Drill: Calculate the pH of: [H + ] = 3.0 x 10 -5 M [HI] = 2.0 x 10 -4 M
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Transcript of Drill: Calculate the pH of: [H + ] = 3.0 x 10 -5 M [HI] = 2.0 x 10 -4 M
![Page 1: Drill: Calculate the pH of: [H + ] = 3.0 x 10 -5 M [HI] = 2.0 x 10 -4 M](https://reader030.fdocuments.in/reader030/viewer/2022033106/5681322c550346895d9890cd/html5/thumbnails/1.jpg)
Drill: Calculate the pH of:
[H+] = 3.0 x 10-5 M [HI] = 2.0 x 10-4 M
![Page 2: Drill: Calculate the pH of: [H + ] = 3.0 x 10 -5 M [HI] = 2.0 x 10 -4 M](https://reader030.fdocuments.in/reader030/viewer/2022033106/5681322c550346895d9890cd/html5/thumbnails/2.jpg)
Acid-Base Equilibria
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Ionization of WaterH2O(l)
H+(aq)+ OH-
(aq)
2 H2O(l)
H3O+(aq) + OH-
(aq)
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Water Ionization Constant
Kw = [H+][OH-] or
Kw = [H3O+][OH-]
Kw = 1.00 x 10-14
Memorize this
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Kw CalculationsIn pure water [H+] = [OH-]
Kw = [H+][OH-]
= 1.0 x 10-14
Let [H+] = x = [OH-]
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Kw CalculationsKw = [H+][OH-] = x2
Kw = x2 =1.0 x 10-14
Thus x = 1.0 x 10-7 M
[H+] = x = 1.0 x 10-7 M
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pH of Pure Water[H+] = 1.0 x 10-7 M
pH = -log[H+]
pH = -log[1.0 x 10-7]
pH = 7 -log 1
Thus pH = 7.00
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Calculate the pH of
3.3 x 10-8 M HI
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Calculate [H+],[OH-], pH, &
pOH of 0.020 M HCl
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Calculate [H+] of 0.050 M H2SO4
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Weak Acid Ionization
HA(aq) H+(aq) + A-
(aq)
HA(aq) + H2O(l)
H3O+(aq) + A-
(aq)
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Acid Dissociation Constant
HA(aq) H+(aq) + A-
(aq)
[H+][A-]
[HA]Ka =
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Weak Base Ionization
NH3(aq) + H2O(l)
NH4+
(aq) + OH-(aq)
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Base Dissociation Constant
NH3(aq) + H2O(l)
NH4+
(aq) + OH-(aq)
[NH4+][OH-]
[NH3]Kb =
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Calculate [H+], [OH-], pH, & pOH of 2.0 M
HC2H3O2 (HAc)Ka = 1.8 x 10-5
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Drill: Calculate [H+],[OH-], pH, &
pOH of 0.025 M KOH
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Acid-Base Equilibria Problems
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Calculate [H+], [OH-], pH, &
pOH of0.50 M NH3
Kb = 1.8 x 10-5
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Calculate [H+],[OH-], pH, & pOH of 0.010 M HC7H5O2 (HBz)
Ka = 6.4 x 10-5
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Calculate the Ka of 0.10 M Hquack
when it ionized 5.0 % in an aqueous
solution.
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The pH of a 0.79 M solution of Hnut is 3.10.
Calculate its Ka
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Drill: Calculate [H+] & pH of 0.50 M NaOH
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Drill: Calculate [H+] & pH of
2.0 M C6H5NH2
Kb = 3.2 x 10-5
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Calculate the pH of a solution of
0.00050 M HBS : Ka = 5.0 x 10-12
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PolyproticAcid
Equilibria
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Calculate [H2CO3], [HCO3
-], [CO3-2], [H+],
[OH-], & pH of 0.44 M H2CO3 Ka1 = 4.4 x 10-7
Ka2 = 4.7 x 10-11
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Calculate [H2SeO3], [HSeO3
-1], [SeO3-2],
[H+],[OH-], & pH of 0.27 M H2SeO3 Ka1 = 2.7 x 10-7
Ka2 = 5.4 x 10-11
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Calculate [H3A],[H2A-], [HA-2],[A-3],[H+], &pH of 0.30 M H3A
Ka1 = 3.0 x 10-7
Ka2 = 5.0 x 10-11
Ka3 = 4.0 x 10-15
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Calculate the pH of
0.025 M HF:Ka = 6.4 x 10-4
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Drill: Calculatethe pH of
0.025 M QOH:Kb = 2.0 x 10-4
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You have 10 identical coins with 1 coin having a slight mass difference. Determine the odd coin with only 3 uses of an
equal arm balance.
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Drill: Calculate the pH of
0.25 M HAz Ka = 2.5 x 10-3
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Drill: Calculate the pH of
0.25 M HAz Ka = 2.5 x 10-3
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Calculate the pH of
0.10 M HClO Ka = 2.5 x 10-8
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Calculatethe pH of
0.025 M QOH:Kb = 2.0 x 10-4
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Drill: Calculate the pH of 0.020
M QOH.Kb = 3.2 x 10-7
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TestReview
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Arrhenius Bronsted-Lowry
Lewis
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Be able to name:•Acids
•Bases
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Be able to describe & Identify:
•Strong Acids
•Strong Bases
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Show the ionization of
HClin solution
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Show the ionization of
NH3
in solution
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Calculate the [H+], [OH-], pH,
& pOHof 0.1 M HNO3
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Calculate the [H+], [OH-], pH,
& pOHof 0.02 M NaOH
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Calculate the [H+], [OH-], pH,
& pOH of 2.0 M NH3
Kb = 1.8 x 10-5
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Calculate the pH, & pOH of
0.10 M HNO2 Ka = 6.0 x 10-4
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Calculate the volume of 0.30 M Ba(OH)2 required to titrate
50.00 mL of 0.40 M H3PO4 to its
equivalence point.
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Calculate [H2A], [HA-], [A-2], [H+], & pH of 0.20 M H2A
Ka1 = 2.0 x 10-7
Ka2 = 5.0 x 10-11
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Calculate the pH of a solution of 0.20 M QNH2.Kb = 2.0 x 10-3
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Drill: 831 mL NH3 was bubbled through 2.0 L of water at 27.0oC under 150 kPa pressure. 80.0 % of
the ammonia dissolves in the water. Calculate the pH
of the final solution.