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Chapter 4: Problem 56

Give an example how each of the following insoluble ionic compounds could be produced using a precipitation reaction. Write the balanced formula equation for each reaction. a. \(\mathrm{Fe}(\mathrm{OH})_{3}(s)\) c. \(\mathrm{PbSO}_{4}(s)\) b. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}(s)\) d. \(\mathrm{BaCrO}_{4}(s)\)

Short Answer

Expert verified
a. \[\mathrm{Fe(NO_{3})_{3}(aq) + 3NaOH(aq) \rightarrow Fe(OH)_{3}(s) + 3NaNO_{3}(aq)}\] b. \[\mathrm{Hg_{2}(NO_{3})_{2}(aq) + 2NaCl(aq) \rightarrow Hg_{2}Cl_{2}(s) + 2NaNO_{3}(aq)}\] c. \[\mathrm{Pb(NO_{3})_{2}(aq) + Na_{2}SO_{4}(aq) \rightarrow PbSO_{4}(s) + 2NaNO_{3}(aq)}\] d. \[\mathrm{Ba(NO_{3})_{2}(aq) + K_{2}CrO_{4}(aq) \rightarrow BaCrO_{4}(s) + 2KNO_{3}(aq)}\]

Step by step solution

01

a. Formation of \(\mathrm{Fe}(\mathrm{OH})_{3}(s)\)

To produce the insoluble ionic compound \(\mathrm{Fe}(\mathrm{OH})_{3}(s)\), mix solutions containing iron(III) ions and hydroxide ions. An example would be mixing \(\mathrm{Fe(NO_{3})_{3}}\)(solution) and \(\mathrm{NaOH}\)(solution). The balanced formula equation for the reaction is: \[\mathrm{Fe(NO_{3})_{3}(aq) + 3NaOH(aq) \rightarrow Fe(OH)_{3}(s) + 3NaNO_{3}(aq)}\]
02

b. Formation of \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}(s)\)

For producing the insoluble ionic compound \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}(s)\), mix the solutions containing mercury(I) ions, like \(\mathrm{Hg_{2}NO_{3}(s)}\) and chloride ions, like \(\mathrm{NaCl(s)}\). The balanced formula equation for the reaction is: \[\mathrm{Hg_{2}(NO_{3})_{2}(aq) + 2NaCl(aq) \rightarrow Hg_{2}Cl_{2}(s) + 2NaNO_{3}(aq)}\]
03

c. Formation of \(\mathrm{PbSO}_{4}(s)\)

To form the insoluble ionic compound \(\mathrm{PbSO}_{4}(s)\), mix solutions containing lead(II) ions and sulfate ions. An example would be mixing \(\mathrm{Pb(NO_{3})_{2}}\)(solution) and \(\mathrm{Na_{2}SO_{4}}\)(solution). The balanced formula equation for the reaction is: \[\mathrm{Pb(NO_{3})_{2}(aq) + Na_{2}SO_{4}(aq) \rightarrow PbSO_{4}(s) + 2NaNO_{3}(aq)}\]
04

d. Formation of \(\mathrm{BaCrO}_{4}(s)\)

For producing the insoluble ionic compound \(\mathrm{BaCrO}_{4}(s)\), mix the solutions containing barium ions and chromate ions. An example would be mixing \(\mathrm{Ba(NO_{3})_{2}}\)(solution) and \(\mathrm{K_{2}CrO_{4}}\)(solution). The balanced formula equation for the reaction is: \[\mathrm{Ba(NO_{3})_{2}(aq) + K_{2}CrO_{4}(aq) \rightarrow BaCrO_{4}(s) + 2KNO_{3}(aq)}\]

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Most popular questions from this chapter

Chlorisondamine chloride $\left(\mathrm{C}_{14} \mathrm{H}_{20} \mathrm{Cl}_{6} \mathrm{N}_{2}\right)$ is a drug used in the treatment of hypertension. A 1.28-g sample of a medication containing the drug was treated to destroy the organic material and to release all the chlorine as chloride ion. When the filtered solution containing chloride ion was treated with an excess of silver nitrate, 0.104 g silver chloride was recovered. Calculate the mass percent of chlorisondamine chloride in the medication, assuming the drug is the only source of chloride.

Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: $$\mathrm{IO}_{3}^{-}(a q)+\mathrm{I}^{-}(a q) \longrightarrow \mathrm{I}_{3}^{-}(a q)$$ Triodide ion concentration is determined by titration with a sodium thiosulfate \(\left(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\right)\) solution. The products are iodide ion and tetrathionate ion \(\left(\mathrm{S}_{4} \mathrm{O}_{6}^{2-}\right)\) a. Balance the equation for the reaction of \(\mathrm{IO}_{3}^{-}\) with \(\mathrm{I}^{-}\) ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HCl required to convert all of the 1 \(\mathrm{O}_{3}^{-}\) ions to \(\mathrm{I}_{3}^{-}\) ions? c. Write and balance the equation for the reaction of $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\( with \)\mathrm{I}_{3}-$ in acidic solution. d. A 25.00 -mL sample of a 0.0100\(M\) solution of \(\mathrm{KIO}_{3}\) is reacted with an excess of \(\mathrm{KL}\) . It requires 32.04 \(\mathrm{mL}\) of \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) solution to titrate the \(\mathrm{I}_{3}^{-}\) ions present. What is the molarity of the \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) solution? e. How would you prepare 500.0 \(\mathrm{mL}\) of the KIO\(_{3}\)solution in part d using solid \(\mathrm{KIO}_{3} ?\)

You are given a solid that is a mixture of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) A 0.205-g sample of the mixture is dissolved in water. An excess of an aqueous solution of \(\mathrm{BaCl}_{2}\) is added. The BaSO\(_{4}\) that is formed is filtered, dried, and weighed. Its mass is 0.298 g. What mass of \(\mathrm{SO}_{4}^{2-}\) ion is in the sample? What is the mass percent of \(\mathrm{SO}_{4}^{2-}\) ion in the sample? What are the percent compositions by mass of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the sample?

A 10.00-mL sample of sulfuric acid from an automobile battery requires 35.08 mL of 2.12 M sodium hydroxide solution for complete neutralization. What is the molarity of the sulfuric acid? Sulfuric acid contains two acidic hydrogens

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide
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