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Acids and Bases
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Acids and Bases
What are acids and bases?
• Acids and Bases are one way of classifying matter through its properties.
Properties of Acids
–Taste sour–Change blue litmus paper to red color–pH less than 7–Reacts with carbonates and bicarbonates
forming CO2 gas –React with metals to form a salt
compound and H2 gas (pop!)–electrolyte
chemwiki
Reacts with carbonates and bicarbonates forming CO2 gas
MgCO3(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) + CO2(g)
carbonate acid salt water carbon dioxide
*Remember that you can test for CO2 using a burning splint. The CO2 gas will put out the flame of the burning splint.
React with metals to form a salt compound and hydrogen gas (pop!)
2 HCl + Mg MgCl2 + H2
acid metal salt hydrogen gas
*Remember that you can test for H2 using a burning splint. The H2 gas will make a popping sound and put out the flame of the burning splint.
Electrolytes - chemicals that dissociate when in water
Dissolve Dissociate
Name of acid Chemical formula Common use or location
Hydrochloric acid HCl Gastric juice
Sulfuric acid H2SO4 Car batteries
Nitric acid HNO3 fertilizer
Carbonic acid H2CO3 Soft drinks
Uric acid C5H4N4O3 urine
Ascorbic acid (Vitamin C) C6H8O6 fruit
Citric acid C6H8O7 Citrus fruit
Acetic acid HC2H3O2 vinegar
Tartaric acid C4H6O6 grapes
Properties of bases
–Taste bitter–Feel slippery–Change red litmus paper to blue
color–pH greater than 7–electrolyte
Neutral solutions
Substances that are neither acids nor bases
• do not change the color of red or blue litmus paper
• pH equals 7• nonelectrolytes
chemwiki
Arrhenius Definition of AcidsArrhenius acids - give (donate)
hydrogen ions (H+) in aqueous solution. *an H+ ion is a proton
HCl + H2O H3O+ + Cl-
Example:
What happened to the H of HCl?
Which substance is the acid: HCl or H2O?
How do you know?
Arrhenius bases – give (donate) hydroxide ions (OH) -1 in aqueous solution.
NaOH (aq) Na+ + (OH)-
Example:
What happened to NaOH when it was added to water?
Why is NaOH classified as an Arrhenius base?
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PracticeUsing the Arrhenius definition, classify the
following as an acid or a base in water1. HI
2. KOH
3. HNO3
4. Ca(OH)2
5. H2SO4
6. Mg(OH)2
Acid, in water HI H+ + I-
Acid, in water HNO3 H+ + NO3-
Base, in water KOH K+ + OH-
Base, in water Ca(OH)2 Ca+2 + 2OH-
Base, in water Mg(OH)2 Mg+2 + 2OH-
Acid, in water H2SO4 2H+ + SO4-2
Arrhenius definition of acids and bases is limited.
Brönsted-Lowry Definition of Acids and Bases
Acids donate a proton or H+ (proton donor)
Bases takes in a proton or H+ (proton acceptor)
NH3 is accepting an H+ so it is a B-L base.
Brönsted-Lowry Definition of Acids and Bases
• A conjugate base is the remainder of the original acid, after it donates its hydrogen ion
• A conjugate acid is the particle formed when the original base gains a hydrogen ion
For example:
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conjugate conjugate
Leftovers from acid
Base that has gained an H+
Practice: Brönsted-Lowry Acids and Bases
Identify the B-L acid (a), conjugate base (c.b.), B-L base (b), and conjugate acid (c.a.)
1. HCl + H2O ↔ H3O+ + Cl-
2. HNO2 + H2O ↔ H3O+ + NO2-
3. SO3-2 + H2O ↔ HSO3
- + OH-
Ans: acid + base ↔ c.a. + c.b
Ans: acid + base ↔ c.a. + c.b
Ans: base + acid ↔ c.a. + c.b
Review
In a B-L acid-base reaction:• What happens to an acid?
• What happens to the base?
• What is a conjugate base?
• What is a conjugate acid?
Lost the proton (H+)
gained the proton (H+)
Acid without the proton (H+)
Base with the proton (H+)
More Practice: Brönsted-Lowry Acids and Bases
Identify the acid, conjugate base (c.b.), base, and conjugate acid (c.a.)
1. HC2H3O2 + H2O ↔ H3O+ + C2H3O2-
2. CO32- + H2O ↔ HCO3
- + OH-
3. NH4+ + H2O ↔ NH3
+ H3O+
Ans: acid + base ↔ c.a. + c.b
Ans: base + acid ↔ c.a. + c.b
Ans: acid + base ↔ c.b. + c.a
The pH concept
Aci
dic
Alk
alin
e (
basi
c)
Neutral
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pH (8:53)
formula: pH = -log[H+] [H+] = concentration of H+ ions
Example 1: What is the pH of a solution with [H+] = 1 x 10-3 M?
formula: pH = -log[H+] where [H+] = concentration of H+ ions
Example 2: What is the pH of a solution with [H+] = 1 x 10-8 M?
The pH concept
1. [H+] = 0.01 M
2. H+] = 0.0001 M
3. [H+] = 10-7 M
4. [H+] = 0.015 M
5. [H+] = 3.2 x 10-10 M
6. [H+] = 6.5 x 10-4 M
7. [H+] = 4.5 x 10-8 M
pH = 2, acid
Practice: Find the pH of the following solutions and state whether the solution is an acid, base or neutral.
pH = 4, acid
pH = 1.8, acid
pH = 9.5, base
pH = 3.2, acid
pH = 7, neutralpH = 7.3, base
pH scale
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[H+][OH-]
14
0
• What is the difference in the dissociation of strong and weak acids?
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Strong Acids and Bases• Strong acids completely dissociate and release
[H+] ions. HCl H+ + Cl-
• Strong bases completely dissociate and release [OH-] ions.
NaOH Na+ + OH-
These are the ONLY strong acids:HCl, HBr, HI, HNO3, HClO4, H2SO4
Some strong bases – NaOH, KOH, LiOH
Particle diagrams
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strong acid – complete dissociation
weak acid – partial dissociation
Comparison between Solutions of Strong and Weak Acids• Two solutions are represented by the diagram below. Which
diagram illustrates a solution of a weak acid? How do you know?
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A B
H+ concentration of Strong and Weak Acids
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How is the pH related to the H+ ion concentration of weak and strong acids?
Concentrated vs. Dilute• Concentrated acids and bases have a
relatively large # of moles (of acid or base) per liter of solution.
• Dilute acids and bases have a relatively small # of moles (of acid or base) per liter of solution.
• 10.0 M HF is more concentrated than 2.0 M HF.
• 2.0 M KOH is more dilute than 10.0 M KOH. 34
Two acids, HCl and HC2H3O2 are both 0.10 M. Which of the two has a higher pH and why?
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H+ Concentration of Strong and Weak Acids
A B
Acid Base Concentration
Molarity- The number of moles of solute dissolved in 1.00 L of solution Molarity (M) = Moles of solute Liter of solution
Example: What is the molarity if 2.0 moles of hydrochloric acid are added to 5.0 L of solution?
M = 2.0 mol = 0.40 M
5.0 L
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Diluting Solutions
• Diluting Solutions: V1M1 = V2M2
• Example: What volume of 2.0 M H2SO4 would you need to prepare 100. mL of 0.40 M H2SO4?
V1 = x
M1 = 2.0M (x)(2.0) = (100)(0.40)
V2 = 100.ml x = 20 mL
M2 = 0.40 M
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Indicators• Chemicals that change color in the presence of
an acid or a base• Used to determine the pH of a solution• Examples: litmus paper (red and blue), pH
paper, phenolphthalein, red cabbage juice
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Indicators
Acid Vocabulary Binary acid – acid that contains only H and one other type of atom
Ex. HBr, H2S
Ternary acid – acid that contains H and a polyatomic ion
Ex. H2SO4
Monoprotic acid – acid that only has one H atomEx. HBr, HI
Polyprotic acid – acid that has more than one H atomEx. H2S, H3PO4
*a hydrogen ion, H+, is a proton
Anion Ending Acid Name
-ide hydro-(stem)-ic acid
-ate (stem)-ic acid
-ite (stem)-ous acid
Naming Acids (stop at 5:47)
No Oxygen
w/Oxygen
Examples: HCl – hydrochloric acid HClO3 – chloric acid
HClO2 – chlorous acid
binary
ternary
Naming Acids
h yd ro - p re fix-ic e n d ing
2 e le m e n ts
-a te e nd ingb e com es-ic e nd ing
-ite e nd ingb e com es
-o us e nd ing
n o h yd ro- p re fix
3 o r m o re e le m e n ts (w ith o xyg e n)
AC ID Ss ta rt w ith 'H '
binary
PracticeName the following
acids:1. HI
2. HF
3. H2SO4
4. H2SO3
5. H2CO2
Write the chemical formula:
6. Hydrobromic acid
7. Hydrosulfuric acid
8. Acetic acid
9. Phosphoric acid
10. Nitrous acid
Hydroiodic acid
Hydrofluoric acid
sulfuric acid
sulfurous acid
carbonic acid
H2S
HC2H3O2
H3PO4
HNO2
HBr
Symbol, ox #, criss-cross
Hydroxides (OH-)
NaOH sodium hydroxide
Mg(OH)2 magnesium hydroxide
Al(OH)3 aluminum hydroxide
Base Nomenclature
Ammonia - NH3 is a common base found in household glass cleaners.
Most bases are named the same as any other ionic compound, for example:
Writing formulas for bases
Just like all ionic compounds, write the symbol for each ion, its oxidation number, and then criss-cross to get the subscripts.
Example: potassium hydroxide
K+1 (OH)-1
KOH or K(OH)
Practice writing formulas for bases
1. Zinc hydroxide
2. Iron (II) hydroxide
3. Calcium hydroxide
4. Lithium hydroxide
Neutralization
• one type of double replacement reaction• Reactants are acid and base, products are
salt and water
• Acid + Base Salt + water
HCl + NaOH NaCl + H2O
47
Titration (6:52)
• A controlled acid-base neutralization reaction• The process of finding the concentration of an
unknown solution by using a certain volume of a known concentration solution.
49
• This solution is also called the analyte or titer
• Unknown concentration
known concentration
End point of a titration
• The point where neutralization is achieved• Occurs just before the indicator has changed
color• DETERMINED BY OBSERVATION, DURING THE
TITRATION EXPERIMENT
50
51
Equivalence Point
• the stoichiometric end point of a titration
• when moles of H+ from acid = moles of OH- from base
• DETERMINED FROM THE DATA COLLECTED IN THE TITRATION EXPERIMENT
Neutralization Problems-
(#H+)MAVA = MBVB(#OH-)
• #H+ = #H in chemical formula• MA = molarity of acid
• VA = volume of acid
• MB = molarity of base
• VB = volume of base• #OH- = #OH in chemical formula
53
Practice: Neutralization Problem
(#H+)MAVA = MBVB(#OH-)
When 45.0 mL of 3.00 M HBr is added to 80.0 mL of Ca(OH)2 What is the molarity of the Ca(OH)2 that was neutralized?
#H+ = MA =
VA =
MB =
VB =
#OH- =
54
Practice: Neutralization Problem(#H+)MAVA = MBVB(#OH-)
• In a titration experiment, if 65.0 mL of an HCl solution reacts with 47.2 mL of a 0.65-M NaOH solution, what is the concentration of the HCl solution?
#H+ = MA =
VA =
MB =
VB =
#OH- =
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Ion Stoichiometry : )
H2SO4 + 2NaOH Na2SO4 + 2H2O
240 grams of NaOH react with sulfuric acid. How many moles of H+ ions are consumed?