1. take out hw and stamp sheet #’s 20-22,24,32a,34a,35,36 #’s 31a,33a,37,39,40, 48-50,56,58ab...
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![Page 1: 1. Take out HW and Stamp Sheet #’s 20-22,24,32a,34a,35,36 #’s 31a,33a,37,39,40, 48-50,56,58ab 2. Solve this problem: What is the pH of a solution with](https://reader036.vdocuments.net/reader036/viewer/2022062801/56649e215503460f94b0d192/html5/thumbnails/1.jpg)
1. Take out HW and Stamp Sheet #’s 20-22,24,32a,34a,35,36#’s 31a,33a,37,39,40, 48-50,56,58ab
2. Solve this problem: What is the pH of a solution with a pOH of 11.09?
3. HW = pH problem set due Mon & study for quiz
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14 1 x 10-14 1 x 10-0 0 13 1 x 10-13 1 x 10-1 1 12 1 x 10-12 1 x 10-2 2 11 1 x 10-11 1 x 10-3 3 10 1 x 10-10 1 x 10-4 4 9 1 x 10-9 1 x 10-5 5 8 1 x 10-8 1 x 10-6 6
6 1 x 10-6 1 x 10-8 8 5 1 x 10-5 1 x 10-9 9 4 1 x 10-4 1 x 10-10 10 3 1 x 10-3 1 x 10-11 11 2 1 x 10-2 1 x 10-12 12 1 1 x 10-1 1 x 10-13 13 0 1 x 100 1 x 10-14 14
NaOH, 0.1 MHousehold bleachHousehold ammonia
Lime waterMilk of magnesia
Borax
Baking sodaEgg white, seawaterHuman blood, tearsMilkSalivaRain
Black coffeeBananaTomatoesWineCola, vinegarLemon juice
Gastric juice
Mor
e ba
sic
Mor
e ac
idic
pH [H1+] [OH1-] pOH
7 1 x 10-7 1 x 10-7 7
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pH
pOH
[H3O+]
[OH-]
pH + pOH = 14
pH = -log[H3O+]
[H3O+] = 10-pH
pOH = -log[OH-]
[OH-] = 10-pOH
Kw = [H3O+] [OH-] = 1 x10-14
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pH + pOH = 14pH + 11.09 = 14
Solution is acidic
pH = 14 – 11.09 = 2.91
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Solution is basic
Kw = [H3O+] [OH-] = 1.0 x10-14
1.0 x10-14 = [3.3 x 10-10] [OH-]
[OH-] = 3.0 x 10-5 M
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pH
pOH
[H3O+]
[OH-]
pH + pOH = 14
pH = -log[H3O+]
[H3O+] = 10-pH
pOH = -log[OH-]
[OH-] = 10-pOH
Kw = [H3O+] [OH-] = 1 x10-14
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OH-
H3O+OH-
OH-H3O+
H3O+
[H3O+] = [OH-] [H3O+] > [OH-] [H3O+] < [OH-] acidic
solutionneutralsolution
basicsolution
co
nc
en
trat
ion
(m
ole
s/L
)
10-14
10-7
10-1
Timberlake, Chemistry 7th Edition, page 332
pH = 3
pH = 7
pH = 11
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6 5 .
7
3 4 1 2
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0.120 M H2SO4 2 mol H3O+
1 mol H2SO4
X =0.240 M H3O+
pH = - log [H3O+] = -log [0.240M H3O+]
pH = 0.620
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pH
pOH
[H3O+]
[OH-]
pH + pOH = 14
pH = -log[H3O+]
[H3O+] = 10-pH
pOH = -log[OH-]
[OH-] = 10-pOH
Kw = [H3O+] [OH-] = 1 x10-14
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pH = - log [H3O+]
4.60 = -log [H3O+]
[H3O+] = 2.51 x 10-5 M2nd log -4.6
You can check your answer by working backwards.
pH = - log [2.51x10-5 M]
pH = 4.60
10- 4.60
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pH
pOH
[H3O+]
[OH-]
pH + pOH = 14
pH = -log[H3O+]
[H3O+] = 10-pH
pOH = -log[OH-]
[OH-] = 10-pOH
Kw = [H3O+] [OH-] = 1 x10-14
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DefinitionDefinition◦Analytical method in which a standard solution is used to determine the concentration of an unknown solution.
standard solution
unknown solutionCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Buret
stopcock
Erlenmeyer flask
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Titrant◦The substance added to the analyte in a titration (a standard solution)
Analyte◦The substance being analyzed
Equivalence point◦The point in a titration at which the quantity of titrant is exactly sufficient for stoichiometric reaction with the analyte.
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Titrant
Analyte
If the concentration of the titrant is known, then the unknown concentration of the analyte can be determined.
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Quantitative analysis — used to determine the amounts or concentrations of substances present in a sample by using a combination of chemical reactions and stoichiometric calculations
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The “perfect pink” for a titration with phenolphthalein
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Indicator - changes color to indicate pH change
Volume base added
Example… phenolphthalein is colorless in acid and pink in basic solution
pH
Endpoint =7
pink
point at which exactly enough reactant has been added for the solution to be neutralized and no more
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◦Point at which equal amounts of H3O+ and OH- have been added.
◦Determined by… indicator color change dramatic change in pH
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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moles H3O+ = moles OH-
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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25.5 mL of 1.3M KOH are required to neutralize 50.0 mL of HCl. Find the molarity of HCl.
Acid (H3O+)
M = ?V = 50.0 mL
Base (OH-)
M = 1.3MV = 25.5 mL MA = 0.66M HCl
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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equivalence point
14.0
12.0
10.0
8.0
6.0
4.0
2.0
0.00.0 10.0 20.0 30.0 40.0
pH
Volume of 0.100Volume of 0.100 M M NaOH added NaOH added(mL)
Titration of an Acid With an Base
0.00 1.0010.00 1.3720.00 1.9522.00 2.1924.00 2.7025.00 7.0026.00 11.3028.00 11.7530.00 11.9640.00 12.3650.00 12.52
NaOH added (mL) pH
Titration Data
Solutionof NaOHSolutionof NaOH
Solutionof HCl H+
H+ H+
H+
Cl-
Cl-
Cl-
Cl-
Na+
Na+
Na+
Na+
OH-
OH-OH-
OH-
25 mL
phenolphthalein - colorless
phenolphthalein - pink
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• ArrheniusArrhenius - In aqueous solution… - In aqueous solution…
HCl(aq) H+(aq)+ Cl-(aq)
AcidsAcids increase hydrogen ion concentration [H+]
H
HH H H
H
ClClO O
–+
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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A Brønsted-Lowry acid is a proton donorA Brønsted-Lowry base is a proton acceptor
acidconjugate
basebase conjugate
acid
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From the Latin word conjugare, meaning “to join together.”
Reactions between acids and bases always yield their conjugate bases and acids.
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HNO3, HCl, H2SO4 and HClO4 are among the only known strong acids.
Strong and Weak Strong and Weak Acids/BasesAcids/Bases
The strength of an acid (or base) is determined by the amount of IONIZATION.
The strength of an acid (or base) is determined by the amount of IONIZATION.
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Weak acids are much less than 100% ionized in water.
One of the best known is acetic acid = CH3CO2H
Strong and Weak Strong and Weak Acids/BasesAcids/Bases
Strong and Weak Strong and Weak Acids/BasesAcids/Bases
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Strong Base: 100% dissociated in water.
NaOH (aq) ---> Na+ (aq) + OH- (aq)
Strong and Weak Strong and Weak Acids/BasesAcids/Bases
Other common strong Other common strong bases include KOH and bases include KOH and Ca(OH)Ca(OH)22..
CaO (lime) + HCaO (lime) + H22O -->O -->
Ca(OH)Ca(OH)22 (slaked lime) (slaked lime)CaOCaO
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Weak base: less than 100% ionized in water
One of the best known weak bases is
ammoniaNH3 (aq) + H2O (l) NH4
+ (aq) + OH- (aq)
Strong and Weak Strong and Weak Acids/BasesAcids/Bases
Strong and Weak Strong and Weak Acids/BasesAcids/Bases
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The more polar the H-X bond and/or the weaker the H-X bond, the more acidic the compound.
Acidity increases from left to right across a row and from top to bottom down a group.
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H2O can function as both an ACID and a
BASE.
Equilibrium constant for water = KEquilibrium constant for water = Kww
KKww = [H = [H33OO++] [OH] [OH--] = 1.00 x 10] = 1.00 x 10-14-14 at 25 at 25 ooCC
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Timberlake, Chemistry 7th Edition, page 335
1.0 MHCl0
gastricjuice1.6
vinegar2.8
carbonated beverage3.0
orange3.5
apple juice3.8
tomato4.2
lemonjuice2.2 coffee
5.0
bread5.5
soil5.5
potato5.8
urine6.0
milk6.4
water (pure)7.0
drinking water7.2
blood7.4
detergents8.0 - 9.0
bile8.0
seawater8.5
milk of magnesia10.5
ammonia11.0
bleach12.0
1.0 MNaOH(lye)14.0
8 9 10 11 12 14133 4 5 621 70
acidic neutral basic[H+] = [OH-]