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Chapter 6: Problem 52

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. \(\mathrm{Hg}_2(NO_3)_2(aq) + 2NaCl(aq) \rightarrow Hg_2Cl_2(s) + 2NaNO_3(aq)\) c. \(\mathrm{Pb(NO_3)_2 (aq) + Na_2SO_4 (aq) \rightarrow PbSO_4 (s) + 2NaNO_3(aq)}\) d. \(\mathrm{Ba(NO_3)_2 (aq) + K_2CrO_4 (aq) \rightarrow BaCrO_4 (s) + 2KNO_3(aq)}\)

Step by step solution

01

a. Precipitation Reaction for Fe(OH)鈧�

To produce \(\mathrm{Fe}(\mathrm{OH})_{3}(s)\) as a precipitate, we need two soluble reactants that form this compound. One option is choosing a soluble iron compound (such as \(\mathrm{Fe}^{3+}\) salt) and a source of the hydroxide ion, \(\mathrm{OH}^{-}\) (like \(\mathrm{NaOH}\)). The balanced formula equation for this reaction is: \[\mathrm{Fe(NO_3)_3 (aq) + 3NaOH (aq) \rightarrow Fe(OH)_3 (s) + 3NaNO_3(aq)}\]
02

b. Precipitation Reaction for Hg鈧侰l鈧�

To form \(\mathrm{Hg}_{2}\mathrm{Cl}_{2}(s)\) as the precipitate, we need a soluble mercury(I) compound and a soluble source of chloride ions. For instance, we can use \(\mathrm{Hg}_{2}(\mathrm{NO}_{3})_{2}\) as the mercury(I) compound and \(\mathrm{NaCl}\) as the chloride source. The balanced formula equation for this reaction is: \[\mathrm{Hg}_2(NO_3)_2(aq) + 2NaCl(aq) \rightarrow Hg_2Cl_2(s) + 2NaNO_3(aq)\]
03

c. Precipitation Reaction for PbSO鈧�

In order to form \(\mathrm{PbSO}_4(s)\) as a precipitate, we can choose a soluble lead(II) compound such as \(\mathrm{Pb(NO_3)_2}\) and a soluble sulfate source like \(\mathrm{Na_2SO_4}\). The balanced formula equation for this reaction is: \[\mathrm{Pb(NO_3)_2 (aq) + Na_2SO_4 (aq) \rightarrow PbSO_4 (s) + 2NaNO_3(aq)}\]
04

d. Precipitation Reaction for BaCrO鈧�

To produce \(\mathrm{BaCrO}_4(s)\) precipitate, we must select a soluble barium compound, for example, \(\mathrm{Ba(NO_3)_2}\), and a soluble source of chromate ions like \(\mathrm{K_2CrO_4}\). The balanced formula equation for this reaction is: \[\mathrm{Ba(NO_3)_2 (aq) + K_2CrO_4 (aq) \rightarrow BaCrO_4 (s) + 2KNO_3(aq)}\]

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Insoluble Ionic Compounds
Insoluble ionic compounds are those that do not dissolve significantly in water. They tend to form precipitates when mixed in aqueous solutions. A precipitate is a solid substance that appears out of a liquid solution due to a chemical reaction. Known for their low solubility, these compounds are crucial in predicting precipitation reactions.
For example,
  • Fe(OH)_3 is insoluble and forms when iron(III) ions meet hydroxide ions in solution.
  • PbSO_4 precipitates when lead(II) ions bond with sulfate ions.
Recognizing insoluble ionic compounds helps in conducting practical experiments that require precise outcomes, like in laboratory synthesis or wastewater treatment.
Balanced Formula Equations
Balanced formula equations ensure that the number of atoms for each element is the same on the reactant and product sides of a chemical equation. This law, known as the Law of Conservation of Mass, states that mass cannot be created or destroyed in a chemical reaction. Therefore, equations need accurate balancing to reflect this principle.
For instance, to produce Fe(OH)_3, the equation is balanced as:
  • Fe(NO_3)_3(aq) + 3NaOH(aq) 鈫� Fe(OH)_3(s) + 3NaNO_3(aq)
Here, the balanced equation means every atom present in the reactants is accounted for in the products. This ensures precision in lab settings and accurate predictions in chemical processes.
Solubility Rules
Solubility rules are guidelines used to predict the solubility of ionic compounds in water. These rules are not absolute but provide a good basis for anticipating whether a compound will dissolve or form a precipitate. Understanding these rules is pivotal in determining the outcomes of mixing solutions.
Here are some basics:
  • Most nitrates (NO_3) are soluble.
  • Chlorides (Cl), bromides (Br), and iodides (I) are generally soluble, except those of silver (Ag), lead (Pb), and mercury (Hg).
  • Sulfates (SO_4) are mostly soluble, with exceptions like barium (Ba), lead (Pb), and calcium (Ca) sulfates.
  • Hydroxides (OH) are typically insoluble except for those of strong base cations like sodium (Na) and potassium (K).
Learning these guidelines helps predict possible reactions and informs laboratory practices necessary for creating desired chemical substances.
Chemical Reactions
Chemical reactions involve the transformation of substances through the breaking and forming of chemical bonds, resulting in different substances called products. These reactions can produce gases, changes in color, temperature shifts, or precipitates. Precipitation reactions, in particular, involve the formation of an insoluble solid from aqueous reactants.
For example, the formation of PbSO_4 from Pb(NO_3)_2 and Na_2SO_4 happens when lead and sulfate ions react to form an insoluble precipitate. This process is part of many natural and industrial procedures, including water purification and metal recovery.
  • Understanding chemical reactions helps in designing processes, synthesizing new compounds, and analyzing chemical changes.

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Most popular questions from this chapter

Acetylsalicylic acid is the active ingredient in aspirin. It took \(35.17 \mathrm{mL}\) of \(0.5065 \mathrm{M}\) sodium hydroxide to react completely with \(3.210 \mathrm{g}\) of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?

Tris(pentafluorophenyl)borane, commonly known by its acronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of \(\mathrm{C}, \mathrm{F},\) and \(\mathrm{B} ;\) it is \(42.23 \%\) C and \(55.66 \%\) F by mass. a. What is the empirical formula of BARF? b. A \(2.251-\mathrm{g}\) sample of BARF dissolved in \(347.0 \mathrm{mL}\) of solution produces a 0.01267-M solution. What is the molecular formula of BARF?

A 10.00 -mL sample of vinegar, an aqueous solution of acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right),\) is titrated with \(0.5062 \mathrm{M} \mathrm{NaOH},\) and \(16.58 \mathrm{mL}\) is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is \(1.006 \mathrm{g} / \mathrm{cm}^{3},\) what is the mass percent of acetic acid in the vinegar?

Three students were asked to find the identity of the metal in a particular sulfate salt. They dissolved a 0.1472 -g sample of the salt in water and treated it with excess barium chloride, resulting in the precipitation of barium sulfate. After the precipitate had been filtered and dried, it weighed 0.2327 g. Each student analyzed the data independently and came to different conclusions. Pat decided that the metal was titanium. Chris thought it was sodium. Randy reported that it was gallium. What formula did each student assign to the sulfate salt? Look for information on the sulfates of gallium, sodium, and titanium in this text and reference books such as the \(C R C\) Handbook of Chemistry and Physics. What further tests would you suggest to determine which student is most likely correct?

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$ \begin{array}{c} \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) \\ \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g) \end{array} $$ A \(10.00-\mathrm{g}\) mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture is then reacted with \(156 \mathrm{mL}\) of \(3.00 \mathrm{M}\) silver nitrate to produce the maximum possible amount of silver chloride. a. Determine the percent magnesium by mass in the original mixture. b. If \(78.0 \mathrm{mL}\) of HCl was added, what was the concentration of the HCl?
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