Matter

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Matter

• Anything that has mass and takes up space.

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Substances Versus Mixtures

• Substances- cannot be separated by physical
  means.

• Mixtures- can be separated by physical means

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Pure Substance

• uniform composition
• All samples have identical properties like
  boiling point, melting pt., color, and density
  which can be used to identify the substance
• Review Are these intensive or extensive
  properties?

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Element

• Building block for everything else
• Cannot be broken down or separated by ordinary
  chemical or physical means
• Represented by chemical symbol
• Ex. Iron, copper, silver, hydrogen
• Remember the diatomic elements/molecules

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Compounds

• 2 or more different elements chemically combined
• Have different properties than components
• Separated into elements ONLY by chemical means
  (chemical reactions)
• Definite composition (constant element
  proportion)
• Represented by a chemical formula
• Ex. H2O (water), NaCl (sodium chloride)

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Mixture

• A physical blend of 2 or more substances
• Can be separated by physical means like
  filtration, distillation, etc.
• Individual components keep their identifying
  properties

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• Homogeneous mixture
• Components are uniformly distributed, there are
  parts but you cannot see them.
• Also called solutions.
• Ex. Salt water, air, brass

• Heterogeneous mixture
• Not uniform, you can see the parts
• Can settle upon standing
• Ex. Oil and vinegar, salt and pepper, soil, trail
  mix

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Classify

1. Which represent substances?
2. Which represent mixtures?
3. Which is an element?
4. Which is a heterogeneous mixture?

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CFU
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Separation Techniques
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MAGNETISM

• Use when one of the substances in the mixture
  is magnetic.

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FILTRATION

• Use when one of the substances in the liquid
  mixture is an insoluble solid
• Other information the insoluble substance is
  removed from the liquid mixture using a porous
  barrier (filter paper).

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EVAPORATION

• Use when the mixture is an aqueous solution
  containing a soluble solid
• Other information the water will boil off and
  the soluble solid will remain in the evaporating
  dish

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DISTILLATIONhttp//www.youtube.com/watch?v3VRi0K
PGb3o

• Use when the mixture is composed of two or more
  liquids
• Other information based on differences in
  boiling points liquid with lowest BP will boil
  (and then condense) first

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CHROMOTOGRAPHY

• Use when separating a mixture such as ink,
  chlorophyll
• Other information based on the distance the
  components of a mixture travel (mobile phase) on
  the surface of, or within, another material
  (usually cellulose paper, called stationary
  phase)
• https//www.youtube.com/watch?vZCzgQXGz9Tg

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Solutions

• A Homogeneous Mixture that can be separated by
  physical means.

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Solution Vocabulary

• Solution a homogeneous mixture that consists
  of
• Solute substance that dissolves, present in
  lesser amount
• Solvent thing that does the dissolving, present
  in greatest amount.

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heating curves

• solutions are NOT pure substances
• the amount of solute varies in solutions, and so
  does the BP and FP
• ?amount of solute, ?BP, ?FP
• heating curves for solutions will not be
  consistent

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Dissociate to separate into ions

• Electrolyte-any substance that dissociates and
  produces ions that conduct electricity.
• Ex. Salt (solute) dissociates in water and the
  solution conducts electricity

• Non-electrolyte any substance that does not
  dissociate and therefore does not contain ions
  that conduct electricity.
• Ex. Sugar (solute) does not dissociate in water
  so the solution does not conduct electricity

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Dissolving

• a solvent surrounds a solute
• Your body relies on water to dissolve
• the molecules in your body.
• Watch this

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• Soluble
• substance dissolves in solvent
• Ex. Sugar (solute) is soluble in water (solvent)

• Insoluble
• substance does not dissolve in solvent
• Ex. Sand is insoluble in water

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• Miscible- describes two liquids that do mix

• Immiscible describes two liquids that do not
  mix

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Solution Types

• Solvent is Gas ex. Air (nitrogen gas is the
  solvent)
• Solvent is Liquid ex. Sugar water (water is the
  solvent)
• WATER IS THE MOST COMMON SOLVENT AND IS CALLED
  THE UNIVERSAL SOLVENT
• Solvent is Solid ex. Nitrinol (titanium
  dissolved in nickel, nickel is solvent, used to
  make braces)

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Solubility

• Maximum amount of solute that will dissolve in a
  given amount of solvent at a given temp
  pressure
• Usually expressed as grams of solute per 100 g
  of solvent.
• Affected by changes in the temperature or pressure

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To Increase Solubility for a solid solute in a
liquid solvent

• Increase temperature of solvent
• Increase surface area of solute (crush)
• Agitate (stir or shake)
• Not affected by changes in pressure

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To Increase Solubility for a gas solute in a
liquid solvent

• Decrease temperature of solvent
• Increase pressure
• Not affected by surface area of solute

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Gas solubility
High Temp Low Temp
You want more gas particles in the liquid
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Saturated Solution

• contains the maximum amount of dissolved solute
  for a given amount of solvent at a specific temp
  and pressure.

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Unsaturated Solution

• contains less dissolved solute for a given temp
  and pressure than a saturated solution

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Supersaturated Solution

• contains more dissolved solute than a saturated
  solution at the same temp
• Must heat a saturated solution, then slowly cool

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Determining the solubility of a solution

• Add more solute seed crystal. If
• It dissolves, the original solution was
  unsaturated (still more available space).
• It does not dissolve and falls to the bottom of
  the container, the original solution was
  saturated (no more available space).
• It crystallizes, the original solution was
  supersaturated (over full, past capacity).

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Concentration is the amount of solute dissolved
in a given amount of solvent.

• Concentrated

• Dilute

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Molarity

• A unit of concentration
• The number of moles of solute dissolved in 1.00 L
  of solution.
• Molarity (M) Moles of solute
• Liter of solution

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Practice Problem

• What is the molarity if 2.0 moles of glucose are
  added to 5.0 L of solution?

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Preparing Molar Solutions
From the number of moles you need, calculate the
mass. Measure solute mass.
Add exact volume up to calibration mark. Close
lid, and swirl solution
Place solute in volumetric flask
http//wiki.chemeddl.org/mediawiki/index.php/3.5.1
_Concentration
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Changing the concentration

• Add more solvent (yellow)? decreases
  concentration
• The amount of solute is the same, but now the
  solution volume has increased
• How would you increae the concentration?
• http//wps.prenhall.com/wps/media/objects/1053/107
  8985/ist/ch03_11.html

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Solution Dilution

• When you need to make a concentrated solution
  more dilute, use this formula
• M1V1 M2V2
• M1 concentrated solution
• V1 amount of concentrated solution need to make
  dilute solution
• M2 dilute solution
• V2 amount of diluted solution wanted

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Practice

• How many liters of 16.8M HCl is need to make 2.5L
  of 3.5M HCl?

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Practice problem

• Mrs. Imamazing needs to make 12 liters of a 0.10
  M HCl solution for her chemistry students to use
  in a lab. She finds a large bottle of 12.00 M
  HCl solution in the acid cabinet. Describe how
  she would make the solution?

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Daltons Law of Partial Pressures

• at constant volume temperature, the total
  pressure exerted by a mixture of gases is equal
  to the sum of the partial pressures
• Total pressure P gas1 P gas2 Pgas3.
• Ptotal P1 P2 P3.

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Daltons Law

• What is the pressure of hydrogen, in atm, if it
  is mixed with oxygen, which exerts a pressure of
  2.1 atm, and the total pressure is 3.6 atm?

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Daltons Law

• Standard Deviants