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?



  • Two or more pure substances physically mixed together.

  • Cannot be represented by a chemical formula.

    • Salt water

    • Sand and rocks

    • Air


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



  • Identify each of the following as:

    • pure substance/mixture

    • element/compound


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


  • 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


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


Types of Solutions

  • 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. 

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:



ethylene glycol



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


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