Exam 2 Flashcards by Aaron Bevins

Arrhenius Plot equation

ln(k) = -Ea / R (1/T) + ln(A)

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gas constant (Arrhenius Equation)

R = 8.314 J/mol*K

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Acid Ionization Constant (HClO2)

1.1 * 10^-2

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Acid Ionization Constant (HNO2)

4.6 * 10^-4

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Acid Ionization Constant (HF)

3.5 * 10^-4

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Acid Ionization Constant (HCHO2)

1.8 * 10^-4

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Acid Ionization Constant (HC7H5O2)

6.5 * 10^-5

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Acid Ionization Constant (HC2H3O2)

1.8 * 10^-5

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Acid Ionization Constant (HClO)

2.9 * 10^-8

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Acid Ionization Constant (HCN)

4.9 * 10^-10

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Acid Ionization Constant (HC6H5O)

1.3 * 10^-10

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Percent ionization of a weak acid _________ with increasing concentration of the acid

Decreases

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The equilibrium H3O+ concentration of a weak acid _________ with increasing initial concentration of the acid

Increases

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Kw =

1.0 * 10^-14

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Strong Bases

LiOH, NaOH, KOH, Sr(OH)2, Ca(OH)2, Ba(OH)2

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Kb [(CO3)2-]

1.8 * 10^-4 (must occur with a + charge ion)

Kb (CH3NH2)

4.4 * 10^-4

Kb (C2H5NH2)

5.6 * 10^-4

Kb NH3

1.76 * 10^-5

Kb [(HCO3)-]

2.3 * 10^-8 (must occur with a + charge ion)

Kb (C5H5N)

1.7 * 10^-9

Kb (C6H5NH2)

3.9 * 10^-10

Give an example of a triprotic acid

Phosphoric Acid (H3PO4)

Give an example of a diprotic acid

Carbonic Acid (H2CO3), Sulfurous acid (H2SO3), Sulfuric Acid (H2SO4)

Integrated Rate Law of a 0 order reaction

[A]t = -kt + [A]0

Half-Life expression of a 0 order reaction

t1/2 = (1/k) ([A]0/2)

Half-Life expression of a 1st order reaction

t1/2 = (1/k)(0.693)

Half-Life expression of a 2nd order reaction

t1/2 = (1/k)(1/[A]0)

Integrated Rate Law of a 1st order reaction

ln[A]t = (-kt) + ln[A]0

Integrated Rate Law of a 2nd order reaction

1/[A]t = (kt)+(1/[A]0)