ACID,BASES AND SALT for Class 10th....CREATED TO PIYUSH BHANDARI
Acid, Bases & Salt Video
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Transcript of Acid, Bases & Salt Video
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Acid, Bases & Salt VideoAcid, Bases & Salt Video
Pre Test1. True
2. False
3. True
4. True
5. False
6. False
7. True
8. True
9. False
10. False
Post Test1. Neutralization
2. Base
3. Anion
4. Electrolytes
5. False
6. False
7. True
8. False
9. False
Post Test10. bitter, slippery, high
pH
11. Acids donate hydrogen, Bases accept Hydrogen
12. An easy way to gauge is something is a strong/weak acid or base
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Ch. 8Solutions, Acids, & Bases
Ch. 8Solutions, Acids, & Bases
III. Particles in Solution “Like Dissolves Like” Electrolytes
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A. “Like Dissolves Like”A. “Like Dissolves Like”
Polar substances will only dissolve in polar liquids• Rubbing alcohol and water
Nonpolar substances will only dissolve in nonpolar liquids• Oil and butter
Substances that aren’t the same don’t mix.• Oil and water
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A. “Like Dissolves Like”A. “Like Dissolves Like”
NONPOLAR
NONPOLAR
POLAR
POLAR
Detergents• polar “head” with long nonpolar “tail”• can dissolve both types (polar and nonpolar)
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B. ElectrolyteB. Electrolyte
An electrolyte is a substance that when dissolved in water form ions
Electrolytes get their name from the fact that the conduct electricity in water. Example: salt dissolved in water
Many sports drinks contain “electrolytes” which are salts dissolved in water
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B. ElectrolytesB. Electrolytes
ElectrolyteNon-
Electrolytesolute exists as
ions onlyEasily conducts electricity
- +
salt
- +
sugar
solute exists asmolecules only
Does NOT conduct electricity
- +
acetic acid
WeakElectrolyte
solute exists asions and
MoleculesSlightly conducts
electricity
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B. ElectrolytesB. Electrolytes
Dissociation• separation of +/-
ions when an ionic compound dissolves in water
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B. ElectrolytesB. Electrolytes
Ionization• breaking apart of
polar covalent molecules into ions when dissolving in water
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Ch. 8Solutions, Acids, & Bases
Ch. 8Solutions, Acids, & Bases
IV. Intro to Acids & Bases
Definitions Properties Uses
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A. AcidsA. Acids
• Acids contain at least one hydrogen atom that can be removed when the acid is dissolved in water.
• These form hydronium ions, H3O+.• Also called a proton donor
HCl + H2O H3O+ + Cl–
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A. BasesA. Bases
• Bases form hydroxide ions (OH-) in a water solution.
• a proton acceptor
NH3 + H2O NH4+ + OH-
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A. IndicatorsA. Indicators
• Indicators are an organic substance that changes color in an acid or base.
Examples:• litmus - red/blue• phenolphthalein - colorless/pink• goldenrod - yellow/red• red cabbage juice - pink/green
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B. PropertiesB. Properties
sour tastepH less than 7corrosiveelectrolytes turn litmus red react with metals to
form H2 gas
bitter tastepH greater than 7corrosiveelectrolytes turn litmus blueslippery feel
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C. UsesC. Uses
H3PO4 –phosphoric acid - soft drinks, fertilizer, detergents
H2SO4 – sulfuric acid - fertilizer, car batteries
HCl – hydrochloric acid - gastric juiceHC2H3O2 – acetic acid - vinegar
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C. UsesC. Uses
NaOH – sodium hydroxide -lye, drain and oven cleaner
Mg(OH)2 – magnesium hydroxide - laxative, antacid
NH3 –ammonia - cleaners, fertilizer
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Ch. 8Solutions, Acids, & Bases
Ch. 8Solutions, Acids, & Bases
V. Strength of Acids & Bases Strength vs. ConcentrationStrong vs. Weak pH
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A. Strength vs. ConcentrationA. Strength vs. Concentration
Strong and weak – tells how easy the acid or base dissociates in solution.
Concentration – The amount of acid or base in a solution.
It is possible to have a dilute concentration of a strong acid that would be less harmful than a concentrated weak acid.
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A. Strength of Acids & BasesA. Strength of Acids & Bases
The strength of an acid or base depends on how completely a compound separates into ions when dissolved in water.
Ions can carry an electric charge so a strong acid will carry more electricity than weak acid.
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B. Strong vs. WeakB. Strong vs. Weak
Strong Acid/Base• 100% ions in water• strong electrolyte• HCl, HNO3, NaOH, LiOH
Weak Acid/Base• few ions in water• weak electrolyte• HC2H3O2, NH3
- +
- +
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B. Strong AcidsB. Strong Acids
Acids that ionize almost completely in a solution are strong acids.
Ex: HCl, HNO3, and H2SO4 They have a very low pH
(0-1).
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B. Strong BasesB. Strong Bases
Bases that dissociate completely in a solution are strong bases.
Ex: NaOHThey have a very high pH (13-14)
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C. pH ScaleC. pH Scale
0
7INCREASING
ACIDITY NEUTRALINCREASING
BASICITY
14
pH (potential of Hydrogen)• a measure of the concentration of H+
ions in a solution • measured with a pH meter or an
indicator with a wide color range (0-14)
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C. pH ScaleC. pH Scale
pH of Common SubstancespH of Common Substances
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Which of the following "molecular" pictures best represents a concentrated solution of the weak acid HA?
ConcepTestConcepTest
A B
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Is the following statement TRUE or FALSE?• A strong acid has a lower pH than a
weak acid.• True- • But: Strong/weak refers to amount of
ionization whereas pH refers to concentration of H+.
ConcepTestConcepTest
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Ch. 8Solutions, Acids, & Bases
Ch. 8Solutions, Acids, & Bases
VI. Neutralization Neutralization Reaction
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A. Neutralization ReactionA. Neutralization Reaction
Chemical reaction between an acid and a base.
Products are a salt (ionic compound) and water.
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ACID + BASE SALT + WATER
HCl + NaOH NaCl + H2O
Neutralization does not always mean pH = 7.
=
A. Neutralization ReactionA. Neutralization Reaction
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KOH + HNO3 H2O + KNO3
Acid
Base
Salt
HNO3
KOH
KNO3
A. Neutralization ReactionA. Neutralization Reaction