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![Page 1: Solutions Applied Chemistry 4.0. Background to Solutions A solution is a homogenous mixture that has different substances dissolved in it that cannot.](https://reader030.fdocuments.us/reader030/viewer/2022032415/56649efc5503460f94c0eecc/html5/thumbnails/1.jpg)
Solutions
Applied Chemistry 4.0
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Background to Solutions A solution is a homogenous mixture that
has different substances dissolved in it that cannot be seen.This results in a single physical state.
Parts of a solution Solute: substance that is dissolved
…present in smaller amount
Solvent: substance that does the dissolving
…present in larger amount
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Parts of a Solution
Solvent
Solute
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Properties of Solutions
Small particles
Evenly distributed particles (uniform)
Particles will not separate when at rest
The ability to dissolve (solubility)
Dissolving Salt Animation
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Background (cont.)
Soluble means something can be dissolved in something else.
Insoluble mean something cannot be dissolved in something else.
Dissolving a solid in a liquid can affect the boiling point and freezing point. This is called a colligative property.
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Types of SolutionsSolid Solutions
Solid solution – final phase is solid
Alloys: Solid solutions containing two or more metals or a metal and a nonmetal
Advantages of alloys over pure metals: Stronger Cheaper More resistant to corrosion Lighter Harder
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Examples of Alloys
Brass is an alloy of copper and zinc.
Steel is an alloy of carbon and iron.
Bronze is an alloy of copper and tin.
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A closer look at alloys
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Types of SolutionsGaseous and Liquid Solutions
Gaseous Solutions – final phase is gas Ex. Air
Liquid Solutions – final phase is liquid Miscible liquids: Can mix in all
proportions (ex. alcohol and water)
Immiscible liquids: Cannot mix in all proportions (ex. oil and water)
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Miscible Liquids
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Immiscible Liquids
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Types of Solutions
Aqueous Solutions
Solutions with water as the solvent.
Because water can dissolve so many things, it is called the Universal solvent.
Electrolyte – a solution that conducts electricity.
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Example of an electrolyte
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Other types of solutions Tincture: Solutions with alcohol as the
solvent (ex – herbal medicines) A saline solution is a solution of salt and
water.The solute is salt.The solvent is water.
A dilute solution is a solution with little solute.
A concentrated solution is a solution with a lot of solute.
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Concentration
A measure of the amount of solute in a solution.
% Concentration = mass of solute x 100 mass of solution
Usually used for concentrated solutions.
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Example: Salt water is prepared by mixing 3g of salt with 97g of water. Calculate % concentration.
Mass of solute:
Mass of solvent:
Mass of solution: (solvent + solute)
% Con:
3 g
97 g (water)
100 g
3 x 100 = 3%
100
Dilution: to decrease the concentration by adding more solvent
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Parts per million (ppm)-Usually used with dilute solutions.
One hundred or One thousand100 1000
One hundredth or One thousandth1/100 1/1000
One million or One billion1,000,000 1,000,000,000
One millionth or One billionth1/1,000,000 1/1,000,000,000
1 ppm 1 ppb
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Parts per million
Sea water is a 3% solution.
Means: 3 grams of salt to 100 grams of sea water or 3 parts salt to 100 parts sea water
Looks like: 3/100 dilution(keep as a fraction)
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ppm Examples
Food coloring is a 10% aqueous solution.
Means:10 grams of pigment to 100 grams of solution or 10 parts pigment to 100 parts of solution
Looks like: 10/100 dilution or 1/10 dilution
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Parts per Million Lab Cup 1 contained a 10% solution or a 1/10
dilution of food coloring. What did you do for Cup 2?
1 drop from Cup 1 + 9 drops of water for a total of 10 drops
You made a 1/10 dilution of a 10% solution orYou made a 1/10 dilution of a 1/10 dilution
Looks like: 1/10 of 1/10 Means 1/10 x 1/10 = 1/100 In Cup 2, you have 1/100 dilution of food
coloring. In Cup 2, you have a 1/100 x 100 = 1%
concentration.
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Other examples of ppm
1 ppm means 1 second in 12 days of your life.
1 ppm means 1 penny in $10,000.
1 ppm means one inch in 16 miles.
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Solubility and the Dissolving Process Solubility is a physical property that gives
the # of grams of solute that will dissolve in a solvent (usually 100 g of water) at a given temperature & pressure
Saturated: A solution is saturated if it contains as much solute as can possibly be dissolved under existing conditions of temperature and pressure.
Unsaturated: Has less solute than the maximum amount that can be dissolved.
Supersaturated: Has more solute than the maximum amount that can be dissolved.
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Unsaturated vs. Saturated Solution
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Supersaturated Solutions
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Three Factors Affecting the Rate of Dissolving
Surface Area – increases the number of collisions between the solute and solvent Sugar cube vs. sugar crystals
Stirring – increases the number of collisions between the solute and solvent. Stirring sugar in coffee/tea
Temperature – increases the energy of the collisions between the solute and solvent. Warm water vs. cold water
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Solubility Graph for NaNO3
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0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
So
lub
ilit
y (
g/1
00 g
wat
er )
Saturated sol’n
Supersaturated solution
Unsaturated solution
At 20oC, a saturated solution contains how many grams of NaNO3 in 100 g of water?
What is the solubility at 70oC?135 g/100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC?
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC?
supersaturated
90 g
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Solubility Graph for NaNO3
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110
120
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150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
So
lub
ilit
y (
g/1
00 g
wat
er )
At 20°C, a saturated solution contains how many grams of NaNO3 in 100 g of water?
What is the solubility at 70oC?
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC?
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC?