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Chapter 15: Q47E (page 874)

Question: A solution contains \(1.0 \times 1{0^{ - 2}}\)mol of KI and 0.10 mol of KCl per liter. \(AgN{O_3}\)is gradually added to this solution. Which forms first, solid AgI or solid AgCl?

Short Answer

Expert verified

The solid AgI will form first.

Step by step solution

01

Find which will form first:

For AgCl,

\(\begin{array}{*{20}{c}}{{K_{sp}}(AgCl) = \left( {A{g^ + }} \right)\left( {C{l^ - }} \right) = 1.8 \times {{10}^{ - 10}}}\\{\left( {A{g^ + }} \right) = \frac{{1.8 \times {{10}^{ - 10}}}}{{0.10M}} = 1.8 \times {{10}^{ - 9}}M}\end{array}\)

For AgI,

\(\begin{array}{*{20}{c}}{{K_{sp}}(AgI) = \left( {A{g^ + }} \right)\left( {{I^ - }} \right) = 1.5 \times {{10}^{ - 16}}}\\{\left( {A{g^ + }} \right) = \frac{{1.5 \times {{10}^{ - 16}}}}{{1 \times {{10}^{ - 2}}M}} = 1.5 \times {{10}^{ - 9}}M}\end{array}\)

\(\left( {A{g^ + }} \right)(AgCl) > \left( {A{g^ + }} \right)(AgI)\)

Therefore the solution is solid AgI will form first.

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Most popular questions from this chapter

Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:

\(\begin{array}{l}(a)KH{C_4}{H_4}{O_6}\\(b)Pb{I_2}\\(c)A{g_4}\left[ {Fe{{(CN)}_6}} \right],a salt containing the Fe{(CN)_4}^ - ion\\(d)H{g_2}{I_2}\end{array}\)

Identify all chemical species present in an aqueous solution of \(C{a_3}{\left( {P{O_4}} \right)_2}\)and list these species in decreasing order of their concentrations. (Hint: Remember that the \(PO_4^{3 - }\) ion is a weak base.)

Calculate the concentration of Ag+ required to begin precipitation of Ag2CO3 in a solution that is 2.50 脳 10-6M in CO3 2-

Question: The calcium ions in human blood serum are necessary for coagulation (Figure 15.5). Potassium oxalate, \({K_2}{C_2}{O_4}\), is used as an anticoagulant when a blood sample is drawn for laboratory tests because it removes the calcium as a precipitate of\(Ca{C_2}{O_4} \times {H_2}O\). It is necessary to remove all but 1.0% of the \(C{a^{2 + }}\) in serum in order to prevent coagulation. If normal blood serum with a buffered pH of 7.40 contains 9.5 mg of \(C{a^{2 + }}\) per 100 mL of serum, what mass of \({K_2}{C_2}{O_4}\)is required to prevent the coagulation of a 10 mL blood sample that is 55% serum by volume? (All volumes are accurate to two significant figures. Note that the volume of serum in a 10-mL blood sample is 5.5 mL. Assume that the \({K_{sp}}\)value for \(Ca{C_2}{O_4}\)in serum is the same as in water.)

The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem:

MgF2 (S) 鈬� Mg2+(aq) + 2F- (aq)

In a saturated solution of MgF2 at 18 掳C, the concentration ofMg2+is 1.21脳10-3 M.

The equilibrium is represented by the preceding equation.

(a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 掳C.

(b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2solution at 18 掳C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible.

(c) Predict whether a precipitate of MgF颅2 will form whensolution of 100.0mL of a 3.00 脳10-3 -M Mg(NO3)2 is mixed with 200.0 mL of a 2.00 脳 10鈥�3 -M solution of NaF at 18 掳C. Show the calculations to support your prediction.

(d) At 27 掳C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17脳10-3 M. Is the dissolving of MgF2 in water an endothermic or an exothermic process? Give an explanation to support your conclusion.
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