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Solutions, Acids, and Bases
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Parts of a solution
Solute The substance that
is dissolved into the solution.
examples: • Sugar in kool-aid• Salt in salt water
• CO2 in pop
Solvent The substance that
does the dissolving in a solution.
examples:• Most common is
water.
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Dissolving
Three ways to dissolve a solute in a solvent:
1. Dissociation
2. Dispersion
3. Ionization
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1. Dissociation
The process in which an ionic compound separates into ions in a solution. (physical change)
Example: salt in water
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2. Dispersion
Breaking the solute into small pieces and spreading throughout the solvent.
Ex. Sugar in waterPhysical change
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3. Ionization
The process in which neutral molecules lose or gain electrons.
Chemical changeEx: HCl in water
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Conductivity
Many solutions can conduct an electric current if electrolytes are present. (ions)
Electrolytes = substances that will conduct an electric current when dissolved. Ex. NaCl, KCl, MgBr2
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Freezing Point Depression
Lowering the freezing point of water by the addition of a solute
ex. salt. Used on icy roads in
winter Ice-cream
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Boiling point elevation
The addition of a solute to a liquid solvent will usually raise the boiling point of the solvent.
Adding salt to boil water when cooking
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Rate of Solution
Speed at which solute dissolves in a solvent.
1st Stirring the solution. Helps to move the solute particles away from the solid solute.
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Other factors:
2nd : Powdering the solute.
Increases the surface area
3rd : Heating the solution.
Speeds up the molecules
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Concentration
ConcentratedA large amount
of solute dissolved in a solvent
DiluteA little bit of
solute dissolved in a solvent
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Saturation
A solution that contains all the solute it can possibly hold at a given temperature is said to be saturated.
Unsaturated = contains less solute than it can possibly hold
Supersaturated = a solution that holds more solute than it should at a given temperature.
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Supersaturation example:
Sodium acetate in water.
Used in commercial hand warmers.
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Page 692 Q1 - 3
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Insoluble
A substance that will NOT dissolve in water.
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“Like dissolves like”
Nonpolar solvents will dissolve nonpolar solutes.
examples: benzene & acetone Polar solvents will dissolve polar solutes
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2 factors that affect solubility:
1.Temperature Increase in temp
generally increases solubility of a solid in a liquid
Increase in temp decreases solubility of a gas in a liquid.
2. Pressure Usually has little, if
any, effect on solid and liquid solutes.
Increase in pressure increases the solubility of a gas in a liquid.
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Acids
Very important chemicals in everyday life processes.
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Properties of acids:
1. Sour taste (never taste a chemical)
2. All contain hydrogen ( which turn into hydronium ions H3O+)
3. Also called “proton donors”
4. React with active metals to produce hydrogen gas. (exp. 21)
Zn + 2HCl ZnCl2 + H2
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Indicators
Chemicals used to identify acids and bases by changing color.
ACIDS:
A. Litmus paper (blue to red)
B. Phenolphthalein (colorless)
C. Methyl Orange (orange to red)
D. Bromothymol Blue (changes to yellow)
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Common acids
Sulfuric (H2SO4) used in car batteries
Nitric (HNO3) also fertilizers
Hydrochloric (HCl) stomach acid Carbonic (H2CO3) carbonated drinks
Acetic (HC2H3O2) vinegar
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Bases
Also very important in everyday processes.
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Properties of Bases:
Taste bitter; feel slippery Contain hydroxide (OH) ions. Known as “proton acceptors” Phenolphthalein turns bright pink Red litmus paper turns blue Bromothymol blue turns blue Methyl orange turns yellow
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Common bases:
Sodium hydroxide NaOH making soap; drain cleaners
Potassium hydroxide KOH battery electrolyte
Calcium hydroxide Ca(OH)2 making plaster and drywall
Magnesium hydroxide Mg(OH)2antacids
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Solutions of acids and bases
pH scale (page 704) A numerical scale developed to
measure the relative strengths of acids and bases
Ranges from 0 to 14 0 is the strongest acid 14 is the strongest base.
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What happens when an acid and a base combine? Always forms water and a salt. Salt = ionic compound formed when a
positive ion of a base combines with a negative ion of an acid.
Neutralization.
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What determines if an acid is classified as “strong” or weak? Which is stronger? 1 M acetic acid or
1M hydrochloric acid? Strength is determined by how well the
acid or base dissociates into solution. Strong acids and strong bases are good
electrolytes.
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Buffers
A mixture of a weak acid or weak base with its salt.
Resists large changes in pH.
Examples:– Bicarbonate ions in
your blood stream.