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Chapter 4: Problem 32

Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (a) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{BaCO}_{3}\) (c) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) (d) \(\mathrm{Ca}(\mathrm{OH})_{2}\)

Short Answer

Expert verified
(a) Soluble, ions: \(NH_4^+, SO_4^{2-}\); (b) Insoluble; (c) Soluble, ions: \(Pb^{2+}, NO_3^-\); (d) Slightly soluble, ions: \(Ca^{2+}, OH^-\).

Step by step solution

01

Check Ammonium Sulfate

Use the solubility rules: Salts containing ammonium ions \((NH_4^+)\) and sulfate ions \((SO_4^{2-})\) are generally soluble. Therefore, ammonium sulfate \((NH_4)_2SO_4\) is soluble in water. The dissolution equation is \((NH_4)_2SO_4 (s) \rightarrow 2NH_4^+ (aq) + SO_4^{2-} (aq)\). The ions present in solution are \(NH_4^+\) and \(SO_4^{2-}\).
02

Check Barium Carbonate

Consult the solubility rules: Salts containing carbonate ions \((CO_3^{2-})\) are generally insoluble, with exceptions when paired with alkali metal ions or ammonium. \(BaCO_3\) does not meet these exceptions, hence it is insoluble in water. No dissolution occurs, so no ions are present in solution.
03

Check Lead Nitrate

According to solubility rules, nitrates \((NO_3^-)\) are always soluble regardless of the cation. \(Pb(NO_3)_2\) is thus soluble in water. The dissolution is \(Pb(NO_3)_2 (s) \rightarrow Pb^{2+} (aq) + 2NO_3^- (aq)\), forming \(Pb^{2+}\) and \(NO_3^-\) ions in solution.
04

Check Calcium Hydroxide

Solubility rules state that hydroxides are generally insoluble except when paired with alkali metals and a few alkaline earth metals. \(Ca(OH)_2\) is slightly soluble, meaning it will dissolve to some extent. The dissolution is \(Ca(OH)_2 (s) \rightarrow Ca^{2+} (aq) + 2OH^- (aq)\). In a saturated solution, \(Ca^{2+}\) and \(OH^-\) ions are present in limited quantity.

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Key Concepts

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

Ionic Compounds
Ionic compounds are fascinating chemical substances. They are formed when positive ions (cations) and negative ions (anions) attract each other to form a neutral compound.
These oppositely charged ions come from metal and non-metal elements.
  • Characteristics: Ionic compounds typically have high melting and boiling points because the ionic bonds are quite strong.
  • Solubility: Many ionic compounds are soluble in water, but this depends on the specific ions involved.
  • Electrical Conductivity: When dissolved in water, ionic compounds often conduct electricity due to the movement of ions.
Understanding ionic compounds helps in predicting the behavior of substances in chemical reactions and solutions.
Chemical Equations
Chemical equations are symbolic representations of chemical reactions. Each equation shows the reactants (starting substances) and the products (new substances formed). The key here is balance.
  • To be correct, a chemical equation must have the same number of each type of atom on both sides.
  • The state of each compound is noted, such as solid (s), liquid (l), gas (g), or aqueous (aq).
When an ionic compound dissolves in water, the equation represents how the compound splits into its constituent ions.
Ammonium Sulfate Solubility
Ammonium sulfate \((NH_4)_2SO_4\) is a good example of a soluble ionic compound. According to solubility rules:
  • Salts containing ammonium \(NH_4^+\) are generally soluble.
  • Sulfates \(SO_4^{2-}\) are also soluble, with some exceptions not including ammonium sulfate.
The dissolution equation for ammonium sulfate in water is:\[(NH_4)_2SO_4 (s) \rightarrow 2NH_4^+ (aq) + SO_4^{2-} (aq)\]This equation indicates the solution contains ammonium ions and sulfate ions, which can influence its properties.
Barium Carbonate Insolubility
Barium carbonate \(BaCO_3\) is mostly insoluble in water. The solubility rules provide insight:
  • Carbonate salts \(CO_3^{2-}\) are generally insoluble except for those involving alkali metals and ammonium. Barium does not fit these exceptions.
This means that barium carbonate does not dissolve, so it does not produce ions in a water solution. It often forms a solid precipitate.
Lead Nitrate Solubility
Lead nitrate \(Pb(NO_3)_2\) is quite soluble in water. This is because:
  • Nitrate ions \(NO_3^-\) are universally soluble, no matter which cation they are paired with.
This results in the dissolution of lead nitrate as:\[Pb(NO_3)_2 (s) \rightarrow Pb^{2+} (aq) + 2NO_3^- (aq)\]After dissolving, it creates a solution containing lead and nitrate ions.
Calcium Hydroxide Solubility
Calcium hydroxide \(Ca(OH)_2\) is a unique case as it is only slightly soluble in water. The solubility rules state:
  • Hydroxides \(OH^-\) are usually insoluble, with exceptions for some alkaline earth metals like calcium.
Thus, even with calcium, it only slightly dissolves:\[Ca(OH)_2 (s) \rightarrow Ca^{2+} (aq) + 2OH^- (aq)\]The presence of calcium and hydroxide ions is limited, which means its solubility is low but not negligible.

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Most popular questions from this chapter

Elemental bromine is the source of bromine compounds. The element is produced from certain brine solutions that occur naturally. These brines are essentially solutions of calcium bromide that, when treated with chlorine gas, yield bromine in a displacement reaction. What are the molecular equation and net ionic equation for the reaction? A solution containing \(40.0 \mathrm{~g}\) of calcium bromide requires \(14.2 \mathrm{~g}\) of chlorine to react completely with it, and \(22.2 \mathrm{~g}\) of calcium chloride is produced in addition to whatever bromine is obtained. How many grams of calcium bromide are required to produce 10.0 pounds of bromine?

A solution of hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\), is titrated with a solution of potassium permanganate, \(\mathrm{KMnO}_{4}\). The reaction is $$ \begin{array}{c} 5 \mathrm{H}_{2} \mathrm{O}_{2}(a q)+2 \mathrm{KMnO}_{4}(a q)+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \\ 5 \mathrm{O}_{2}(g)+2 \mathrm{MnSO}_{4}(a q)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+8 \mathrm{H}_{2} \mathrm{O}(l) \end{array} $$ It requires \(51.7 \mathrm{~mL}\) of \(0.145 \mathrm{M} \mathrm{KMnO}_{4}\) to titrate \(20.0 \mathrm{~g}\) of the solution of hydrogen peroxide. What is the mass percentage of \(\mathrm{H}_{2} \mathrm{O}_{2}\) in the solution?

Silver nitrate reacts with strontium chloride in an aqueous precipitation reaction. What are the formulas of silver nitrate and strontium chloride? Write the molecular equation and net ionic equation for the reaction. What are the names of the products? Give the molecular equation for another reaction that produces the same precipitate.

A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as barium sulfate, \(\mathrm{BaSO}_{4}\). How many grams of barium ion are in a 458 -mg sample of the barium compound if a solution of the sample gave \(513 \mathrm{mg} \mathrm{BaSO}_{4}\) precipitate? What is the mass percentage of barium in the compound?

If \(45.1 \mathrm{~mL}\) of a solution containing \(8.30 \mathrm{~g}\) of silver nitrate is added to \(31.3 \mathrm{~mL}\) of \(0.511 \mathrm{M}\) sodium carbonate solution, calculate the molarity of silver ion in the resulting solution. (Assume volumes are additive.)
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