10.6: EndofChapter Material
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Additional Exercises
 What is the relationship between the K_{sp} expressions for a chemical reaction and its reverse chemical reaction?
 What is the relationship between the K_{w} value for H_{2}O and its reverse chemical reaction?
 For the equilibrium \[PCl_{3}(g)+Cl^{2+}(g)\rightleftharpoons PCl_{5}(g)+60kJ\nonumber \]
list four stresses that serve to increase the amount of PCl_{5}.  For the equilibrium \[N_{2}O_{4}+57kJ\rightleftharpoons 2NO_{2}\nonumber \]
list four stresses that serve to increase the amount of NO_{2}.  Does a very large K_{eq} favor the reactants or the products? Explain your answer.
 Is the K_{eq} for reactions that favor reactants large or small? Explain your answer.
 Show that K_{a} × K_{b} = K_{w} by determining the expressions for these two reactions and multiplying them together. \[HX(aq)\rightleftharpoons H^{+}(aq)+X^{}(aq)\\ X^{+}(aq)+H_{2}O(l)\rightleftharpoons HX(aq)+OH^{}(aq)\nonumber \]
 Is the conjugate base of a strong acid weak or strong? Explain your answer.
 What is the solubility in moles per liter of AgCl? Use data from Table \(\PageIndex{2}\)  Solubility Product Constants for Slightly Soluble Ionic Compounds.
 What is the solubility in moles per liter of Ca(OH)_{2}? Use data from Table \(\PageIndex{2}\)  Solubility Product Constants for Slightly Soluble Ionic Compounds.
 Under what conditions is K_{eq} = K_{P}?
 Under what conditions is K_{eq} > K_{P} when the temperature is 298 K?
 What is the pH of a saturated solution of Mg(OH)_{2}? Use data from Table \(\PageIndex{2}\)  Solubility Product Constants for Slightly Soluble Ionic Compounds.
 What are the pH and the pOH of a saturated solution of Fe(OH)_{3}? The K_{sp} of Fe(OH)_{3} is 2.8 × 10^{−39}.
 For a salt that has the general formula MX, an ICE chart shows that the K_{sp} is equal to x^{2}, where x is the concentration of the cation. What is the appropriate formula for the K_{sp} of a salt that has a general formula of MX_{2}?
 Referring to Exercise 15, what is the appropriate formula for the K_{sp} of a salt that has a general formula of M_{2}X_{3} if the concentration of the cation is defined as 2x, rather than x?
 Consider a saturated solution of PbBr_{2}(s). If [Pb^{2+}] is 1.33 × 10^{−5} M, find each of the following.
 [Br^{−}]
 the K_{sp} of PbBr_{2}(s)
 Consider a saturated solution of Pb_{3}(PO_{4})_{2}(s). If [Pb^{2+}] is 7.34 × 10^{−14} M, find each of the following.
 [PO_{4}^{3−}]
 the K_{sp} of Pb_{3}(PO_{4})_{2}(s)
Answers
 They are reciprocals of each other.


increase the pressure; decrease the temperature; add PCl_{3}; add Cl_{2}; remove PCl_{5}

 favor products because the numerator of the ratio for the K_{eq} is larger than the denominator
 \[K_{a}\times K_{b}=\frac{[H^{+}][X]}{[HX]}\times \frac{[HX][OH]}{[X]}=[H^{+}][OH^{}]=K_{W}\nonumber \]
 1.3 × 10^{−5} mol/L
 K_{eq} = K_{P} when the number of moles of gas on both sides of the reaction is the same.
 10.35
 4x^{3}
 ^{ }
 ^{ }
 2.66 × 10^{−5} M
 9.41 × 10^{−15}