78 g Al(OH)3 1 dm 3
dm 3 mole 1000 cm3
0.78 g Al(OH)3
Practice Problem 2
HomeworkProblems
50 g NaOH 1 mole 1000 cm3
200 cm3 40 g 1 dm3
6.25 M NaOH
Homework Problem 1
100 cm3 0.25 mole CaSO4 136 g 1 dm3
d m 3 mole 1000 ml
3.4 g CaSO4
Homework Problem 2
100 ml 0.5 mole HCl 36 g 1 dm3
dm3 mole 1000 ml
1.8 g HCl
Homework Problem 3
Making Dilutions
A solution can be made less concentrated by dilution with solvent
Making Dilutions
M1 V1 = M2 V2
original solution 1 = diluted solution 2
Volume units must be the same for both volumes in this equation.
Making Dilutions
How do you prepare
100ml of 0.40M MgSO4 from a stock solution
of 2.0M MgSO4?
Dilution Problem
M1 V1 = M2 V2
M1 = V1 =
M2 = V2 =
Dilution Problem
M1 V1 = M2 V2
M1 = 2.0M MgSO4 V1 = unknown
M2 = 0.40M MgSO4 V2 = 100ml
Dilution Problem
Step 1 - write the equation:
M1 V1 = M2 V2 Step 2 - manipulate the equation:
V1 = M2 V2 /M1
Step 3 - add the numbers:
V1 = (0.40M) (100ml) /2.0M
Dilution Problem
Step 4 - do the calculation:
V1 = 20ml
Step 5 - describe the preparation:
Add 80ml of distilled water to 20ml of the 2.0 M MgSO4 solution
Dilution Problem
HomeworkProblems
Molarity Calculations:
1. 0.975M (NH4)2C4H4O6 2. 0.257M CoSO4 3. 0.291M Fe(NO3)2
Preparations:
1. 390g NiCl2
2. 95.3g AgF 3. Use 50cm3 of the 1.0M
NaCl solution. Add 200cm3 of distilled water to make the total volume 250cm3.
Dilutions: 1. Add 19.2cm3 of 0.52M CoCl2 solution
to a graduate. Add distilled water to make the total volume 100cm3.
2. Add 72.5cm3 of 0.69M Ba(NO3)2 solution to a graduate. Add distilled water to make the total volume 200cm3.
3. Add 37.5ml of 2M NH4Br solution to a graduate. Add distilled water to make the total volume 500ml.
Solution Preparation
Other SolutionConcentrations
Molality
moles solutem = m =
Kg solventKg solvent
Normality
equivalentsequivalents soluteN = N =
dmdm33 solution solution