Chapter 17: Acids and Bases

*Know the material covered in Chemistry I related to acids and bases (see section 9.7).

Recognize that all equilibrium problems are solved in fundamentally the same manner using ICE tables.

Know how to determine the correct number of significant figures going from logs to exponents and vice versa.

DEFINE:

• Arrhenius acid and Arrhenius base.
• Brønsted-Lowry acid and Brønsted-Lowry base.
• Lewis acid and Lewis base and give examples of each

DO:

• State the names, formulas and uses of common acids and bases (tables 17.1 and 17.2)
• Learn the names and formulas of the common strong acids (table 17.3)
• Identify conjugate acid-base pairs
• Explain the difference between strong and weak acids (and strong and weak bases)
• Rank acids (either binary OR oxyacids) based on their acid strength
• Explain how bond polarity and bond strength influence the acidity of binary acids.
• Explain how the strength of oxyacids depends on the electronegativity of the central atom and the number of oxygens attached to that atom
• Write an expression for the acid ionization constant (K_a) and the base ionization constant K_b.
• Describe the autoionization of water to produce H₃O⁺ and OH^-
• Write the equilibrium expression for K_w and state that K_w=1.0x10^-14 at 25°C
• Recognize that p(x) = -log₁₀(x) and write mathematical relationships for pH, pOH and pK
• State and use the relationship between K_a, K_b and K_w
• Write equilibrium expressions for the stepwise ionization of polyprotic acids (K_a1, K_a2 etc…)
• Determine whether an aqueous solution of a cation, anion or salt is acidic, basic or pH-neutral.
• Explain how Lewis acids and bases react to form adducts.

CALCULATE:

• pH from [H₃O⁺], pOH from [OH^-] and pK_a from K_a ( and likewise pK_{( )} for other K_{( )}’s) and vice versa
• Use the relationship between pH, pOH and pK_w to convert between pH and pOH
• pH of a strong acid from [H₃O⁺] = [HA] and pOH of a strong base from [OH^-] = [B]
• Use ICE tables to set up the calculation of equilibrium concentrations for weak acids in water (using initial acid concentrations and K_a) and weak bases in water (using initial base concentrations and K_b)
• The percent ionization of a weak acid (or weak base)
• The pH of a mixture of acids after comparing the K_a’s to determine if one dominates the mixture.
• Determine the pH of a salt solution
• The concentration of each species present and the pH of a polyprotic acid solution using acid dissociation data and ICE tables

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