Honors Chemistry
Study Guide – Chapter 16
Test Date: ______
· Chapter 16: Acid-Base Equilibria
Be able to . . . .
o Identify the properties of acid and bases discussed in both the reading guide and the introductory video.
o Give the general equation for a neutralization reaction.
§ In a neutralization reaction, acids and bases combine so that the properties of each are lost.
o Define Arrhenius, Bronsted-Lowry and Lewis acids and bases and identify any limitations with these theories.
o Write the name of an acid when given its formula and write the formula for an acid when given its name.
§ Review your polyatomic ions!
o Name and write the formulas for the seven strong acids and the examples of strong bases we discussed in class.
o Explain the meaning of the word amphoteric; write two chemical equations for an amphoteric substance, one in which it behaves as an acid and one in which it behaves as a base.
o Identify conjugate acid-base pairs and recall that there is an inverse relationship between the strengths of the components in this pair.
§ A strong acid has a weak conjugate base; a strong base has a weak conjugate acid.
o Use the strength of an acid to decide which type of arrow (single or double) is appropriate when that acid is combined with water and predict the resulting products.
§ If an acid is polyprotic (more than one ionizable hydrogen atom), you must draw each consecutive removal of the hydrogen ion.
o Convert between pH, pOH, [H+] and [OH-]; decide if a solution is acidic, basic, or neutral.
o Find the pH, pOH, [H+] and [OH-] for a strong acid or base.
§ Be careful when working with Ca(OH)2, Sr(OH)2, and Ba(OH)2. For every one mole of base that dissociates, there are two moles of OH- generated. For example, if you have a 0.025 M solution of Ca(OH)2, you have a [OH-] = 0.05 M.
o Find the pH, pOH, [H+] and [OH-] for a weak acid or base; calculate Ka for a weak acid and Kb for a weak base.
§ Unlike strong acids and bases, weak acids and bases do not completely dissociate so an ICE table should be used.
§ Because the value of K is so small for a weak acid or base, you may assume that “x” is such a small number that it is negligible when subtracting it from the initial value of the weak acid or base. This will allow you to forgo needing the quadratic formula when solving for “x”.
o Find the percent ionization for a weak acid or base after completing an ICE table problem.
o Explain why the value of the equilibrium-constant (K) for a weak acid or base is less than one, while the value of K for a strong acid or base is greater than one.
§ Each dissociation step for a polyprotic acid has its own Ka value. The first Ka value is always the largest, meaning it is the easier proton to remove.