Review of Acids, Bases, & Salts
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Transcript of Review of Acids, Bases, & Salts
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Review of Acids, Bases, & Review of Acids, Bases, & SaltsSalts
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Arrhenius AcidArrhenius Acid
•Has H in the formula•Produces H+ as the only positive ion in solution
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Formula of an AcidFormula of an Acid
•Inorganic – formula starts with H•Organic – formula ends with COOH
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Properties of AcidsProperties of Acids
•Sour Taste•Electrolytes
•React with bases to form a salt + H2O
•Turn litmus RED•React with most metals to produce H2(g)
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Ionization of an AcidIonization of an Acid
HCl H+ + Cl-
HCl + H2O H3O+ + Cl-oror
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Arrhenius BaseArrhenius Base
•Has OH in the formula•Produces OH- as the only negative ion in solution
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Formula of a BaseFormula of a Base
•Has format MOH•M is a metal
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Properties of BasesProperties of Bases
•Bitter Taste•Slippery Feel•Electrolytes•React with acids to form a salt + H2O•Turn litmus BLUE
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Ionization of a BaseIonization of a Base
NaOH Na+ + OH-
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Ionization of NHIonization of NH33
NH3 + H2O NH4+ + OH-
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Formula of a SaltFormula of a Salt
Metal + Nonmetal
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Write the formula of Write the formula of potasium sulfatepotasium sulfate
K+ & (SO4)2-
KK22SOSO44
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ElectrolytesElectrolytes
•Solutions conduct – they contain ions•Acids (HX), bases (MOH), & salts (MX) are electrolytes
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NONNONelectrolyteselectrolytes
Solutions of covalent compounds (all nonmetals). They do NOT
conduct.
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Identify the electrolytes Identify the electrolytes
• LiOH• CH3COOH• C6H12O6
• NaNO3
• H2SO4
• CH3OH• Ca(OH)2
• HCl• C8H18
• Al(OH)3
• HNO3
• CH3CH2COOH• K2SO4
• CH3CHOHCH3
• CH3OCH3
• H3PO4
• Mg(OH)2
• CH3CH2OH
Yes - BYes - BYes - AYes - A
NNooYes - SYes - S
Yes - AYes - A
NoNoYes - BYes - B
Yes - AYes - A
NoNo
Yes - BYes - BYes - AYes - A
Yes - AYes - A
Yes - SYes - SNoNo
NoNoYes - AYes - A
Yes - BYes - BNoNo
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pH scalepH scale
0-14Acidic: 0 to 7,
Neutral: 7Basic: 7-14
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Most acidic on pH scaleMost acidic on pH scale
pH = 0
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Most basic on pH scaleMost basic on pH scale
pH = 14
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OHOH--
Hydroxide ion
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HH++
Hydrogen ionor
Proton
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HH33OO++
Hydronium ion. Interchangeable with H+.
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Acidic SolutionAcidic Solution
[H+] [OH-]
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Basic SolutionBasic Solution
[OH-] [H+]
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If the pH changes from 3 If the pH changes from 3 to 5, how does the [Hto 5, how does the [H++] ]
change?change?
The pH changes by 2, so the [H+] changes by 102 or 100X. Since the
pH went up, it became LESS acidic. The new solution has a [H+] 100
times less than the original solution.
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How can pH be safely How can pH be safely tested?tested?
Instrumental – use pH meterIndicators – use a series of indicators to narrow down the pH rangeTest acids with metals (NOTNOT Cu, Ag, or Au)
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Bronsted-Lowry AcidBronsted-Lowry Acid
Proton Donor
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Bronsted-Lowry BaseBronsted-Lowry Base
Proton Acceptor
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Bronsted-Lowry Acids & Bronsted-Lowry Acids & BasesBases
HCl + H2O H3O+ + Cl-
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Strong Acids & BasesStrong Acids & Bases
Complete or almost complete ionization.
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Weak Acids & BasesWeak Acids & Bases
Ionization occurs only to a slight extent, a few
percent.
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Reactions of Acids with Reactions of Acids with MetalsMetals
Metal + Acid H2(g) + salt
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Zn(s) + HCl Zn(s) + HCl ? ?
Zn(s) + 2HCl Zn(s) + 2HCl H H22(g) + ZnCl(g) + ZnCl22
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Al(s) + HCl Al(s) + HCl ? ?
2Al(s) + 6HCl 2Al(s) + 6HCl 3H 3H22(g) + 2AlCl(g) + 2AlCl33
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Neutralization ReactionsNeutralization Reactions
Acid + Base Salt + H2O
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Net Ionic Equation for Net Ionic Equation for Neutralization ReactionsNeutralization Reactions
H+ + OH- H2O
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At neutralizationAt neutralization
Moles H+ = Moles OH-
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Molarity (M)Molarity (M)
Molarity = Moles solute Liters of soln
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Titration EquationTitration Equation
MaVa = MbVb
This equation works when the This equation works when the number of H’s on the acid number of H’s on the acid EQUALS the number of OH’s on EQUALS the number of OH’s on the base!the base!
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Titration EquationTitration Equation
naMaVa = nbMbVb
This equation works when the This equation works when the number of H’s on the acid does NOT number of H’s on the acid does NOT equal the number of OH’s on the equal the number of OH’s on the base!base!nnaa = number of acidic H’s in acid. = number of acidic H’s in acid.nnbb = number of OH’s in base. = number of OH’s in base.
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pHpH
-log[H+] or –log[H3O+]
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pOHpOH
-log[OH-]
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pOH + pH = pOH + pH =
14
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[OH[OH--] X [H] X [H++] = ] =
1.0 X 10-14
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If the [HIf the [H++] = 1 X 10] = 1 X 10-3-3
1.The pH =2.The pOH =3.The [OH-] =
33
1111
1 X 101 X 10-11-11
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IndicatorIndicator
Substance that changes color over a narrow
pH range.
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Molarity HMolarity H22SOSO44 Vs. Molarity H Vs. Molarity H++
H2SO4 2H+ + SO42-
[H+] = 2[H2SO4]
2M H2SO4 4M H+
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What is the concentration of a What is the concentration of a hydrochloric acid solutionhydrochloric acid solution if 50.0 mL50.0 mL
of a 0.250 M KOH0.250 M KOH solution are needed to neutralize 20.0 mL20.0 mL of the of the
HClHCl solution solution of unknown concentration?
MaVa = MbVb
X(20.0 mls) = .250M(50.0mls)
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Acid1.50 M
Base? M
Final Volume 16.07 24.25
Initial Volume 5.45 4.05
Amount Used
(1.50 M)(10.62 mls) = X(20.20 (1.50 M)(10.62 mls) = X(20.20 mls)mls)
10.62 20.20