Unit IX Study Guide: Acids and Bases
Chapters 14, 15 and 18.3
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Nomenclature/formula writing (especially acids and ionic compounds)
Polyatomic ions
Strong/weak electrolytes
Dissociation and ionization
Double replacement reactions
Molarity
Logarithms
Equilibrium constants
Stoichiometry
To Memorize:
**Definitions of all words in bold
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Properties of acids (page 468)
Properties of bases (page 471)
3 main types of acids and bases
Strong acids and bases (table 2 on page 501) and NH3 is a weak base
Relationship between an acid or a base and its conjugate
Kw=[OH-][H3O+]= 1.0x10-14 at 25°C
Table 4 on page 504
pH + pOH = 14
Purpose and function of an indicator
Parts of a titration curve including explanations of the pH at various time points
Steps 1-4 on page 520
Ka and Kb expressions
Ka x Kb = Kw
Components of a buffer
Henderson-Hasselbalch equation
Hydrolysis of anions and cations
To Master:
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Classify an acid or base as one of the 3 types.
Identify acids, bases, conjugate acids, and conjugate bases in a given acid/base equation.
Predict the products of an acid/base reaction using a ‘strength of acids’ chart.
Write neutralization reactions.
Calculate the pH or pOH of a solution when given [H3O+], [H+] or [OH-] and identify the solution as acidic, basic
or neutral.
Calculate the pH of a strong acid or strong base solution when given the molarity.
Determine the appropriate indicator for a titration or determine the pH range of a solution when given the chart on
page 513 and color data (you do NOT need to memorize the chart).
Determine the concentration of an unknown solution when given titration data.
Write the Ka or Kb expression for a given acid, base or conjugate.
Calculate the Ka or Kb for a weak acid or base when given its concentration and the pH of the solution or
calculate the pH when given its dissociation constant and initial concentration.
Calculate the Kb for a weak base given Ka of its conjugate acid, or Ka from Kb.
Describe how a buffer solution is usually prepared and be able to use the Henderson-Hasselbalch equation to
calculate the pH.
Write reactions for the addition of an acid or a base to a buffer.
Draw titration curves for various types of titrations and label the equivalence point (greater than, less than or
equal to pH =7) and buffer regions where appropriate.