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ACIDS AND BASESUnit VII
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I ELECTROLYTES
An electrolyte is a compound, that when dissolved in water, conducts electricity How?
Ions (charges) produced are free to move Movement of charge is conductivity
Examples Acids Bases “Salts”
Soluble Ionic compounds
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II PROPERTIES
Acids Good conductors Dissolve metals
Table J--Metals above “H2” dissolve in acid
Taste sour Turns litmus paper red Turns phenolphthalein clear
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II PROPERTIES
Bases Good conductors Dissolve fats
Feels slippery Taste bitter Turns litmus paper blue Turns phenolphthalein pink
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III DEFINITIONS
A. Arrhenius Acids
An Arrhenius acid contains H+ ions When dissolved in water these H+ ions
combine to form hydronium ion (H3O+) Examples: HCl H2SO4 HC2H3O2
Bases An Arrhenius base contains OH- ions
(hydroxide ion) bonded to NH4+ or a metal
Examples: NaOH Ca(OH)2
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III DEFINITIONSB. Brönsted-Lowry
Acids A Brönsted-Lowry acid loses or donates
protons to its conjugate (substance that differs by an H+) HCl + NH3 → Cl - + NH4
+
HCl and Cl- are conjugate pairs; HCl is the acid and Cl - is its conjugate base
Bases A Brönsted-Lowry base gains or accepts protons
from its conjugate HCl + NH3 → Cl - + NH4
+
NH3 and NH4+ are conjugate pairs; NH3 is
the base and NH4+ is its conjugate acid
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IV NOMENCLATURE
A. Naming Compounds Binary Acids
A binary acid contains hydrogen and a nonmetal To name a binary acid
Use “hydro-” Add nonmetal root word End with “ic acid”
Ex. HCl Hydrochloric acid
Ex. H2O
Hydroxic acid
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IV NOMENCLATURE Ternary Acids
A ternary acid contains hydrogen and a polyatomic ion To name a ternary acid
Determine the polyatomic that is present using Reference Table E
If the polyatomic ion ends in “ate” change the ending to “ic”
If the polyatomic ion ends in “ite” change the ending to “ous”
Ex. HClO3 Chlorate becomes Chloric acid (no hydro
is used)
Ex. HNO2 Nitrite becomes Nitrous acid
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IV NOMENCLATURE
Bases To name a base, name as you would any
compound Write the first element Write the polyatomic Add a Roman numeral if needed
Ex. NaOH Sodium hydroxide
Ex. Cu(OH) 2 Copper II hydroxide
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IV NOMENCLATURE
B. Writing Formulas- Acids
• If binary • Write H+ and the other element present• Assign charges and criss-cross
Ex. Hydrochloric acid
H+1 Cl-1
HCl
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IV NOMENCLATURE
• If ternary • Identify the polyatomic present using
ending• Write H+ and the polyatomic ion• Assign charges and criss-cross
• Ex. Chloric acid• chloric comes from chlorate
ClO3-1
• H+1 ClO3-1
• HClO3
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V REACTIONS
A Neutralization Mixing of acid and base
HCl + NaOH → Makes salt and water
Break (ionize) the acid and base H+1 Cl-1 Na +1 OH-1
Join H to OH (H2O) Join metal to nonmetal (assign charges and
crisscross)
HCl + NaOH → H2O + NaCl
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Lab technique for neutralization is called Titration Occurs when moles of acid equals moles of
base For 1:1 acid–base reactions
Moles acid = Moles base MAVA = MBVB
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EXAMPLES OF TITRATION PROBLEMS Given the balanced equation:
HCl + NaOH → H2O + NaCl How many milliliters of 3.0M NaOH are needed to
neutralize 20 milliliters of 2.5M HCl? MB= 3.0M NaOH MA= 2.5M HCl VA= 20 mLs HCl
Ratio is 1:1 so MAVA = MBVB can be used 2.5M x 20 mLs = 3.0M x VB
50 = 3VB
VB=16.7 mLs NaOH
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EXAMPLES OF TITRATION PROBLEMSGiven the balanced equation:
H2SO4 + 2 NaOH → 2 H2O + Na2SO4
How many milliliters of 1.2 M NaOH are needed to neutralize 23 milliliters of 1.9 M H2SO4?
MB= 1.2 M NaOH
MA= 1.9 M H2SO4
VA= 23 mLs H2SO4
Ratio is NOT 1:1 so MAVA = MBVB CANNOT be used23mL H2SO4 x 1L x 1.9 mole H2SO4 x 2 mole NaOH x 1L x 1000
ml
1000 mL 1 L 1 mole H2SO4 1.2 mole NaOH 1L
VB= 72.8 mLs NaOH
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IV REACTIONS
B Hydrolysis Mixing of salt and water
Makes parent acid and base of the salt
NaCl + HOH → HCl + NaOH
Reverse of neutralization
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VI STRENGTH
Acid and base strength depend on number of ions in solution More ions; stronger acid or base
Some acids ionize 100% (strongest acids) HCl HBr HI H2SO4 HNO3 HClO4
Some bases ionize 100% (strongest bases) LiOH NaOH KOH RbOH CsOH NH4OH
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A. pH
Every aqueous solution contains H + and OH-
• Acids have more H+ than OH-
• Bases have more OH- than H+
pH represents the amount of H + in a solution
1 7 14
Strong Weak Neutral Weak Strong
acid acid base base
Most H+ Equal H+ and OH- Least H+
Least OH- Most OH -
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pH Scale is logarithmic•Values change by factors of 10
• ex. pH = 3 vs. pH = 5• Difference in pH• 2 units
• 10 x 10• pH 3 is 100 times stronger than pH 5• pH 5 is 1/100th as strong as pH 3
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B. Acid Base Indicators Compounds that change color over pH ranges
Table M Common Acid–Base Indicators• methyl orange 3.2–4.4 red to yellow• bromthymol blue 6.0–7.6 yellow to blue• phenolphthalein 8.2–10 colorless to
pink• litmus 5.5–8.2 red to blue• bromcresol green 3.8–5.4 yellow to
blue• thymol blue 8.0–9.6 yellow to blue