Tuesday 13 May 2014

Solution and Suspension PPT - part1

 

Solutions and Suspensions
part 1 – Matter, Solutions


Kalam Kudus Christian School

Chemistry Checkpoint 2

Mr. Markus


                          

Pure Substance


  • A type of matter in which all particles are of the same chemical composition (element, compound)

    • Au (pure gold)

    • H2O

    • NaCl

    • Sugar (C6H12O6)

    • Ar

  • Which of the previous examples is a compound?  an element?

  • Why is salt water not a pure substance?

01-gold-bar.jpg

Mixtures


  • Two or more pure substances physically mixed together.

  • Cannot be represented by a chemical formula.

    • Salt water

    • Sand and rocks

    • Air


Beakers

Heterogeneous Mixture


  • A mixture where substances are not evenly distributed (non uniform)

    • oil and vinegar salad dressing

    • vegetable soup

    • sand and sugar

    • soil

    • granite

Sample of Granitegranite

Homogeneous Mixture (Solution)


  • A mixture where all components are evenly distributed (uniform).

  • “same throughout”

    • salt water

    • gasoline

    • syrup

    • air

Battery-jar-water-beaker

Practice


  • Identify each of the following as:

    • pure substance/mixture

    • element/compound


mlcls

Definition of Solutions


  • A solution is a homogeneous mixture in which one substance is dissolved in another substance

  • The solute is(are) the substance(s) present in the lesser amount(s), dissolved by the solvent

  • The solvent is the substance present in the larger amount, does the dissolving/dissolves the solute



Solution


  • Formed when one substance is dissolved by another.

  • In order to be dissolved, a substance must be soluble.

  • A homogeneous mixture.

  • Particles are evenly distributed.

  • Parts cannot be separated by filtering.

  • Solvent—does the dissolving

  • Solute—dissolved by the solvent


180px-SaltInWaterSolutionLiquid

Solution Practice


  • Identify the solute and solvent in each of the following:

    • Salt water

    • Iced tea

    • Coca-cola coke

    • Paint/paint thinner

    • Nail polish/acetone

    • Ethanol



Tea_Glass3

Types of Solutions

Kirk_effect
  • Solid dissolved in a liquid.

    • Salt water

  • Gas dissolved in a liquid

    • Coca-cola

  • Two solids

    • Metal alloys: brass = copper + zinc

  • Two gases

    • Air: nitrogen (78% vol), oxygen (21% vol), argon (1% vol), carbon dioxide (0.03% vol).

  • In solutions of 2 solids or 2 gases, the solvent is the component present in largest quantity. 


IONIC COMPOUNDS
Compounds in Aqueous Solution


Many reactions involve ionic compounds, especially reactions in water — aqueous solutions.


K+(aq)  +  MnO4-(aq)


KMnO4 in water


Aqueous Solutions


How do we know ions are present in aqueous solutions?



They are called ELECTROLYTES

HCl, MgCl2, and NaCl are strong electrolytes. They dissociate completely (or nearly so) into ions.



Aqueous Solutions


Some compounds dissolve in water but do not conduct electricity.  They are called nonelectrolytes.


Examples include:

sugar

ethanol

ethylene glycol


npo00008anpo00008cnpo000088

nonelectrolyte


weak electrolyte


strong electrolyte


Electrolytes in the Body

 

Make your own

50-70 g sugar

One liter of warm water

Pinch of salt

200ml of sugar free fruit squash

Mix, cool and drink


  • Carry messages to and from the brain as electrical signals

  • Maintain cellular function with the correct concentrations electrolytes

gatorade_products




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