acids and bases. distinguish between strong and weak acids and bases. include: electrolytes and...
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ACIDS AND BASES
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• Distinguish between strong and weak acids and bases.
Include: electrolytes and non-electrolytes
Additional KEY Termsconcentrated dilutemonoprotic diprotic
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For a solution to conduct an electric current, charged particles or ions must be present in the solution.
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Electrolytes conduct an electric current when in aqueous solution or when in a molten state.
• All ionic compounds act as electrolytes (as do highly polar molecular compounds)
• Most molecular compounds are non-electrolytes.
NaCl(s) Na+(aq) + Cl–
(aq)
C11H22O11(s) C11H22O11(aq)
non-electrolytes
electrolytes
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• Only hydrogen in a very polar bond is ionizable
(H must be bonded to a very electronegative element)
Cl HH
O
H
H H
H
H
C C
+ +
δ+δ-
δ+
δ-++-
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Electrolytes are classified as strong OR weak Strong: produces many ions in solution.
• dissociates 100% in water (NaCl)
Weak: partially dissociates (<<100%) in solution.• usually weak polar molecules (vinegar)
A (s) B+(aq) + C–
(aq)
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ionic polar
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ionic polar
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• easily donate protons • completely dissociate or ionize
Strong acids are strong electrolytes:
HCl (s) H+(aq) + Cl-
(aq)water
Indicate complete dissociation using single arrow
[HCl]i = [H+]e = [Cl-]e
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Name of Strong Acid Formula
perchloric acid HClO4
hydrochloric acid HCl
sulfuric acid H2SO4
nitric acid HNO3
hydroiodic acid HI
hydrobromic acid HBr
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Weak acids are weak electrolytes:
HC2H3O2 + H2O H3O+ + C2H3O2-
acetic acid
The reverse reaction is favored over the forward one. The ions formed react very easily to reform the acid and the water.
• incompletely ionize• equilibrium reached between ions and acid
Indicate equilibrium using reversible arrow
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Name of Weak Acid Formula
carbonic acid H2CO3
hydrofluoric acid HF
acetic acid HC2H3O2
phosphoric acid H3PO4
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Strong bases are strong electrolytes:
NaOH (s) Na+(aq) + OH-
(aq)
water
Indicate complete dissociation using single arrow.
[NaOH]i = [Na+]e = [OH-]e
• easily accept protons • completely dissociate into OH-, or oxide, (O-2)
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Basically, any hydroxide and Alkali (1A) or Alkali-Earth Metal (2A) would be a strong base because of 100%
dissociation
Name of Base Formula
barium hydroxide Ba(OH)2
strontium hydroxide Sr(OH)2
lithium hydroxide LiOH
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NH3(g) + H2O (l) NH4+
(aq) + OH-(aq)
Does not produce hydroxide ions readily. The reverse reaction is favored.
Weak bases are weak electrolytes: • incompletely ionize• equilibrium reached between ions and base
Indicate equilibrium using reversible arrow
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Common weak bases are usually conjugate bases of strong acids.
In fact: The stronger the A/B, the weaker its conjugate.
The weaker the A/B, the stronger its conjugate.
HA + H2Obaseacid
H3O+ + A-
Con. baseCon. acid
weak
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Acid Strength Table
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Any acid that contains only one ionizable hydrogen is called monoprotic.
Contains two ionizable hydrogens - diprotic
Three - triprotic
Cl H
H
O
O
HO
O
s
H
O
O
HO
O
sp
H
Sulfuric acid
Phosphoric acid
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Acid Strength Table
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The equilibrium reaction favours the strongest acid.
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HCO3– + PO4
3–
Which direction is favoured and why?
HCO3– + PO4
3– CO32– + HPO4
2–
acid1 base2 C base1 C acid2
fwd reaction is favouredHCO3
– is the stronger acid
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THOUGHTS:
• Don't confuse weak and strong with dilute and concentrated
• Weak and strong indicates the proportion of an acid or base which ionized
• Dilute and concentrated refer only to the volume of acid and base dissolved in a total solution volume
• It is possible to have a concentrated weak acid/base or dilute strong acid/base
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HA H+ + A-
HA + H2O H3O+ + A-
Strong Acid
Weak Acid
HA + H2O + A-
H+ H2O
H3O+
9.0 M 1.0 M 1.0 M[E]+x+ x- x[C]
0010 M[I]
0 2.5 M 2.5 M[E]
+x+ x- x[C]002.5 M[I]
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CAN YOU / HAVE YOU?
• Distinguish between strong and weak acids and bases.
Include: electrolytes and non-electrolytes
Additional KEY Termsconcentrated dilutemonoprotic diprotic