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Chapter 4: Problem 28

Three solutions are mixed together to form a single solution. One contains \(0.2 \mathrm{~mol} \mathrm{~Pb}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\), the second contains \(0.1 \mathrm{~mol} \mathrm{Na}_{2} \mathrm{~S}\), and the third contains \(0.1 \mathrm{~mol}\) \(\mathrm{CaCl}_{2}\). (a) Write the net ionic equations for the precipitation reaction or reactions that occur. (b) What are the spectator ions in the solution?

Short Answer

Expert verified
Three precipitation reactions occur when the solutions are mixed: 1. \(Pb^{2+}(aq) + S^{2-}(aq) \rightarrow PbS(s)\) 2. \(Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s)\) 3. \(Ca^{2+}(aq) + S^{2-}(aq) \rightarrow CaS(s)\) The spectator ions in the solution are \(Na^+\) and \(CH_3COO^-\).

Step by step solution

01

1. \(Pb^{2+}\) and \(S^{2-}\)

These ions could form \(PbS\), which is insoluble according to rule 4. The net ionic equation is: \[Pb^{2+}(aq) + S^{2-}(aq) \rightarrow PbS(s)\]
02

2. \(Pb^{2+}\) and \(Cl^-\)

These ions could form \(PbCl_2\), which is insoluble according to rule 3. The net ionic equation is: \[Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s)\]
03

3. \(Ca^{2+}\) and \(S^{2-}\)

These ions could form \(CaS\), which is insoluble according to rule 4. The net ionic equation is: \[Ca^{2+}(aq) + S^{2-}(aq) \rightarrow CaS(s)\] There are no more possible precipitation reactions between the given ions. #b) Spectator ions in the solution#
04

Spectator ions

The spectator ions are the ions that do not participate in any precipitation reactions. In this case, we can see from the net ionic equations that the two spectator ions are: 1. Sodium ion (\(Na^{+}\)) 2. Acetate ion (\(CH_3COO^{-}\))

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Most popular questions from this chapter

A sample of \(5.53 \mathrm{~g}\) of \(\mathrm{Mg}(\mathrm{OH})_{2}\) is added to \(25.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HNO}_{3}\). (a) Write the chemical equation for the reaction that occurs. (b) Which is the limiting reactant in the reaction? (c) How many moles of \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{HNO}_{3}\), and \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) are present after the reaction is complete?

Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (a) \(\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(a q) \longrightarrow\) (b) \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\) (c) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{KOH}(a q) \longrightarrow\)

Acetone, \(\mathrm{CH}_{3} \mathrm{COCH}_{3}\), is a nonelectrolyte; hypochlorous acid, \(\mathrm{HClO}\), is a weak electrolyte; and ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl}\), is a strong electrolyte. (a) What are the solute particles present in aqueous solutions of each compound? (b) If \(0.1 \mathrm{~mol}\) of each compound is dissolved in solution, which one contains \(0.2 \mathrm{~mol}\) of solute particles, which contains \(0.1 \mathrm{~mol}\) of solute particles, and which contains somewhere between \(0.1\) and \(0.2 \mathrm{~mol}\) of solute particles?

(a) How would you prepare \(175.0 \mathrm{~mL}\) of \(0.150 \mathrm{MAgNO}_{3}\) solution starting with pure solute? (b) An experiment calls for you to use \(100 \mathrm{~mL}\) of \(0.50 \mathrm{M} \mathrm{HNO}_{3}\) solution. All you have available is a bottle of \(3.6 \mathrm{M} \mathrm{HNO}_{3}\). How would you prepare the desired solution?

If you want to double the concentration of a solution, how could you do it? [Section 4.5]
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