Chapter 6 : Solutions, Acids, & Bases. Solution Solute Solvent Concentration Molarity Suspension...
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Transcript of Chapter 6 : Solutions, Acids, & Bases. Solution Solute Solvent Concentration Molarity Suspension...
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Chapter 6 : Solutions, Acids, & Bases
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Solution Solute Solvent Concentration Molarity Suspension Colloid Acid Base Solubility
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Types of Mixtures
Heterogeneous: not the same throughout
Homogeneous: uniform throughout (completely mixed)
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Heterogeneous MixturesSuspensions: a mixture that
looks uniform when stirred or shaken that separates into different layers when it is no longer agitated.
Example: oil & vinegar , orange juice
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Heterogeneous Mixtures Colloids: A mixture of very tiny
particles of pure substances that are dispersed in another substance but do not settle out of the substance.
Example: Jello
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Particles in a colloid are much smaller than those in a suspension and do not settle at the bottom.
The particles stay dispersed throughout the mixture.
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Heterogeneous Liquid-Liquid Mixtures
Liquids that will not dissolve into one another are Immiscible (they do not mix) Example: Oil & Vinegar
The oil is less dense & Floats above the vinegar
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Emulsions Some immiscible liquids can mix in
emulsions. Example: Mayonnaise
An Emulsion is any mixture of immiscible liquids in which the liquids are spread throughout one another
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Homogeneous MixturesUniform throughout
Example: Salt water
Solutions are homogeneous mixtures of two or more substances uniformly spread throughout a single phase
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SolutionsThere are 2 main parts to a solution:
Solute: The substance that dissolves in a solution
Solvent: The substance that dissolves the solute to make a solution
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Miscible Two or more liquids that form a
single layer when mixed are Miscible.
Miscible liquids can be separated by Distillation.
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Chapter 6 Section 2: Dissolving & SolubilitySolutes with a larger surface area will dissolve faster.
Is dissolving a chemical change?
NO it is a Physical Change (pg. 60)
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A substance in small pieces dissolves faster than the same substance in big pieces.
Stirring or shaking a solution helps the solute dissolve faster
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“Movement” does what to the particles in a substance?
Adds energy which increases the speed of the particles
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Solutes dissolve faster when the solvent is Hot
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Not every substance dissolves
Substances can be Soluble and Partly Soluble
Soluble: dissolves in water
Partly Soluble: does not completely dissolve in water.
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Water is the Universal Solvent!Water’s structure helps it dissolve charged particles.
Why? What is the structure of water?
Water is a polar molecule which allows it to dissolves substances easily
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Like Dissolves Like
Water will not dissolve all substances.
Water cannot dissolve substances that are considered “nonpolar”
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Concentration
The quantity of solute dissolved in a given a solution
Solutions can have different concentrations depending on the amount of solute & solvent
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A solution that is dilute has a large amount of solvent compared to solute
A Concentrated Solution has a large amount of dissolved solute.
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Unsaturated vs. Saturated Solutions
Unsaturated solutions can dissolve more solute.
They have more space available for particles to move (spread out).
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Unsaturated vs. Saturated Solutions
*Considered “Unsaturated” as long as a solution can dissolve more solute.
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Unsaturated vs. Saturated Solutions
A Saturated Solution is a solution that cannot dissolve any more solute at the given conditions
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SolubilityThe greatest quantity of a solute that will dissolve in a given quantity of solvent to produce a saturated solution.
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Heating a saturated solution usually allows you to dissolve even more solute.
The Solubility of most solutions will increase as the temperature increases.
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Supersaturated solution!!A solution holding more dissolved solute than is specified by its solubility at a given temperature.
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SupersaturatedSupersaturated solutions are unstable systems because the solute’s solubility is exceeded for a short time.
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Measuring Concentration Precisely
Concentration can be measured/expressed in grams per 100g of solvent or as a mass percent or in grams per 100g of solution.
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Measuring Concentration Precisely
Concentration can also be expressed in units of Molarity
Molarity: is a concentration unit of a solution that expresses moles of solute dissolved per liter of solution.
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MolarityMolarity = moles of solute
liters of solution
*Molarity is the preferred concentration unit because it expresses the molar amount of solute present*
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What are acids?
An Acid is a substance that creates hydrogen ions H+ ◦ will form Hydronium ions when dissolved in water.
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Acids have a pH below 7
Indicators can be used to determine the acidity of a substance.
Litmus paper can be used as an acid indicator◦Acids will turn blue litmus paper red.
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Acidic solutions have similar properties
Sour taste
Can burn skin or eyes
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All acids can conduct electricity when dissolved in water because all acids for hydronium ions (H3O+).
Strong acids will conduct electricity better than weak acids
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Ions created as acids dissolve in water move throughout the solution conducting electricity.
Sulfuric Acid in water conducts electricity in car batteries.
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Weak acids do not ionize completely & will not conduct electricity
◦Example: Acetic Acid (Vinegar)
Fewer ions (charges) = less conductivity
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Basic solutions have similar properties
Bitter taste
Slippery
Bases have a pH Above 7
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Some bases produce Hydroxide ions (OH-)
Bases cause red Litmus paper to turn Blue
Can be very dangerous if not diluted with water
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Like acids, bases can conduct electricity
Strong Bases will conduct electricity better than weak bases.
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Example:
◦Potassium hydroxide (KOH) is a base found in some drain cleaners.
◦KOH is a strong base & solutions will conduct electricity well (more charges/ions)
◦KOH K+ + OH-
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pH values correspond to the concentration of hydronium ions & hydroxide ions.
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A reaction between hydronium ions & hydroxide ions to form water molecules
The resulting solution is more neutral than either of the reactants.
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Strong Acids & Bases react to form water & salt
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Some acid-base reactions do not result in neutral solutions
The pH of the solution depends on the amounts of acid & base that are combined
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CHAPTER 6 SECTION 4: ACIDS & BASES IN THE HOME
Bases in the home…
Soaps (emulsifier) Cleaning Products Detergents Ammonia SolutionsDisinfectants (Bleach)
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OTHER ACIDS & BASES AT HOME…
Antacids are weak bases that neutralize excess stomach acid.
Shampoos are made of detergents that are able to remove dirt & oil without leaving
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Know VocabularySolution
Solute
Solvent
Acid
Bases
Concentration
Molarity
Solubility
Suspension
Colloid
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Know key facts about acids & bases:
Which creates H+ ions?
Which creates OH- ions?
Which can conduct electricity & why?
Which have a pH below 7?
Which have a pH above 7?
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Know key facts about the types of mixtures:What are the 2 main types?
What category do suspensions & colloids fall into?
How are they similar and different?
What are immiscible liquids? Example:
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What can be used to mix immiscible liquids?
Emulsifier
Example:
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A mixture of a strong acid and a strong base will create…Salt & Water
Or a neutralized reactionCloser to what pH? _7_
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Compare & Contrast…
Concentrated & Diluted
Saturated & Unsaturated
Polar & Nonpolar
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Solubility
Know …
Its definition
How it can change based on temperature
How to read a solubility curve
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This is an example of what type of reaction?
2Al + 3CuCl2 2AlCl3 +3Cu
a. Decomposition c. Double Displacement
b. Synthesis d. Single Displacement
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What is the substance that gets dissolved by a solvent in a solution?
A solution is considered acidic if it contains…More hydrogen ions than hydroxide ionsMore hydroxide ions than hydronium ionsEqual amounts of hydroxide ions and
hydrogen ionsLess hydrogen ions than hydroxide ions
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A solution that has a greater amount of solvent than solute would be
Which of the following is an example of a situation in which exothermic chemical reactions occur?a. Ice cubes melt into water.b.Boiling pots of water turn to steam.c .Fireworks explode during a holiday.d. Pieces of KCl dissolve in water.
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Which of the following would have an effect on the solubility of a solution?a. The surface area of the solute b. The temperature of the solventc. Stirring the solutiond. All of the above
A substance with a pH of 2 hasa. The same number of H3O+ ions as it
does OH- ionsb. More H3O+ ions than OH- ions
c. no H3O+ ions or OH- ions
d. More OH- ions than H3O+ ions
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An equation that uses chemical symbols & formulas to summarize a reaction
A protein catalyst that speeds up a specific reaction
A reaction of at least 2 substances that forms a new complex compound; combines
A reaction in which a one element takes the place of another single element in a compound
. The specific substance affected by an enzyme