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180 Chemistry: Matter and Change
Solving Problems: A Chemistry Handbook
SOLVING PROBLEMS:
A CHEMISTRY HANDBOOK
CHAPTER 17
Common ion effect The solubility of a substance is reduced
when the substance is dissolved in a solution containing a common
ion. This is called the common ion effect. For example, PbI 2 is less
soluble in an aqueous solution of NaI than in pure water because the
common ion I Ϫ , already present in the NaI solution, reduces the
maximum possible concentration of Pb 2ϩ and thus reduces the solubility of PbI 2 .
Chapter 17 Review
16. If an equilibrium system contains small amounts of reactants
and large amounts of products, what can you say about the
value of K eq for this equilibrium?
17. The following is the equation for a homogeneous equilibrium.
2A ϩ B 3 2C
What is the value of K eq if [B] ϭ 0.14 mol/L and [C]
ϭ 3.0 ϫ [A]?
18. Is it possible to cause a shift in an equilibrium system without
changing the equilibrium constant? Explain.
19. In a reversible endothermic reaction, four moles of gaseous
reactants yield three moles of gaseous products. Describe four
ways to shift this equilibrium toward the products.
20. At 298 K, the molar solubility of Fe(OH) 2 is higher than that
of AgI, but K sp for Fe(OH) 2 is less than K sp for AgI. Explain
how this is possible.
21. Would you expect Ag 2 CO 3 to be more soluble in pure water or
in a 1.0M Na 2 CO 3 solution? Explain your answer.
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