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Review of Acids, Bases, & Salts
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Has H in the formula Produces H+ as the only positive ion in solution
Arrhenius Acid
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Inorganic – formula starts with H (except H2O & H2O2)
Organic – formula ends with COOH Formula of an Acid
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Properties of Acids Sour Taste Electrolytes
React with bases to form a salt + H2O Turn litmus RED React with most metals to produce H2(g) Properties of Acids
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Ionization of an Acid: Why is it so weird?
Because acids are covalent! Ionization of an Acid: Why is it so weird?
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HCl H+ + Cl- HCl + H2O H3O+ + Cl- Ionization of an Acid or
Arrhenius format or HCl + H2O H3O+ + Cl- Bronsted-Lowry format Ionization of an Acid
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HCl HNO3 HBr HClO4 HI H2SO4 Six strong acids?
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Ionization of a weak base: Why is it so weird?
Because weak bases are covalent! Ionization of a weak base: Why is it so weird?
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Autoionization of water
H2O H+ + OH- Autoionization of water
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Arrhenius Base (Strong bases)
Has OH in the formula Produces OH- as the only negative ion in solution Arrhenius Base (Strong bases)
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LiOH Ca(OH)2 NaOH Sr(OH)2 KOH Ba(OH)2
Six strong bases?
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Formula of a Strong Base
Has format M(OH)x M is a metal X can be 1, 2, or 3 Formula of a Strong Base
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Properties of Bases Bitter Taste Slippery Feel Electrolytes
React with acids to form a salt + H2O Turn litmus BLUE Properties of Bases
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Ionization of a strong base
NaOH Na+ + OH- Ionization of a strong base
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Ionization of NH3, a weak base
NH3 + H2O NH4+ + OH- Ionization of NH3, a weak base
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Metal + Nonmetal Formula of a Salt
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Write the formula of potassium sulfate
K+ & (SO4)2- K2SO4 Write the formula of potassium sulfate
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Electrolytes Solutions conduct – they contain ions
Acids (HX), bases (MOH), & salts (MX) are electrolytes Electrolytes
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Solutions of covalent compounds (all nonmetals), excepting the acids and the weak bases.
They do NOT conduct. NONelectrolytes
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Identify the electrolytes
Yes - B Yes - B 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 - A Yes - A Yes - A No Yes - S Yes - S Yes - A No No No Yes - A Yes - B Yes - A Yes - B No No
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0-14 Acidic: 0 to 7, Neutral: 7 Basic: 7-14
pH scale
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pH = -log[H+] pH = ?
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How do you get [H+] from pH?
[H+] = 10-pH How do you get [H+] from pH?
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pOH = -log[OH-] pOH = ?
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pK = -log[K] pK = ?
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pH = 0 Most acidic on pH scale
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pH = 14 Most basic on pH scale
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Hydroxide ion OH-
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Hydrogen ion or Proton H+
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Hydronium ion. Bronsted-Lowry form of H+. Used interchangeably with H+ .
H3O+
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[H+] [OH-] Acidic Solution
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[OH-] [H+] Basic Solution
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14, at 25C pH + pOH = ?
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If the pH changes from 3 to 5, how does the [H+] 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. It is 1/100 of the original [H+]. If the pH changes from 3 to 5, how does the [H+] change?
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How can pH be safely tested?
Instrumental – use pH meter Indicators – use a series of indicators to narrow down the pH range Test acids with metals (NOT Cu, Ag, or Au) How can pH be safely tested?
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Proton Donor Bronsted-Lowry Acid
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Proton Acceptor Bronsted-Lowry Base
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Bronsted-Lowry Acids & Bases
HCl + H2O H3O+ + Cl- Acid Base c. acid c. base Bronsted-Lowry Acids & Bases
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Complete or almost complete ionization.
Strong Acids & Bases
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Concentration of ions in .4 M HCl
Strong acid HCl H+ + Cl- Concentration of H+ = 0.4 M Concentration of Cl- = 0.4 M Concentration of ions in .4 M HCl
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Ionization occurs only to a slight extent, a few percent.
Weak Acids & Bases
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Reactions of Acids with Metals
Metal + Acid H2(g) + salt Reactions of Acids with Metals
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Zn(s) + 2HCl H2(g) + ZnCl2 Zn(s) + HCl ?
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2Al(s) + 6HCl 3H2(g) + 2AlCl3 Al(s) + HCl ?
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Neutralization Reactions
Acid + Base Salt + H2O Neutralization Reactions
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H+ + OH- H2O Net Ionic Equation for strong acid/strong base Neutralization Reactions
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Moles H+ = Moles OH- At equivalence point
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Molarity = Moles solute
Liters of soln Molarity (M)
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NYS Titration Equation
MaVa = MbVb This equation only works when the number of H’s on the acid EQUALS the number of OH’s on the base! NYS Titration Equation
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naMaVa = nbMbVb Titration Equation
This equation works when the number of H’s on the acid does NOT equal the number of OH’s on the base! na = number of acidic H’s in acid. nb = number of OH’s in base. Titration Equation
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-log[H+] or –log[H3O+] pH
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-log[OH-] pOH
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Equilibrium Constant Expression for aA(aq) + bB(aq) cC(aq) + D(aq)
[C]c[D]d [A]a[B]b K = Equilibrium Constant Expression for aA(aq) + bB(aq) cC(aq) + D(aq)
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Equilibrium Constant Expression for aA(s) + bB(aq) cC(s) + D(aq)
[D]d [B]b K = Equilibrium Constant Expression for aA(s) + bB(aq) cC(s) + D(aq)
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-logK pK
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14 pOH + pH =
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1.0 X 10-14 [OH-] X [H+] =
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The pH = The pOH = The [OH-] =
3 11 1 X 10-11 If the [H+] = 1 X 10-3
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Substance that changes color over a narrow pH range.
Indicator
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Molarity H2SO4 Vs. Molarity H+
H2SO4 2H+ + SO42- [H+] = 2[H2SO4] 2M H2SO4 4M H+ Molarity H2SO4 Vs. Molarity H+
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naMaVa = nbMbVb (1)X(20.0 mls) = (1).250M(50.0mls)
What is the concentration of a hydrochloric acid solution if 50.0 mL of a M KOH solution are needed to neutralize 20.0 mL of the HCl solution of unknown concentration?
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(1.50 M)(10.62 mls) = X(20.20 mls) Acid 1.50 M Base ? M Final Volume
16.07 24.25 Initial Volume 5.45 4.05 Amount Used 10.62 20.20 (1.50 M)(10.62 mls) = X(20.20 mls)
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Why do different salts produce solutions with different pHs?
Hydrolysis of the ions! Why do different salts produce solutions with different pHs?
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Reaction of ions with water to produce H+ or OH-
Hydrolysis
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Which anions undergo hydrolysis?
Anions of weak acids: they produce basic solutions. C2H3O H2O HC2H3O2 + OH- Which anions undergo hydrolysis?
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Which cations undergo hydrolysis?
Cations of weak bases: They produce acidic solutions. NH H2O H3O+ + NH3 Which cations undergo hydrolysis?
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