acids, bases, and salts. electrolytes an electrolyte is a substance that dissociates when dissolved...
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Acids, Bases, and Salts
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Electrolytes
• An electrolyte is a substance that dissociates when dissolved in water. (Nonelectrolytes do not dissociate.)
• These compounds conduct electricity based on this dissociation.
• To dissociate means to separate into ions in solution.
• Acids, bases, and salts (ionic compounds) are all electrolytes.
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Strong vs. Weak Electrolytes
• Strong electrolytes fully dissociate in water. (ex. Ionic compounds, strong acids, strong bases)
• Weak electrolytes only partly dissociate in water. (ex. Weak acids and weak bases)
• Nonelectrolytes do not dissociate in water. (nonpolar covalent compounds)
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Write an equation for the dissociation of magnesium nitrate
in water.
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Write an equation for the dissociation of the weak acid, HF, in
water.
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Acids and Bases
Acids, bases, and salts make up compounds known as electrolytes.
Arrhenius acids – substances that ionize in water to produce the hydrogen ion, H+.
Arrhenius bases – substances that ionize in water to produce the hydroxide ion, OH-.
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HCl(g) → H+(aq) + Cl-(aq)
NaOH(cr) → Na+(aq) + OH-(aq)
Dissociation – already formed ions separate
Ionization – neutral molecules react with water to form charged ions
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Strength of Acids and Bases
Strength of acids and bases depends on how completely they ionize in water- the strongest acids and bases fully ionize in water while weak acids and bases only ionize slightly
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Strong acids (Know these)– HCl, HBr, HI are all strong, while all other binary acids are weakAs a rule, all acids with at least two more oxygens than hydrogens are strong (H2SO4, HNO3,HClO4)
Strong bases – Hydroxides of the Groups I and II elements except for Be are all strong.
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Acid Nomenclature
• In general, names of acids will begin with hydrogen.
• If the anion does not contain oxygen, the acid begins with hydro and ends in –ic
• HCl = hydrochloric acid• HBr = • HCN =
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Acids containing oxygen
• If the acid contains oxygen, the acid does not have hydro at the start and either ends in ic or ous.
• If the anion ends in –ate use –ic• HNO3 = nitric acid• If the anion ends in –ite use –ous• H2SO3 = sulfurous acid
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What is the formula for hydroiodic acid?
HI
HI2
H2I
HIO
3
0% 0%0%0%
1. HI2. HI2
3. H2I
4. HIO3
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What is the formula for hydrocyanic acid?
H3N
HN
HCN
HSC
N
0% 0%0%0%
1. H3N
2. HN3. HCN4. HSCN
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What is the formula for phosphoric acid?
H3PO3
H3PO4
HPO4
HPO3
0% 0%0%0%
1. H3PO3
2. H3PO4
3. HPO4
4. HPO3
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What is the formula for sulfurous acid?
H2SO
3
H2SO
4 H
2S H
S2
0% 0%0%0%
1. H2SO3
2. H2SO4
3. H2S
4. HS2
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What is the name of HNO2?
Hyd
ronitr
ic ac..
.
Hyd
ronitr
ous a...
Nitr
ous acid
Nitr
ic acid
0% 0%0%0%
1. Hydronitric acid2. Hydronitrous acid3. Nitrous acid4. Nitric acid
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What is the name of HCl?
Hyd
roch
loric a...
Hyd
roch
lorous .
..
Chlorous a
cid
Chloric acid
0% 0%0%0%
1. Hydrochloric acid2. Hydrochlorous acid3. Chlorous acid4. Chloric acid
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What is the name of HClO4?
Hyd
roch
loric a...
Chlorous a
cid
Chloric acid
Perchloric
aci...
0% 0%0%0%
1. Hydrochloric acid2. Chlorous acid3. Chloric acid4. Perchloric acid
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Relative Strength of Acids and Bases
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Conjugate Acids and Bases
• The strength of conjugate acids and bases are inversely proportional.
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Kw
• Kw for water is based on the equation:
• 2H2O (l) -> OH- (aq) + H3O+ (aq)
• Kw = [OH-][H3O+] = 10-14
• Therefore, if you know either hydroxide or hydronium concentrations, you can solve for the other.
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pH scale
pH is the measure of the concentration of hydronium ion in a water solution
pH = -log[H30+]
Scale goes from 0 to 14.0 to 7 is acidic, 7 is neutral, 7 to 14 is basic
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pH – log based
• Every increase of 1 on the pH scale changes the concentration by a power of 10.
• How much stronger is a substance with a pH of 4 vs a pH of 6?
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pOH scale
pOH is the measure of the concentration of hydroxide ion in a water solution
pOH = -log[0H-]
Also, pH + pOH =14
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Neutralization Reaction
A neutralization reaction occurs when and acid and a base react to form water and a salt.
Acid + Base -> Water + Salt
***When the base has a CO32- ion, CO2 is also
produced.
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Titrations
• Titrations are a quantitative lab technique that helps identify an unknown concentration of acid or base by titrating it against a titrant, or known acid or base concentration.
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Titration Method
• Add an accurately measured volume of unknown acid (or base) to an Erlenmeyer flask
• Put 2-3 drops of phenolphthalein indicator to the unknown solution.
• Start adding the titrant and continue until the solution turns pink and stays pink.
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Titration Tips
• Record the unknown’s volume by subtracting the ending vs. starting amount from buret (use the right amount of sig figs).
• You can add the titrant quickly at first but once it starts turning pink, swirl the flask and start adding more slowly. Swirl after each drop towards the equivalence point.