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Understanding Chemical Reactions, Stoichiometry, and Acid-Base Chemistry Basics

This guide covers foundational concepts in chemistry, including the types of chemical reactions such as synthesis, decomposition, single and double replacement, and combustion. It discusses the principles of stoichiometry, balancing equations, and the law of conservation of mass. The section on acid-base chemistry defines pH and pOH, explores the behavior of acids and bases, and provides insights into amphoteric compounds. Additionally, it includes calculations for normality, equivalent weight, and dissociation constants, solidifying the relationship between reactants and products.

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Understanding Chemical Reactions, Stoichiometry, and Acid-Base Chemistry Basics

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  1. Figure 3.1 Periodic Table.

  2. 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

  3. Chemical Reactions Types of Reactions • Synthesis or combination reactions • A + B → C • Decomposition reactions • AB → A + B • 3) Single-replacement reactions • A + BC → AC + B • 4) Double-replacement reactions • AB + CD → AD + BC • 5) Combustion reactions • C3H8 + 5 O2 → 3 CO2 + 4 H2O

  4. 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 from Reactants, products Subscripts s, l, aq Balanced reversible

  5. Generalized reaction: ← aA + bB cC + dD → At equilibrium: [C]c [D]d K = [A]a [B]b

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

  7. Acid-Base Chemistry pH = - log [H+] pOH = - log[OH-] pH + pOH = 14 Acid – a compound that donates a hydrogen ion Base – a substance that accepts a proton (hydrogen ion) HA + B-→ A- + HB ← Acid Base Base Acid

  8. Figure 3.2 pH Estimates for common household items.

  9. Amphoteric compounds can react as either an acid or base → H2O + H2O ← HO- + H3O+ Acid Base Base Acid → H2O ← OH- + H+ [OH-] [H+] K = [H2O] Kw = [OH-] [H+] = 10-14

  10. Dissociation Constant → HA H+ + A- ← [H+] [A-] Ka = [HA] BOH B+ + OH- [B+] [OH-] Kb = [BOH]

  11. pKa = - log Ka pKb = -log Kb Ka X Kb = Kw = 10-14

  12. Carbonates

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