Acids & Bases chapter15 6 acids SulfuricH 2 SO 4 NitricHNO 3 HydrochloricHCl PhosphoricH 3 PO 4...
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Transcript of Acids & Bases chapter15 6 acids SulfuricH 2 SO 4 NitricHNO 3 HydrochloricHCl PhosphoricH 3 PO 4...
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Acids & Bases chapter15
6 acidsSulfuric H2SO4
Nitric HNO3
Hydrochloric HCl
Phosphoric H3PO4 …cola
Carbonic H2CO3
Acetic Acid HC2H3O2 …vinegar
What do you notice?
What makes an acid an acid?
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HCl + H20 H+ + Cl-
Acids … ionize themselves… break apart into their ions.
Remember water is very polar
H20 + HCl H30+ + Cl-
You may see…either….. H30+ or H+
These have names: hydronium ion, , hydrogen ion, , proton ion.
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BasesSodium Hydroxide NaOH
Magnesium Hydroxide Mg(OH)2
Aluminum Hydroxide Al(OH)3
Ammonia NH3
Sodium Hydrogen Carbonate NaHCO3
What do you notice?What makes a base a base? (OH) or the ability to make an (OH)
Base solutions are sometimes called ALKALINE SOLUTIONSBases dissociate ….. Break apart producing hydroxide
NaOH + H20 Na+ + OH-
NH3 + H20 NH4+ + OH-
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Strong vs. Weak p.460 & p. 469
Can tell 2 ways memorize them
arrows
HX + H20 H30+ + X- label
Strong acids: HCl, H2SO4, HNO3 ionize completely
Weak acids: H2CO3, HC2H3O2, H3PO4
Strong Base: group 1 or 2 metal hydroxidesWeak base: NH3 dissociates completely
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HF + H20 F- + H30+
H2SO4 + H20 HSO4 + H30+
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Strength of acids
depends on: H+ production
polarity of bonds
ionization
The greater the polarity of bond = greater strength
The greater the ionization = greater strength
Strong acids= HCl, HNO3, H2SO4
Weak Acid = H3PO4, H2CO3, HC2H3O2
Notice: strength of acid does not depend on number of hydrogens
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Strength of bases depends on: OH- production
polarity of bonds dissociation of hydroxide
The greater the polarity of bond = greater strengthThe greater the dissociation = greater strength
Base solutions are sometimes called alkaline solutions
Strong Bases: NaOH, KOH, Ca(OH)2, Ba(OH)2
Weak Base: NH3
Note: Alkali metals are stronger than alkaline earth….why?
Strong Acid/ Strong Base = Strong electrolyte……..why?
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pH Scale pH measures [concentration] of H30+ or OH-
pH ….. O – 14
0 3 7 10 14
Units of 10
4.6 pH is 10x stronger than 5.6pH
4.6 pH has 10x [H30] than 5.6 pH
Pure water is neutral…..pH 7
“self-ionization of water
Water produces ½ H+ and ½ OH-
[H+]
[OH-]
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20 minute lab
Red litmus paper turns blue in base
Blue litmus paper stays blue in base
Determine pH using the rainbow chart
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pH = [H30+] or [H+] pH = power of the Hydrogen
Calculating pH from concentrations
pH = -log [H3O+]
pOH = -log [OH-]
pH + pOH = 14 ws.17.24
Calculator
number exponentFind pH of a solution of hydronium concentration of [3 x 10-5]?
pH = -log [3 x 10-5]
3 -5 =
(-) log
Yellow
2nd EE
(-) log Yellow
2ndEE
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[1 x 10-3 M] HCl
[1 x 10-5 M] HNO3
[0.001 M ] HCl
[0.09 M ] HBr
[1.34 x 10-4M] HCl
[7.98 x 10-2 M] HNO3
Calculate pH
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pH + pOH = 14
ph pOH
2 =14
8 =14
6 =14
13 =14
4 =14
7 =14
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Find the pH of a solution of Hydroxide concentration of [3 x 10-5]
(-)log 3 -5 =
BUT it is hydroxide so…..it is the pOH….so subtract it from 14.
Yellow2nd EE
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Calculate pH
[1 x 10-4 M] NaOH
[1 x 10-3 M] KOH
[1 x 10-6 M] LiOH
[3.2 x 10-2 M] Mg(OH)2
[0.08 M] Ca(OH)2
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Calculate pH
Hydronium concentration of [.001M]
Hydroxide concentration of [.001 M]
H+ concentration of [ 1 x 10-5 M]
OH concentration of [1 x 10-5 M]
Ws.14.1
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Ws.17.26
1. A popular soda pop drink is measured to have a hydronium concentration of 1.34 x 10-4. What is the pH and is it acidic, base or neutral?
2. The molarity of hydroxides in a pancake syrup is
1.0 x 10-8M. Pancake syrup by law must have a pH lower than 7 to be sold in the open market. Calculate the pH and identify if acid, base, neutral. Can it be sold?
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3. You work for Colgate Toothpaste. You need to make stannic fluoride solution of hydroxide molarity [2.44 x 10-4]. What is the ph? Is it acid, base, neutral?
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If pH is 7.40 what is the [hydronium] or the molarity?
“If given pH…find antilog”negative # = [hydronium conc.]
-7.40 = [.00000004] or [4 x 10-
8]
“secret….hydronium concentration is the molarity ”
BUT::::: if they also ask for hydroxide concentration one must use the equilibrium
constant for water:::::::::
Equilibrium Constant for water is
Kw = [H+] [OH-]
Kw = [1 x 10-7] [1 x 10-7]
Kw = 1 x 10-14
Yellow2nd log
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1. The pH of an orange is 4.0pH. What are the [H30] and [OH] in this fruit? What is its Molarity?
2. Lemons have a pH 3.15. What are the hydronium and the hydroxide concentrations? What is its molarity?
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3. What is the molarity of pH is 12.9 for a Calcium hydroxide solution?
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Remember: 3 formulas: pH=-log[H3O]
pOH=-log[OH]
pH + pOH = 14
Remember: [H3O] is hydronium concentration
or…..molarity for an Acid
or…..H+ proton concentration
Remember: [OH] is hydroxide concentration
or molarity for a base
Remember: if given pH use antilog to calculate [H3O] [OH]
put pH in as negative number
Remember: Kw = [H3O] [OH] = 1x10-14
Kw = [1x10-7] [1x 10-7]
Kw = 1x10-14
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Neutralization Reaction
p.474
Strong acid + Strong Base salt + water Look on reference table: 4c
HCl + H20 H+ + Cl-
NaOH + H20 OH- + Na+
Put them together
HCl + NaOH NaCl + H2O
Salt: a compound composed of
a cation+ from an base
and an anion- from a acid.
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Stomach Ache CaCO3 ….tums
HCl + Mg(OH)2 …milk of magnesia
NaCO3 …. Rolaids
Neutralize …………..salt + H20
HCl + CaCO3 CaCl + CO2 + H20
HCl + Mg(OH)2 MgCl + H20
HCl + NaCO3 NaCl + CO2 + H2O
Which will make you burp?
Tums and Rolaids… that is why old people prefer milk of magnesia
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Titration: the controlled addition and measurement of
the amount of a solution of known concentration
required to react completely with a
measured amount of a solution of unknown concentration p.497
Equivalence point: The point at which the two solutions used in a titration are present in chemically equivalent amounts p. 498
Indicator: an organic substance that changes color whether in
acid or base…….Phenolphthalein
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Calculating Titration Problems ws 19-3
On your reference sheet nM1V1 = nM2V2
n = # of (H) or (OH) in the molecule
Ws 19-3
1. A volume of 30mL of 0.25M HCl neutralizes a 50mL sample of KOH solution. What is the concentration of KOH? Create new copyrght
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6. A volume of 50mL of 0.30M HCl neutralizes a 60mL sample Ca(OH)2 solution. What is the concentration of Ca(OH)2?
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2 acid / base theories
Arrhenius acids & bases p. 459
Arrhenius acid = a chemical that increases H+ ions.
Arrhenius base = a chemical that increases OH- ions
“limited because must be in water….not everything in water..p.464”
Bronsted-Lowery acids & bases p.464
Bronsted-Lowery acid = a chemical that is a proton donor (H+)
Bronsted-Lowery base = a chemical that is a proton acceptor (H+)
“ notice no mention of OH”
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Conjugate acid/ base the species that forms in result of gaining or losing a proton (H+)
acid base
Arrhenius H+donor OH- producer
Bronsted-Lowery H+donor H+ acceptor
Overhead worksheet 15.2,3,, 15.4
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Overhead 88 , 87 quick lab
Remember Equilibrium Keq = [conc] [conc] ….(g) and (aq) but not liquids nor solids
Equilibrium Constant for water is Kw = [H+] [OH-]Kw = [1 x 10-7] [1 x 10-7]Kw = 1 x 10-14
On chemistry table….constant like.. pie = 3.14 r = .0821
We can use this constant (Kw = 1 x 10-14) to calculate pH of a solution
Ws problems 17.
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