Figure 3.1 Periodic Table.

18
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Figure 3.1 Periodic Table. Equivalent Weight, EW. EW = MW/Z. Z = valence or charge. g/eq or mg/meq. Normality, N. N = (mass of material/L or solution)/ EW = number of equivalents/ L of solution. N = z X M. Chemical Reactions. Types of Reactions. Synthesis or combination reactions - PowerPoint PPT Presentation

Transcript of Figure 3.1 Periodic Table.

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

Figure 3.1 Periodic Table.

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

Equivalent Weight, EW

EW = MW/Z

Z = valence or charge

g/eq or mg/meq

Normality, N

N = (mass of material/L or solution)/ EW = number of equivalents/ L of solution

N = z X M

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

Chemical Reactions

Types of Reactions

1) Synthesis or combination reactions A + B → C2) Decomposition reactions AB → A + B3) Single-replacement reactions A + BC → AC + B4) Double-replacement reactions AB + CD → AD + BC5) Combustion reactions C3H8 + 5 O2 → 3 CO2 + 4 H2O

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

Consider the following reactions:

CaO(S) + H2O(l) Ca(OH)2(s)→←

→←2 CaO(s) + 3 H2) + 2 PO43-

(aq) Ca3(PO4)2(s) + 6 OH-(aq)

Yielded by, formed fromReactants, productsSubscripts s, l, aqBalancedreversible

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

Generalized reaction:

aA + bB cC + dD←→

At equilibrium:

K = [C]c [D]d

[A]a [B]b

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

Stoichiometry

Law of Conservation of Mass

Balancing Equations1)Insure all products and reactants have proper formula2)Identify most complicated compound. Asume there is only one of these in the equation. Balance the elementsw in this compound one at a time.3)Focus initial attention on atoms present in the fewest compounds4)Continue on a trial and error basis for the remaining compounds. Generally, balance the most prevelant atoms near the end.5)Remove fractions and simplify to the smallest whole numbers possible.

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Introduction to Environmental Engineering, First EditionRichard O. Mines and Laura W. Lackey

Acid-Base Chemistry

pH = - log [H+]

pOH = - log[OH-]

pH + pOH = 14

Acid – a compound that donates a hydrogen ionBase – a substance that accepts a proton (hydrogen ion)

HA + B- → A- + HB←Acid Base Base Acid

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Figure 3.2 pH Estimates for common household items.

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Amphoteric compounds can react as either an acid or base

H2O + H2O ← HO- + H3O+

Acid Base Base Acid

H2O ← OH- + H+

→

→

K = [OH-] [H+]

[H2O]

Kw = [OH-] [H+] = 10-14

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Dissociation Constant

HA H+ + A-→←

Ka = [H+] [A-]

[HA]

BOH B+ + OH-

Kb =[B+] [OH-]

[BOH]

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pKa = - log Ka

pKb = -log Kb

Ka X Kb = Kw = 10-14

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Carbonates

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